Chemical Kinetics

The given reaction 2NO + $O_{2} - - > 2 N O_{2}$ is an example of (AIPMT/NEET 2001)
1. 1st order reaction
2. 2nd order reaction
3. 3rd order reaction
4. none of these
2A --> B=C . It would be zero -order reaction when (AIPMT/NEET 2001)
1. rate of reaction is proportional to square of conc of A
2. the rate of reaction remains same at any conc of A
3. the rate remains unchanged at any conc of B & C
4. rate of reaction doubles if conc of B is increased to double
For reaction, rate andrate constant are 1.02 X 10⁴ M/sec and 3.4X 10^-5 sec/M respectively , then concentration of dinitrogenpentaoxide is
(AIPMT/NEET 2001)
1. 1.732 M
2. 3M
3. 1.02 X M
4. 3.5 X M
An elementary reaction is given as 2P +Q --> products. If concentration of Q is kept constant and concentration of P is doubled then rate of reaction is
(AIPMT/NEET 2002)
1. doubled
2. halved
3. quadrupled
4. remains same
If the rate of the reaction is equal to the rate constant , the order of reaction is (AIPMT/NEET 2003)
1. 3
2. 0
3. 1
4. 2
Activation energy for a simple chemical reaction A --> B is E in forward direction . The activation energy for reverse reaction (AIPMT/NEET 2003)
1. is always double of Ea
2. is negative of E
3. is always less than E
4. can be less than or more than E
Rate constant and rate of reaction are same for (AIPMT/NEET 2003)
1. 1st order
2. 0 order
3. 2nd order
4. All are wrong
Which plots will give the value of activation energy ? (AIPMT/NEET 2003)
1. K vs T
2. 1/K vs T
3. ln K vs T
4. ln K vs 1/T
The reaction A --> B follows 1st order kinetics . The time taken for 0.8 mole of A to produce 0.6 mole of B is 1 hr. What is the time taken for conversion of 0.9 mole of A to produce 0.675 mole of B? (AIPMT/NEET 2003)
1. 1 hr
2. 0.5 hr
3. 0.25 hr
4. 2 hr
Rate of first order reaction is 0.015 M/min at 0.5 m concentration of reactant. The half life of reaction is (AIPMT/NEET 2004)
1. 0.383 min
2. 23.1 min
3. 8.73 min
4. 7.53 min
For first order reaction A-->B the reaction rate at reactant concentration of 0.10 M is found to be 2 X 10^-5 mol/L sec the half life period of the reaction is (AIPMT/NEET 2005)
1. 220 s
2. 30 s
3. 300 s
4. 347 s
Rate of reaction between 2 reactants A & B decreases by a factor of 4 if the concentration of reactant B is doubled . The order of this reaction wrt reactant B is (AIPMT/NEET 2005)
1. -1
2. -2
3. 1
4. 2
Which of the following does not express the reaction rate ?
2A --> B --> 3C --> D (AIPMT/NEET 2006)
1. d[D]/dt
2. -d[A]/2dt
3. -d[C]/3dt
4. -d[B]/dt
Equality relationship between ammonia and hydrogen is (AIPMT/NEET 2001)
1. d[ammonia]/dt = -3/2 d[Hydrogen]/dt
2. d[ammonia]/dt = - d[Hydrogen]/dt
3. d[ammonia]/dt= -1/3 d[Hydrogen]/dt
4. d[ammonia]/dt = -2/3 d[hydrogen] /dt
Reaction obey 1st order wrt hydrogen and ICl both
$H_{2} + 2 I C l - - > 2 H C l + I_{2}$
Which of the following mechanism is in consistent with the given fact ?
Mechanism A : $H_{2} + 2 I C l - - > 2 H C l + I_{2}$
Mechanism B : i (slow ) $H_{2} + I C l - - > H C l + H I$
ii . $H I + I C l - - > H C l + I_{2}$ (AIPMT/NEET 2007)
1. A & B
2. neither A nor B
3. A
4. B
In a first order reaction A --> B if k is the rateconstant and initial concentration of the reactant is 0.5 M , then half life is (AIPMT/NEET 2007)
1. ln 2/K
2. ln 2/K $\sqrt{0.5}$
3. log 2 /K
4. 0.693/0.5 K
If 60 % of first order reaction was completed in 60 min,50% of the same reaction would be completed in approximately (AIPMT/NEET 2007)
1. 45 min
2. 60 min
3. 40 min
4. 50 min
Rate constants $k_{1}$ and $k_{2}$ for 2 different reactions are $10^{16} e^{- 2000 / T}$ and $10^{15} e^{- 1000 / T}$ . temperature at which rate constant will be equal (AIPMT/NEET 2008)
1. 2000/2.303 K
2. 2000K
3. 1000/2.303 K
4. None of these
In the reaction
$B r O^{3 -} + 6 H^{+} + 5 B r^{-} - - > 3 B r_{2} + 3 H_{2} O$ . The rate of appearance of bromine is related to rate of disappearance of bromide ions as followings (AIPMT/NEET 2009)
1. $d [B r_{2}] / d t$ = 3/5 $d [B r^{-}] / d t$
2. $d [B r_{2}] / d t$ = -3/5 $d [B r^{-}] / d t$
3. $d [B r_{2}] / d t$ = -5/3 $d [B r^{-}] / d t$
4. None of these
For the reaction A + B products , it is observed that
1)on doubling the initial concentration of A only, the rate of reaction is also doubled
2) doubling initial concentration of both A & B , there is a change by factor of 8 in the rate of reaction
Rate of this reaction is given by (AIPMT/NEET 2009)
1. rate = k [A] [B]
2. rate = k $[A]^{2}$ [B]
3. rate = k [A] $[B]^{2}$
4. rate = k $[A]^{2}$
  $[B]^{2}$
For the reaction $N_{2} + 3 H_{2} - - > 2 N H_{3}$ , if d[ammonia]/dt = 2X $10^{- 4}$ mol/l sec , the value of -d[hydrogen ] /dt would be (AIPMT/NEET 2009)
1. $10^{- 4}$ mol/L sec
2. 3 X $10^{- 4}$ mol /L sec
3. 4 X $10^{- 4}$ mol/L sec
4. 6 X $10^{- 4}$ mol/L sec
Half period of 1st order reaction is 1386 sec. Specific rate constant of the reaction is (AIPMT/NEET 2009)
1. 5X $10^{- 2}$ /sec
2. 5 X $10^{- 3}$ /sec
3. 0.5 X $10^{- 2}$ /sec
4. 0.5 X $10^{- 3}$ /sec
For an endothermic reaction energy of activation is E and enthalpy of reaction is $∆ H$ .Minimum value of E(AIPMT/NEET 2010)
1. < $∆ H$
2. = $∆ H$
3. > $∆ H$
4. =0
Rate of reaction
$2 N O + C l_{2} - - > 2 N O C l$ is given by rate, equation rate = k $[N O]_{2} [C l_{2}]$ . the value of rate constant can be increased by (AIPMT/NEET 2010)
1. increasing the temperature
2. increasing concentration of NO
3. increasing concentration of chlorine
4. doing all these
For the reaction $N_{2} O_{5} - - > 2 N O_{2} + 1 / 2 O_{2}$ , the rate of disappearance of dinitrogenpentaoxide is 6.25 X $10^{- 3}$ mol/L sec. The rate of formation of nitrogen oxide and oxygen will be(AIPMT/NEET 2010)
1. 6.25 X $10^{- 3}$ mol/L sec & 6.25 X $10^{- 3}$ mol/L sec
2. 1.25 X $10^{- 2}$ mol/L sec & 3.125 X $10^{- 3}$ mol/L sec
3. 6.25 X $10^{- 3}$ mol/L sec & 3.125 X $10^{- 3}$ mol/L sec
4. 1.25 X $10^{- 3}$ mol/L sec & 6.25 X $10^{- 3}$ mol/L sec
During the kinetic study of the reaction 2A + B -->C + D following results were obtained
[A] in M [B] in M Initial rate of formation of D in m/s
I 0.1 0.1 0.006
II 0.3 0.2 0.072
III 0.3 0.4 0.288
IV 0.4 0.1 0.024(AIPMT/NEET2001)
1. Rate = k $[A]^{2}$ [B]
2. Rate = k[A] [B]
3. Rate = k $[A]^{2}$ $[B]^{2}$
4. Rate = k [A] $[B]^{2}$
Which one of the following statements for the order of the reaction is incorrect ?(AIPMT/NEET2011)
1. Order of the reaction is always a whole number
2. Order can be determined only experimentally
3. order is not influenced by stoichometric coefficient of reacatants
4. order of reactions is sum of power to the concentration terms of reactants to express the rate of reaction
For the reaction $N_{2} + O_{2} - - > 2 N O$ , the equilibrium constant is $K_{1}$ .The equlibrium constant is $K_{2}$ for the reaction $2 N O + O_{2} - - > 2 N O_{2}$
What is the K of the reaction $2 N O_{2} - - > 1 / 2 N_{2} + O_{2}$ (AIPMT/NEET2011)
1. 1/(2K1K2)
2. 1/(4K1K2)
3. [1/(K1K2)]1/2
4. 1/(K1K2)
The rate of the reaction $2 N_{2} O_{5} - - > 4 N O_{2} + O_{2}$ can be written in 3 ways
$- \frac{d [N_{2} O_{5}]}{d t} = k [N_{2} O_{5}]$
$\frac{d [N O_{2}]}{d t} = k' [N O_{2}]$
$\frac{d [O_{2}]}{d t} = k'' [O_{2}]$
Relationship of k & k' and k & k '' is
(AIPMT/NEET 2011)
1. k'=2k , k'=k
2. k'=2k , k''=k
3. k'=2k , k"=2k
4. k'=k , k'=k
In a zero order reaction for every 10 rise of temperature the rate is doubled . If the temperature is increased from 10 C to 100 C , the rate of reaction will be (AIPMT/NEET 2012)
1. 64 times
2. 512 times
3. 256 times
4. 128times
In a reaction A + B --> product , rate is doubled when the concentration of B is doubled and rate oncreases by a factor of 8when the concentration of both the reactants (A & B ) are doubled , rate law for the reaction can be written as (AIPMT/NEET 2012)
1. Rate = k $[A]^{2}$ [B]
2. Rate = k[A] [B]
3. Rate = k [A] $[B]^{2}$
4. Rate = k $[A]^{2}$ $[B]^{2}$
Activation energy (E) and rate constant of a chemical reaction at two different temepratures are related by (AIPMT/NEET 2012)
1. $\ln \frac{k_{2}}{k_{1}}$ = - $\frac{E_{a}}{R} (\frac{1}{T_{1}} - \frac{1}{T_{2}})$
2. $\ln \frac{k_{2}}{k_{1}}$ = $\frac{E_{a}}{R} (\frac{1}{T_{1}} - \frac{1}{T_{2}})$
3. $\ln \frac{k_{2}}{k_{1}}$ = $\frac{E_{a}}{R} (\frac{1}{T_{1}} + \frac{1}{T_{2}})$
4. $\ln \frac{k_{2}}{k_{1}}$ = $\frac{E_{a}}{R} (\frac{1}{T_{1}} - \frac{1}{T_{2}})$
What is activation energy for a reaction if its rate double when temperature is rasied from 20 C to 35 C?(R= 8.314 J/mol K) (AIPMT/NEET 2013)
1. 269 kJ/mol
2. 34.7 kJ/mol
3. 15.1 kJ/mol
4. 342 kJ/mol
A reaction having equal energies of activation for forward and reverse reaction has (AIPMT/NEET 2013)
1. $∆$ G = 0
2. $∆$ H=0
3. $∆$ H = $∆$ G = $∆$ S =0
4. $∆$ S= 0
Activation energy of a reaction can be determined from slope of which of the following graphs ? (AIPMT/NEET 2015)
1. ln k vs 1/T
2. T/ln k vs 1/T
3. lnk vs T
4. ln k /T vs T
When initial concetration of a reactant is doubled in a reaction , its half life period is not affected . The order of the reaction is (AIPMT/NEET 2015)
1. 2nd
2. more than 0 but less than 1
3. 0
4. 1st
Rate constant of the reaction A-->B is 0.00006 mole per second. If concentration of A is 5 M, then concentration of B after 20 minutes is (AIPMT/NEET 2015 Re )
1. 0.36 M
2. 0.72 M
3. 1.08 M
4. 3.60 M
The addition of a catalyst during a chemical reaction alters which of the following quantities ? (AIPMT/NEET 2016 Phase I)
1. Activation energy
2. Entropy
3. Internal energy
4. Enthalpy
The rate of first order reaction is 0.04 mol/Lsec at 10 seconds and 0.03 mol/Lsec at 20 secnds after initiation of the reaction. The half life period of the reaction is (AIPMT/NEET 2016 Phase I)
1. 54.1 s
2. 24.1 s
3. 34.1 s
4. 44.1 s
If doubling the concentration of a reactant A increases the rate 4 times and tripling the concentration of A increases the rate 9 times , the rate is proportional to (AIIMS 2001)
1. concentration of A
2. square of concentration of A
3. under root of concentration of A
4. cube concentration of A
A gaseous hypothetical chemical equatin 2A--> 4B +C is carried out in a closed vessel. Concentration of B is found to increase by 0.005 mol/L in 10 sec. Rste of appearance of B is (AIIMS 2002)
1. 5 X $10^{- 4}$ mol/L sec
2. 5 X $10^{- 5}$ mol/L sec
3. 6 X $10^{- 4}$ mol/L sec
4. 4X $10^{- 4}$ mol/L sec
For reaction $N_{2} O_{5} - - > 2 N O_{2} + 1 / 2 O_{2}$ is first order in diNitrogenpentaoxide with rate cosntant 0.62 /sec . Rate of reaction is
(AIIMS 2003 )
1. 7.75 X $10^{- 1}$ mol/L sec
2. 6.35 X $10^{- 3}$ mol/L sec
3. 5.15 X $10^{- 5}$ mol/L sec
4. 3.85 X $10^{- 1}$ mol/L sec
If concentration is expressed in moles per litre, the unit of rate constant for the first order reaction is (AIIMS 2004)
1. mole/L sec
2. mole/ L
3. /second
4. /mol L second
Which of the following rate laws has an overall order of 0.5 for reaction involving substance x, y & z ?(AIIMS 2005)
1. Rate= k $(C_{X}) (C_{Z}) (C_{y})$
2. Rate= k $(C_{X})^{0.5} (C_{Z})^{0.5} (C_{y})^{0.5}$
3. Rate= k $(C_{X})^{1.5} (C_{Z})^{0} (C_{y})^{- 1}$
4. Rate= k $(C_{X}) (C_{Z})^{n} / (C_{y})$
For chemical reaction A --> B it is found that rate of reaction doubles when the concentration of A is increased 4 times. Order in A for this reaction is(AIIMS 2005)
1. 2
2. 1
3. 1/2
4. 0
Inversion of cane sugar us repesneted by
$C_{11} H_{22} O_{12} + H_{2} O - - > 2 C_{6} H_{12} O_{6}$
it is reaction of
(AIIMS 2006)
1. bimolecular
2. unimolecular
3. pseudo unimolecular
4. None of these
A first order reaction which is 30% complete in 30 min has a half life of (AIIMS 2007)
1. 24.2 min
2. 58.2 min
3. 102.2 min
4. 120.2 min
For the reaction Hydrogen + Chlorine --> 2HCl . Order of reaction is (AIIMS 2008)
1. 8
2. 21
3. 3
4. 0
Rate constant of reaction is 0.069 and initial concentration is 0.2 mol/L . Half life period is (AIIMS 2009)
1. 400 sec
2. 600 sec
3. 800 sec
4. 1200 sec
Rate constant of a first order reaction is 3 X 10 ^-6 per second. If the initial concetration is 0.10 M , the initial rate of reaction is (AIIMS 2010)
1. 3 X 10^-5 m/s
2. 3 X 10^-6 m/s
3. 3 X 10^-4 m/s
4. 3 X 10^-7 m/s
A first-order reaction is half completed in 45 mins.how long does it need 99.9% of the reaction to be completed (AIIMS 2011)
1. 5hrs
2. 7.5 hrs
3. 10 hrs
4. 20 hrs
A substance A decomposes by first order reaction starting initially with [A] = 2 m and after 200 min [A] =0.15 m , For this reaction k is (AIIMS 2012)
1. 0.0129 /min
2. 0.0229 /min
3. 0.0329 /min
4. 0.0440 /min
For a reaction A --> xP when [A] =2.2 m , the rate was found to be 2.4 nM/sec. On reducing concentration of A to half, the rate changes to 0.05 nM/sec . The order of reaction wrt A is (AIIMS 2012)
1. 1.5
2. 2
3. 2.5
4. 3
If a substance with half life 3 days is taken at other place in 12 days. Amount left is (Aiims 2014)
1. 1/4
2. 1/8
3. 1/16
4. 1/32
An endothermic reaction with high activation energy for forward is given by
(AIIMS 2014)
Rate constant k, for the reaction $N_{2} O_{5} - - > N O_{2} + 1 / 2 O_{2}$ is 0.23 /sec . Which equation given below describes of [dinitrogen pentaoxide] with time ?
1. $[N_{2} O_{5}]$ = $[N_{2} O_{5}]_{0}$ + kt
2. $[N_{2} O_{5}]$ = $[N_{2} O_{5}]_{t}$
3. log $[N_{2} O_{5}]_{t}$ =log $[N_{2} O_{5}]_{0}$ - kt
4. log $[N_{2} O_{5}]_{0}$ / $[N_{2} O_{5}]_{t}$ = kt
Assertion: instantaneous rate off reaction can be studied in chemical kinetics
Reason: ionic reactions occur instantaneously
(AIIMS 2011)
1. both the assertion and reason are true andd reason is true explaination of assertion
2. both the assertion and reason are true and reason is not correct explaination of assertion
3. the assertion is true but reason is false
4. assertion is false but reason is true
Assertion : Acid hydrolysis of ester takes place more rapidly in didetriumoxide than water
Reason: D3O+ is stronger acid than hydronium ion
(AIIMS 2012)
1. both the assertion and reason are true and reason is true explaination of assertion
2. both the assertion and reason are true ans reason is not correct explaination of assertion
3. the assertion is true but reason is false
4. assertion is false but reason is true
Assertion: Photosynthesis in plants involves reaction of carbon-di-oxide & water in presence of light & chlorophyll
Reason: It is chlorophyll which absorbs light & passes this energy to reactant molecules (AIIMS 2013)
1. both the assertion and reason are true and reason is true explaination of assertion
2. both the assertion and reason are true and reason is not correct explaination of assertion
3. the assertion is true but reason is false
4. assertion is false but reason is true
Assertion : Order of reaction can never be fractional for elementary reaction
Reason : An elementary reaction takes lace by one step mechanism (AIIMS 2014)
1. both the assertion and reason are true and reason is true explaination of assertion
2. both the assertion and reason are true and reason is not correct explaination of assertion
3. the assertion is true but reason is false
4. assertion is false but reason is true
Assertion : The emission of light during burning of P in oxygen is called chemiluminescence
Reason : Chemical energy is converted into light energy
(AIIMS 2015)
1. both the assertion and reason are true and reason is true explaination of assertion
2. both the assertion and reason are true and reason is not correct explaination of asasertion
3. the assertion is true but reason is false
4. assertion is false but reason is true
Assertion : photochemical reactions Hydrogen + chlorine --> 2HCl , and hydrogen + bromine --> 2HBr have equal quantum efficiencies
Reason : both the reactions proceed by different mechanism
1. both the assertion and reason are true and reason is true explaination of assertion
2. both the assertion and reason are true and reason is not correct explaination of asasertion
3. the assertion is true but reason is false
4. assertion is false but reason is true
Assertion : Half-life period of a reaction of first order is independent of initial concentration
Reason : Half life period for first order reaction is t=2.303/k (log2)
1. both the assertion and reason are true and reason is true explaination of assertion
2. both the assertion and reason are true ans reason is not correct explaination of asasertion
3. the assertion is true but reason is false
4. assertion is false but reason is true
Assertion : Glow worm shows chemiluminescence
Reason : Glow worm emits light due to oxidation of protein , luciferin present in it
1. both the assertion and reason are true ans reason is true explaination of assertion
2. both the assertion and reason are true ans reason is not correct explaination of asasertion
3. the assertion is true but reason is false
4. assertion is false but reason is true
If a second order reaction involving a single reactant in 25% complete 20 mins then what is its half life if initial concentration of the reactant is being made double at same temperature
1. 50 min
2. 30 min
3. 60 min
4. 15 min
On introducing a catalyst at 500K at the rate of first order reaction increases by 1.718 times. The activation energy in presnece of catalyst is 4.15kJ/mol . The slope of plot of ln k (/sec ) versus 1/T (in K) in absence of catalyst is
1. +1
2. -1
3. +1000
4. -1000
Arrhenius equation for trans isomerisation of 2-butene and 2-butene nitrile are given as follows
a. for 2-butene K(S-1) = 10 ^13.8
b. for 2-butene nitrile K'(S-1) = 10^11
Temperature at which K=K' is
1. 913.87K
2. 533.43 K
3. 1000.02 K
4. 407.05 K
Thermal decomposition of a compound is of 1st order. If 50% of a sample of the compound is dcomposed in 120 minutes, how long will it take for 90% of the compound to decompose ?
1. 399 min
2. 410 min
3. 250 min
4. 120 min
The decomposition of dichloroheptaoxide at 400K in the gas phase to chlorine and oxygen is first order .After 55 seconds at 400 K the pressure of dichloroheptaoxide falls from 0.062 to 0.044 atm. Rate constant and pressure of dichloroheptaoxide after 100 sec of decomposition at this temperature are
1. 5.2 X 10^-4 /sec ; 0.05 atm
2. 6.2X 10^-3 /sec , 0.033 atm
3. 5.8X 10^-3 /sec , 0.44 atm
4. 4.6X 10^-3 /sec , 0.033 atm
A substance having half life period of 30 minutes decomposed according to the first order rate law . The fraction decomposed , the balance remaining after 1.5 hours and time for 60% decomposition on its doubling the initiail concentration will be
1. 87.4; 0.126 ; 39.7 min
2. 80.6; 0.135; 40.8 min
3. 90.5; 0.144; 2829 min
4. 80.2 ; 0.135 ; 26.6 min
In the Arrhenius eqaution for a certain reaction the value of A and E are 4 X10 ^13 /sec and 98.6 kJ/mol . If the reaction is first order , the temperature at which its half life period is 10 minutes is
1. 280 K
2. 290 K
3. 311.35K
4. 418.26 K
First order reaction is 50 % complete in 30 minutes at 27 C and in 10 minutes at 47 C . The rate constant at 47 C and energy of activation of reaction in kJ/mole will be
1. 0.0693 , 43.848 kJ/mol
2. 0.0560 ; 45.621 kJ/mol
3. 0.0625 ; 42.926 kJ/mol
4. 0.0660 ; 46.189 kJ/mol
75 % of first order reaction was completed in 32 minutes . When was 50 % of the reaction completed
1. 24 min
2. 4 min
3. 16 min
4. 8 min
Fraction of X (half life = 25 min ) left after 100 minutes
1. 1/3
2. 1/4
3. 1/2
4. 1/16
Activation energy of decomposition of dinitropentaoxide is (when rate constants are 3.45 X 10 ^-5 and 6.9 X 10 ^-3 at 27 C and 67 C respectively )
1. 10200 kJ
2. 488.5kJ
3. 112kJ
4. 14.7 kJ
50 % of the amount of a radioactive substance decomposes in 5 years . Time required for decomposition of 99.9 % of substance will be
1. 10 years
2. between 10 & 50 years
3. less than 10 years
4. between 49 & 50 years
1.386 hours are required for disappearance of 75% of reactant of first order reaction . What is rate constant of reaction?
1. 3.6 X $10^{- 3}$ /sec
2. 7.2 X $10^{- 3}$ /sec
3. 2.7 X $10^{- 4}$ /sec
4. 1.8 X $10^{- 3}$ /sec
For a first order reaction , the ratio of time for the completion of 99.9% and half of the reaction is
1. 8
2. 10
3. 11
4. 12
For first order reaction A--> 2B + C the initial pressure is Pa= 90 mmHg , the pressure after 10 minutes is found to be 180 mmHg .Rate constant of reaction is
1. 1.15 $10^{- 3} s e c^{- 1}$
2. 3.45 X $10^{- 3} s e c^{- 1}$
3. 2.3 X $10^{- 3} s e c^{- 1}$
4. 6 X $10^{- 3}$ /sec
The rate law of the reaction RCl + NaOH --> ROH + HCl is given by rate = k[RCl] . The rate of the reaction will be
1. unaffected on doubling the concentration of NaOH
2. doubled on doubling the concetration of NaOH
3. halved on reducing the concentration of NaOH to 1/2
4. halved on reducing the concentration of RCl to 1/2
For a given reaction of first order , it takes 20 minutes for concentration to drop from 1 nol/litre to 0.6 mol/litre . The time required for concentration to drop from 0.6 mol/litre to to 0.36 mol/litre will be
1. more than 20 minutes
2. less than 20 minutes
3. equal to 20 minutes
4. infinity
Unit of rate constant of a reaction having order 1.5 would be
1. $(m o l L^{- 1})^{- 1 / 2} t i m e^{- 1}$
2. $(m o l L^{- 1})^{- 3 / 2} t i m e^{- 1}$
3. $(c o n c)^{- 0.5} t i m e^{- 1}$
4. $(c o n c)^{- 0.75} t i m e^{- 1}$
The half life period of radioactive element is 140 days. After 560 days , one gram of the element will reduce to
1. 1/2 g
2. 1/4 g
3. 1/8 g
4. 1/16 g
In a reaction , the concetration of reactant is increased two times and three times then the increased in rate of reaction were 4 times and 9 times respectively, order of reaction is
1. 0
2. 1
3. 2
4. 3
In a first order reaction , the concentration of the reactant ,decreases from 0.8 M to 0.4 M in 15 minutes. The time taken for concentration to change from 0.1 M to 0.025 M is
1. 7.5 minutes
2. 15 minutes
3. 30 minutes
4. 60 minutes
Half life of 2 sample are 0.1 and 0.4 seconds . There respective concetration are 200 and 50 respectively . Order of reaction is
1. 0
2. 2
3. 1
4. 4
Rate constant is doubled when temperature increases from 27 C to 37 C . Activation energy is
1. 34
2. 54
3. 100
4. 50
For a reaction X --> Y + Z the half life period is 10 minute. In what period of time would the concetration of X be reduced to 10% of original concentration
1. 20 min
2. 33 min
3. 15 min
4. 25 min
For endothermic change, where enthalpy change of reaction in kJ/mole, the minimum value for energy of activation will be
1. Less than enthalpy change
2. 0
3. More than enthalpy change
4. eqaul to enthalpy change
Rate constant activation energy and Arrhenius parameter of chemical reaction at 25 C are 3X $10^{-4}$ /sec. 1044kJ/mol and 6 X $10^{14}$ /sec . Rate constant as t is infinity is
1. 2 X $10^{18}$ / sec
2. 6.0 X $10^{14}$ /sec
3. infinity
4. 3.6 X $10^{30}$ /sec
Rate law for a gaseous reaction A + B --> C+ D Rate = k[A]^2 . Volumes of reaction vessel containing these gases is suddenly reduced to 1/4 th initial volume . Rate of reaction relative to original rate would be
1. 1/16
2. 16/1
3. 1/8
4. 8/1
In the reaction $2 N_{2} O_{5} - - > 4 N O_{2} + O_{2}$ initial pressure is 500 atm and rate constant K is 3.38 X 10 ^ -5 /sec. After 10 minutes final pressure of dinitropentaoxide is
1. 490 atm
2. 250 atm
3. 480 atm
4. 420 atm
For the reaction $H_{2} + B r_{2} - - > 2 H B r$ expermental data suggested r=k[H2][Br2]^1/2 . The molecularity and order of the reaction are
1. 2, 3/2
2. 3/2 , 3/2
3. not defined , 3/2
4. 1,1/2
The reaction $2 N a + C l_{2} - - > 2 N a C l$ is found to follow 3rd order kinetics . Its molecularity is
1. 1
2. 2
3. 3
4. 4
An example of Pseudo unimolecular reaction is
1. Dissociation of HI
2. Hydrolysis of methyl acetate in dil solution
3. Dissociation of phosphrous pentachloride
4. Decomposition of hydrogen peroxide
Diazonium salt decomposes . At ) C , the evolution of Nitrogen becomes 2 times faster when the initial concetration of salt is doubled ,therefore it is
1. 1st order reaction
2. 2nd order reaction
3. independent of initial concetration
4. zero order reaction
Reaction $2 F e C l_{3} + S n C l_{2} - - > 2 F e C l_{2} + S n C l_{4}$ is an example of
1. 1st order reaction
2. 2nd order reaction
3. 3rd order reaction
4. none of these
Inversion of cane sugar in dilute acid is a
1. unimolecular reaction
2. Bimolecular reaction
3. Trimolecular reaction
4. Pseudo unimolecular reaction
Rate constant of reaction is found to be 0.003 mol / Lmin . The order of reaction
1. 0
2. 1
3. 2
4. 1.5
For reaction RX + OH --> ROX + X , rate expression is R+ 4.7 X $10^{- 5}$ [RX] [OH] + 2.4 X $10^{- 5}$ [RX]
% of react by Sn2 mechanism when [OH]= 0.001 M
1. 1.9
2. 66.2
3. 95.1
4. 16.4
For an elementary reaction 2A + B--> C+D , the molecularity is
1. 0
2. 1
3. 2
4. 3
Reaction involving 2 different reactants can never be
1. unimolecular reaction
2. I order reaction
3. II order reaction
4. Bimolecular reaction
For hypothetical reaction aA + bB --> prodcut , rate law is r= K $[A]^{x} [B]^{y}$ then
1. (a+b) = (x+y)
2. (a+b) < (x+y)
3. (a+b) >(x+y)
4. All of these
From the following which is a second order reaction
1. K = 0.054 /sec
2. k = 0.0039 mol L /sec
3. K= 0.000394 L / mol sec
4. K= 0.0000398 Lsec /Mol
For rate constant is numerically same for three reactions of 1sr , 2nd & 3rd respectively . Which is correct?
1. if [A] =1 then r1=r2=r3
2. if [A] < 1 then r1 >r2>r3
3. if [A] >1 then r3 >r2>r1
4. All of these
Reaction was found to be 2nd order wrt concentration CO. If the concentration of CO is doubled , with everything else kept the same , the rate of reaction will
1. double
2. remain unchanged
3. triple
4. increase by factor 4
For gaseous reaction , following data is given
A--> B $k_{1} = 10^{15} e^{- 2000 / T}$
C--> D $k_{2} = 10^{14} e^{- 1000 / T}$

The temperature at which $k_{1} = k_{2}$ is
1. 1000 K
2. 2000 K
3. 868.82 K
4. 434.2 K
$T h e r e i s f o r m a t i o n o f H_{2} O_{2} a s H_{2} O + O - - > 2 O H - - > H_{2} O_{2} ∆ H = 72 k J / m o l a n d E = 77 k J / m o l . E a w i l l b e$
1. 149 kJ/mol
2. -149 kJ/mol
3. 5kJ/mol
4. -5kJ/mol
Conversion of A--> B follows second order kinetics . Doubling concentration of A will increase the rate of formation of B by a factor
1. 1/4
2. 2
3. 1/2
4. 4
Rate constant of a reaction with virus is 0.00031 /second . Time required for a virus to become 75% inactivated is
1. 17.5 min
2. 40 min
3. 74.5 min
4. 41 min
Consider reaction 2A + B --> Products .When concentration of B alobe doubled , the half life didnot change . When the concentration of A alone was doubled , rate increased 2 times . Unit of rate constant for this reaction is
1. L /mol sec
2. no unit
3. mol/L sec
4. /second
For reaction A--> xP when [A] =2.2 mM , the rate was found to be 2.4 mM/sec On redcuing concentration of A to half , the rate changes to 0.6mM/sec. The order of reaction wrt A is
1. 1.5
2. 2
3. 2.5
4. 3
Reaction $2 N_{2} O_{5} - - > 4 N O_{2} + O_{2}$ follows 1st order kinetics . Hence , molecularity of the reaction is
1. unimolecular
2. Pseudo unimolecular
3. Bimolecular
4. none of the above
For reaction pA + pB--> prodcuts , rate law expression is r= l $[A]^{l} [B]^{m}$ then
1. (p+l)< (l+m)
2. (p+q) > (l+m)
3. (p+q) may or may not be equal to (l+m)
4. (p+q) =(l+m)
Reaction $2 N O + O_{2} - - > 2 N O_{2}$ is of first order
If volume of reaction vessel is reduced to 1/3, the rate of reaction would be
1. 1/3 times
2. 2/3 times
3. 3 times
4. 6 times
Which is wrongly match ?
1. saponification of methylmethanote -bimolecular reaction
2. Hydrolysis methylmethanote -psuedo unimolecular reaction
3. decomposition of hydrogen peroxide - 1st order
4. Combination of hydrogen and bromine to form HBr - zero order
In a reaction 2A + B --> $A_{2} B$ reactant A will disappear at
1. half the rate that B will decrease
2. the same rate that B will decrease
3. twice the rate that B will decrease
4. same rate product will form
For a reaction 2A + B --> prodcuts , doubling the initial concentration of both the reactants increases the rate by as factor of 8 , and doubling the concentration of B alone doubles the rate. The rate law for the reaction is
1. r = k[A] $[b]^{2}$
2. r = k $[A]^{2}$ [B]
3. r = k [A] [B]
4. r = k $[A]^{2}$ $[B]^{2}$
Reaction X + 2Y + Z --> N occurs by following mechanism
1. X + Y --> M (rapid )
2. M + Z --> O (slow )
3. O + Y --> N (very fast0
Rate law is
1. rate = k[Z]
2. rate = k [X] [Y]
3. rate = k[N]
4. rate = k[X] [Y][Z]
Hypothetical reaction $A_{2} + B_{2} - - > 2 A B$ follows mechanism as given below
$A_{2}$ -->A + A (fast )
A + $B_{2}$ --> AB + B (slow )
A + B --> AB
order of overall reaction will be
1. 2
2. 1
3. 3/2
4. 0
Mechanism of reaction A +2B + C --> D is
step 1 (fast ) A + B --> X
step 2 (slow ) X + C --> Y
step 3 (fast ) Y + B --> D
rate law is
1. v= k [C]
2. v= [A] [C]
3. v= k[A] [B] [C]
4. v=k [D]
Catalyst decomposition of Hydrogen peroxide is a ___ order reaction
1. 1st
2. 2nd
3. 3rd
4. zero
In the reaction $N H_{4} N O_{2} - - > N_{2} + 2 H_{2} O$ volume of nitrogen after 20 min and after a long time is 40 mL and 70 mL . Value of rate constant is
1. 1/20 ln (7/4) /min
2. (2.303/1200) log (7/3) /sec
3. 1/20 ln (7/3) /min
4. (2.303/20) log (7/3) /sec
Half life of decomposition of dinitrogenpentaoxide is first order . After 15 minutes volume of oxygen produced is 9Ml and at end of the reaction 35 m L . Rate constant is
1. 1/15 log 35/26
2. 1/15 log 44/26
3. 1/15 log 35/36
4. none of these
Giventhat temperautre coefficient for saponification of ethyl acetate by NaOH is 1.75 . Activation energy is
1. 10.7 kcal /mol
2. 12.7 kcal/mol
3. 14.7 kcal /mol
4. 16.7 kcal / mool
Reaction takes place in 3 steps . Rate constants are k1, k2 & k3 . Overall rate constant k = (k1) (k2) / k3 . If E1 , E2 & e3 are 60 kJ , 30 kJ and 10 kJ . Overall energy of activation is
1. 40kJ/mol
2. 30
3. 400
4. 60
How faster would reaction proceed at 25 C than 0 C if the activation energy is 65 kJ ?
1. 2 times
2. 5 times
3. 11 times
4. 16 times
by increasin the temperature by 10 C , the rate of forward reaction at equailibrium by a factor of 2 . Rate of backward reaction by this increase in temperature
1. remains unaffected
2. increases by a factor greater than 2
3. decreases by a factor greater than 2
4. is also increased by a factor of 2
Distribution of molecular kinetic energy at 2 temeprature is as shown in the following graph

Which Conclusion are correct ?
1. The number of molecules with energy Ea or greater is proportional to shaded area for each temperature
2. The number of molecules with energy Ea or lesser is proportional to shaded area for each temperature
3. number of molecukes with energy Ea is the mean of all temperatures
4. Graph is not according to Maxwell Boltzmann energy distribution law
Rate of a reaction gets doubled when the temperature changes from 7 C to 17 C. By factor of what will it change when temeprature will change from 17 C to 27 C ?
1. 1.81
2. 1.71
3. 1.91
4. 1.76
un a reaction , the threshold energy is equal to
1. Activation energy +normal energy of reactants
2. Activation energy -normal energy of reactants
3. Activation energy
4. none of these
Following data are for the decomposition of ammonium nitrate in aq solution
Volume of nitrogen(in cc) time (min)
6.25 10
9.50 15
11.42 20
13.65 25
35.05 finally
Order of reaction
1. 0
2. 1
3. 2
4. 3
Differential rate law for reaction
$H_{2} + I_{2} - - > 2 H I$ is
1. - $\frac{d [H_{2}]}{d t}$ = - $\frac{d [I_{2}]}{d t}$ = - $\frac{d [H I]}{d t}$
2. $\frac{d [H_{2}]}{d t}$ = $\frac{d [I_{2}]}{d t}$ = $\frac{d [H I]}{d t}$
3. 1/2 $\frac{d [H_{2}]}{d t}$ = 1/2 $\frac{d [I_{2}]}{d t}$ =- $\frac{d [H I]}{d t}$
4. -2 $\frac{d [H_{2}]}{d t}$ = -2 $\frac{d [I_{2}]}{d t}$ = $\frac{d [H I]}{d t}$
For a reaction E= 0 and k = 32000 /sec at 300 K . The value of k 310 kwould be
1. 64000
2. 32000
3. 3200
4. 320000
Mechanism of the reaction
$2 N O + C l_{2} - - > 2 N O C l 1 . 2 N O - - > (N O)_{2} 2 . (N O)_{2} + C l_{2} - - > N O C l$
rate equation would be
1. kK [nitric oxide] [chlorine]
2. kK[nitrogen monoxide] ^2 [chlorine]
3. kK [chlorine]
4. kK[nitrogen monoxide] [chlorine]
Acid catalysed ionisation of hydroxy butyric acid proceeeds as a reversible reaction. Which is I order in both forward and backward steps
$A \overset{\leftrightarrow}{} B$
Rate -d[A]/dt is given by
1. K1 [A]
2. -K2[B]
3. K1 [A]- K2[B]
4. K1 [A]/K2[B]
2 reaction A --> products and B--> products have rate constant ka and kb at temperature T and activation energies are Ea and Eb . If ka > kb and Ea < Eb
1. on increasing temperature ka will be greater than kb
2. at lower temperature ka and kb will differ more
3. as temeprature rises ka and kb will close to each other
4. all of these
half life of a reaction was doubled when initial concentration was doubled. Order of reaction is
1. 3
2. 0
3. 1
4. 2
For decomposition HI at 1000K
the following data was obtained
[HI] . M Rate of decomposition of HI
0.1 2.75 X $10^{- 8}$
0.2 11 X $10^{- 8}$
0.3 24.75 X $10^{- 8}$
order of reaction is
1. 1
2. 2
3. 0
4. 1.5
For a reaction dx/dt = K[H]. If pH of reaction medium changes from 2 to 1 rate becomes 100 times of value at pH = 2
Order of reaction is
1. 1
2. 2
3. 0
4. 3
for formation of NOCl, when concentration of chlorine is doubled , the rate of reaction becomes 2 times of the original . When concetnration of NO is doubled the rate becomes 4 times. Order of reaction is
1. 1
2. 2
3. 3
4. 4
For 1st order reaction T average reaction , T 50 (half life ) and T (75 % reaction ) are in ratio of
1. 1.44 :3:2
2. 1.44 :1:2
3. 1:2:1.44
4. 1:2:3
For reaction A + B --> C it is found that doubling the concentration of A increases the rate by 4 times , and doubling concentration of B doubles reaction rate . Overall order of reaction
1. 4
2. 3/2
3. 3
4. 1
nA --> products
dx/dt = k[A]^n
for reaction , rate constant and rate of reaction are eqaul , them on doubling the concentration of A , rate becomes
1. 4 times
2. halved
3. constant
4. double
Number of natural life times required for a first order reaction to acheive 99.9% level of completion is
1. 6.9
2. 1.5
3. 0.105
4. 9.2
A +B -> Prodcut . dx/dt = k[A]^ a [B]^b
if dx/dt = k then order is
1. 4
2. 2
3. 1
4. 0
Activation energy for a chemical reaction mainly depends upon
1. temperature
2. nature of reacting species
3. concentration of reacting species
4. collision frequency
A molecule of gas is struck by another molecule of same gas , the first molecule shows
1. an exchange of potential energy
2. an exchange of kinetic energy
3. an exchange of chemical energy
4. no exhange of energy
Activation of a chemical reaction can be determined by
1. changing concentration of reactants
2. Evaluating rate constant at standard temperature
3. Evaluating rate constant at 2 different temeperatures
4. Evaluating velocities of reaction at 2 different temeprature
Energies of activation for forward and reverse reaction for $A_{2} + B_{2} - - > 2 A B$ are 180 kJ/mol and 200kJ/mol. In presence of catalyst lowers activation energy of both (forward & backward ) by 100kJ/mol. Forward reaction will be
1. 300
2. 120
3. 280
4. -20
A -->B enthalpy chaange is -10 kJ/mol and E= 50 kJ/mol , then Ea of B --> A will be
1. 40kJ/mol
2. 50 kJ/mol
3. -50kJ/mol
4. 60kJ/mol
Rate of a reaction double when its temperature changes from 300 k to 310 K . Activation energy of such a reaction will be
1. 53.6 kJ/mol
2. 48.6 kJ/mol
3. 58.6 kJ/mol
4. 60.6 kJ/mol
Rate of chemcial reaction doubles for every 10 C rise of temperature is raised by 50 C the rate of the reaction increases by about
1. 10 times
2. 24 times
3. 32 times
4. 64 times
Reactant (A ) forms 2 products
A --> B having k1 and energy E1
A --> C having k2 and energy E2
If E2= 2E1 , then k1 and k2 are related as
1. $k_{1} = {2k}_{2} e^{E / R T}$
2. $k_{1} = k_{2} e^{E / R T}$
3. $k_{2} = k_{1} e^{E / R T}$
4. $k_{1} = {Ak}_{2} e^{E / R T}$
First order rate constant k is related to temperature as log k = 15- $10^{6}$ / T . Correct values are
1. A = $10^{15}$ , E = 1.9 X $10^{4}$ kJ
2. A = $10^{-15}$ and E = 40 kJ
3. A = $10^{15}$ and E = 40 kJ
4. A = $10^{-15}$ , E = 1.9 X $10^{4}$ kJ
Arrhenius relationship of 2 different reaction is shown below. Which reaction is faster at a lower temperature and which is more sensitive to changes of tmeperature ?
1. B faster , A more sensitive
2. B in both cases
3. Ain both cases
4. A faster , B more sensitive
Ratecosntant of most of the reactions increases with increase in temperature . According to the Arrhenius equation $k = A e^{- E / R T}$ . Curve of rate constant k against temperature T will be
For a reaction , the rate constant is expressed as $k = A e^{- 40000 / T}$ . Energy of activation is
1. 40000 cal
2. 88000 cal
3. 80000 cal
4. 90000 cal
Ratio of rate cosntants at 27 C and 37 C is Q. What should be the energy for a reaction Q= 2.5 ?
1. 71 kJ
2. 212kJ
3. 35 kJ
4. 12.1 kJ
Decomposition of nitric oxide into nitrogenand oxygen in presence of gaseous argon follow second order kinetics with k = $5 X 10^{11} L / m o l s e c e^{- 41570 / T}$ .
Energy of activation is
1. 500000J
2. 41570 k
3. 5000 J
4. 345612.98 J
In a first order reaction concentration of reactant decreases from 800 mol per dm cube to 50 mol per dm cube in 200 second . Rate constant of reaction in per second is
1. 20000
2. 0.0000345
3. 0.01386
4. 0.0002
Rate constant for a second order reaction is 0.00008 per M min . How long will it take a 1M solution to be reduced to 0.5 M ?
1. 0.00008 min
2. 8665 min
3. 0.0004 min
4. 12500 min
A reaction that is of first order wrt reactant A has rate constant 6 per min . If we start with [A] =0.05 mol/L , when would [A] would reach value 0.05 mol/L
1. 0.384 min
2. 0.15 min
3. 3 min
4. 3.84 min
Order of a chemical reaction that obeys expression t= 1/k.a is
1. 1st
2. 2nd
3. 3rd
4. 4 th
For a reaction , optiocal density of solution was measured, which may be loneraly related to concentrration of reactant. Values of optiocal density are 0.80 , 0.35 and 0.20 at the end of 20 min . 40 min and infinity after the staart of reaction . Rate constant is
1. 0.00693 per min
2. 0.0351 per min
3. 0.0693 per min
4. 0.00351 per min
rate constant for the reaction A --> B is 0.0002 L/mol. Concetration of A at which rate of the reaction is (1/12) X $10^{- 5}$ M /sec
1. 0.25 M
2. $(1 / 20) \sqrt{5 / 3}$ M
3. 0.5 M
4. none of these
In a I order reaction A --> products , the concentration of the reactant decrease to 6.25% of its initial value in 80 minutes. What is the rate constant and rate of reaction , 100 minutes after the start , if the initial concentration is 0.2 mol/Litre ?
1. 2.17 X $10^{- 2}$ per min; 3.47 X $10^{- 4}$ mol /litre min
2. 3.465 X $10^{- 2}$ per min ; 2.16 X $10^{- 4}$ mol /litre min
3. 3.465 X $10^{- 3}$ per min; 2.67 X $10^{- 3}$ mol /litre min
4. 2.165 X $10^{- 3}$ per min; 2.6 X $10^{- 4}$ mol /litre min
Which of the following formula represents a first order reaction?
1. k = x/t
2. k = 1/2t [1/(a-x)^2 - 1/a^2]
3. k= 2.303/t log (a/a-x)
4. k = 1/t (a/a-x)
In a first order reaction . concentration of the reactant decreases from 0.8 m to 0.4 M in 15 minutes . The times taken for concetration from 0.1 M to 0.025 M is
1. 10min
2. 15 min
3. 7.5 min
4. 30 min
Rate constant of decomposition of dinitrogen pentaoxide is 0.023 per second. Which is the right equation ?
1. $[N_{2} O_{5}]_{t} = [N_{2} O_{5}]_{o} + k t$
2. $[N_{2} O_{5}]_{t} e^{k t} = [N_{2} O_{5}]_{o}$
3. $\log [N_{2} O_{5}]_{t} = \log [N_{2} O_{5}]_{o} - k t$
4. $\log \frac{[N_{2} O_{5}]_{t}}{[N_{2} O_{5}]_{o}} = k t$
If the rate constant for disintegration of a radioactive nucleus is $λ$ . Therefore probability P of survival of a radioactive for one mean life is
1. e
2. $e^{+ 2}$
3. $e^{- 1}$
4. $e^{- 2}$
First order reaction which is 30 % complete in 30 minutes has a half life period of
1. 24.2 min
2. 58.2 min
3. 102.2 min
4. 120 .2 min
Half life for the reaction in 24 hr at 30 C . Starting with 10 g of dinitrogenpentaoxide how many grams of dinitrogenpentaoxide will remain after a period of 96 hours ?
1. 1.25 g
2. 0.63 g
3. 1.7 g
4. 0.5 g
Half life of a reaction is found to be inversely proportional to cube of ots initial concentration . Order of reaction is
1. 2
2. 5
3. 3
4. 4
Observe the following reaction A + 3B --> 2C .Rate of reaction {-d[A]/dt} = 0.003 mol/litre min. Value of -d[B]/dt is
1. 0.003 mol/litre sec
2. 0.009 mol/litre sec
3. 0.001 mol/litre sec
4. 0.0015 mol/litre sec
In the formation of sulphur trioxide by contact process , rate of reaction d[oxygen ]/dt = 0.0004 mol/litre sec
Rat3e of reaction expressed in terms of Sulphur trioxdie will be
1. 0.0003 mol/L sec
2. 0.0006 mol/L sec
3. 0.00015 mol/L sec
4. 0.00045 mol/L sec
If 3A --> 2B , then rate of reaction of d[B] /dt is equal to
1. 2 d[A]/dt
2. -1/3 d[A]/dt
3. -2/3 d[A]/dt
4. -3/2 d[A]/dt
In reduction reaction of peroxydisulphate ion by iodide ion , rate of diappearance is Iodide is 0.00045 mol / Lsec . Formation of sulphate ion is
1. 0.001 mol /L sec
2. 0.002mol /L sec
3. 0.003 mol /L sec
4. 0.004 mol /L sec
Reaction of formation of ammonia under certain conditions of temperature and partial pressure of the reactants , rate of formation of ammonia is 0.001 kg/hr . Rate of conversion of hydrogen under the same conditions is
1. 0.000182 kg/hr
2. 0.0015kg/hr
3. 15200 kg/hr
4. 0.00182 kg/hr
Rate of formation of sulphur trioxide is 10 g/sec. Rrate of disappearance of oxygen will be
1. 5 g/sec
2. 100 g/sec
3. 20 g/sec
4. 2 g/sec
Rate of heterogeneous reaction doesnt depend on
1. Concnetration of reactants
2. surface area of reactants
3. pressure of reactant gases
4. potential energy of reactant
Gaseous hypothetical chemical eqaution 2A --> 4B + C is carried out in a closed vessel . Concentration of B is found to increase by 0.005 mol /L in 10 second . Rate of appearance of B is
1. 0.0005 mol /Lsec
2. 0.00005 mol /Lsec
3. 0.00006 mol /Lsec
4. 0.0004 mol /Lsec
For reaction 2A + 3B --> 4C rate of reaction may be represented by
1. r= 2 d [A]/dt = 3 d[B]/dt = 4 d[C]/dt
2. r= -6 d [A]/dt = -4d[B]/dt = 3d[C]/dt
3. r= -1/2 d [A]/dt = 1/3 d[B]/dt = 1/4 d[C]/dt
4. r= -1/2 d [A]/dt = -1/3 d[B]/dt = 1/4 d[C]/dt
Rate of disappearance of sulphur dioxide in formation of sulphur trioxide is 0.00128 g/sec Then formation of Sulphur trioxide is
1. 0.00064 g/sec
2. 0.0008 g/sec
3. 0.00128 g/sec
4. 0.0016 g/sec
For reaction 2A + B --> 3C + D which is not following does not express the reaction rate
1. d[D]/dt
2. -d[A]/dt
3. -d[C]/3dt
4. -d[B]/dt
instantaneous rate of disappearanace of MnO4 ion in the reaction is 0.00456 M/sec. Rate of appearance of iodine is
1. 0.00114 m/sec
2. 0.0057 M/sec
3. 0.00456 M/sec
4. 0.0114M/sec
Rate constant for the reaction of decomposition of dinitrogenpentaoxide is 0.00003 per second .If the rate of reaction is 0.00024 Mol/ Litre sec , then concetnration of dinitrogen pentaoxide is
1. 1.4 M
2. 1.2 M
3. 0.04 M
4. 0.8 M
Rate of reaction is expressed in different ways as
1/2 (d[C]/dt ) =-1/3 , (d[D]/dt) = 1/4 (d[A]/dt) = - (d[B]/dt) . Reaction is
1. 4A + B --> 2C + 3 D
2. B + 3D --> 4A + 2C
3. 4A + 2B --> 2C + 3 D
4. B + 1/2D --> 4A + 3C
For a reaction A --> B , the rate pf reaction qaudrupled when concentration of A is doubled. Rste expression of the reaction is r = k[A] ^n when n is
1. 1
2. 0
3. 3
4. 2
Rate constant of a first order reaction is 3 X $10^{- 6}$ per second. If initial concetration is 0.10M , the initial rate of reaction is
1. 3 X $10^{- 5}$ M/sec
2. 3 X $10^{- 6}$ M/sec
3. 3 X $10^{- 8}$ M/sec
4. 3 X $10^{- 7}$ M/sec
For reaction H2 + Br2--> 2HBr overall order is found to be 3/2 ,Rate of reaction can be expressed as
1. $[H_{2}] [B r_{2}]^{1 / 2}$
2. $[H_{2}]^{1 / 2} [B r_{2}]^{1}$
3. $[H_{2}]^{3 / 2} [B r_{2}]^{0}$
4. all of these
For a reaction , rate = k [trichloroethanal ][NO] . If concetration is expressed in mole/litre , units of k is
1. litre mol/sec
2. mol/litre sec
3. litre/mol sec
4. per second
Rate of 1st order reaction X --> products is 0.00075 mol/Lmin Value of rate constant when concetration of X is 0.5 mol /L
1. 0.0000375 per sec
2. 0.000025 per sec
3. 0.00015 per second
4. 0.0008 per second
Rate constant for a reaction of formation of HI is 49 , then rate constant of formation of hydrogen and Iodine from HI is
1. 7
2. 1/49
3. 49
4. 21
Rate of the reaction 3A + 2 B --> products is given by rate expression
Rate = k [A][B]²
if A is taken in excess then order of reaction is
1. 3
2. 2
3. 1
4. 5
In decomposition reaction of dinitrogenpentaoxide rate constant is 0.62 pre seocnd . Value of rate of reaction when dinitorgenpentaoxide is 1.25 mol
1. 0.775 per mol second
2. 0.00635per mol second
3. 0.0000515 per mol second
4. 0.385 per mol second
Rate law of a reaction A+ B --> products Rate= k $[A]^{n} [B]^{m}$ . On doubling the concetration of A and halving concentration of B , the ratio of new rate to the earlier rate of reaction will be
1. n-m
2. $2^{m - n}$
3. 1/ $2^{m + n}$
4. m+n
For reaction of formation of HCl taking place on water, order of reaction is
1. 1
2. 2
3. 3
4. 0
Rate of reaction between A & B increases by a factor of 100, when concentration of A is increased 10 folds . Order of reaction wrt A is
1. 10
2. 1
3. 0
4. 2
Rate of reaction between 2reactants A & B decreases by a factor 4 if the concentration of reactant B is doubled . The order of this reaction wrt B is
1. 1
2. -2
3. 2
4. 1
For the reaction NO2 + CO--> CO2 + NO , the experimental rate expression is - dc/dt = k[NO2]^2 , number of molecules of CO involves in the slowest step will be
1. 0
2. 1
3. 2
4. 3
For a reaction A +B --> products , rate is first order wrt A and second order wrt B . If 1 mole oeach of A & B are introduced into 1 L vessel and initial rate were 0.01 mol/ L sec . Rate when half of the reactants have been used
1. 0.00125 mol /Lsec
2. 0.012mol /Lsec
3. 0.0025 mol /Lsec
4. none of these
For reaction of decomposition of dinitrogen pentaoxide rate of reaction and rate cosntant are 0.000102 and 0.000034 per second. Concentration of nitric oxide at that time will be
1. 1.73
2. 3
3. 1.02
4. 3.4
Rate equation for reaction
2A + B --> C is rate = k[A][B]
Correct statement is
1. K is independent of [A] and [B]
2. t 1/2 is constant
3. unit of k is per second
4. Rate of o formation of C is twice the rate of disappearance of A
Rate of a gaseous reaction is given by expression R = k[A] [B] . if volume of the vessel is suddenly reduced to 1/4 of initial volume ,new rate relating to original rate will be
1. 1/10
2. 1/8
3. 8
4. 16