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CBSE Questions for Class 12 Engineering Chemistry Chemical Kinetics Quiz 7 - MCQExams.com

For certain first-order reaction, 75% of the reaction complete in 30 min. How much time did it require to complete 99.9% of the reaction?
  • 150 min
  • 100 min
  • 90 min
  • 300 min
For the reaction system:
2NO(g)+O2(g)2NO2(g), volume is suddenly reduced to half its value by increasing the pressure on it. If the reaction is of first order with respect to O2 and second order with respect to NO, the rate of reaction will:
  • diminish to one-eighth of its initial value
  • increase to eight times of its initial value
  • increase to four times of its initial value
  • diminish to one-fourth of its initial value
Which is correct about zero order reaction?
  • Rate of reaction depends on decay constant
  • Rate of reaction is independent of concentration
  • Unit of rate constant is concentration
  • Unit of rate onstant is concentration time
The rate of a particular reaction doubles when temperature change from  270C to 370C. Calculate the energy of the activation of such reaction.
  • 53582 KJ
  • 53.58 KJ
  • 29.86 KJ
  • none of these
The activation energy of a reaction is 94.14 kj/mole, and the value of rate constant at 313K is 1.8\times 10^{-1}sec^{-1}. Calculate the frequency factor A.
  • [A]=8.25\times 10^{10}s^{-4}.
  • [A]=7.923\times 10^{10}s^{-4}.
  • [A]=9.194\times 10^{10}s^{-4}.
  • none of these
Find the two third life (t_{2/3}) of a first order reaction in which K=5.48\times 10^{-14}sec^{-1}.
  • t_{2/3}=5\times 10^{13} sec
  • t_{2/3}=2\times 10^{13} sec
  • t_{2/3}=1.25\times10^{13} sec
  • none of these
What is the activation energy of a reaction if its rate doubles when temperatures is raised from 20^oC to 35^oC?(R=8.314 JK^{-1} mol^{-1})
  • 34.7 kJ mol^{-1}
  • 15.1 kJ mol^{-1}
  • 342 kJ mol^{-1}
  • 269 kJ mol^{-1}
The rate constant for the decomposition of a hydrocarbon is 2.418\times 10^{-5}S^{-1} at 546 K. If the energy of activation is 179.9 kJ/mol. What will be the value of pre-exponential factor A?
  • [A]=9.245\times 10^{12}s^{-1}.
  • [A]=3.912\times 10^{12}s^{-1}.
  • [A]=7.83\times 10^{12}s^{-1}.
  • None of these
Which one of is first order reaction ?
  • NH_4NO_2 \rightarrow N_2 + 2H_2O
  • 2HI\rightleftharpoons H_2 + I_2
  • 2NO_2 \rightarrow 2NO + O_2
  • 2NO + O_2 \rightarrow 2NO_2
The energy of activation for a first order reaction is 104 kJ mol^{-1}. The rate constant at  25^oC is 3.7\times 10^{-5} s^{-1}. What is the rate constant at 30^oC ?
  • 5.2\times 10^{-4}s^{-1}
  • 7.4 \times 10^{-5} s^{-1}
  • 7.72\times 10^{-5}s^{-1}
  • None of these
What is the activation energy for a reaction whose rate constant doubles when temperature changes from 30^oC to 40^oC?
  • 72.56\ KJmol^{-1}
  • 45.45\ KJmol^{-1}
  •  54.66\ kJ mol^{-1}
  • None of these
Find out the percentage of the reactant molecules crossing over the activation energy barrier at 325K, given that \triangle { H }_{ 325 }=0.12kcal,\quad { E }_{ a(b) }=+0.02kcal.
  • 0.80%
  • 80.63%
  • 20%
  • None of these
For a reversible reaction : { N }_{ 2 }+{ O }_{ 2 }\rightleftharpoons \quad 2NO
Activation energy of the backward reaction is lower than that of forward reaction. The slope of k verse 1/T graph will be:
  • zero
  • -\frac { H }{ 2.303\quad R }
  • \frac { H }{ 2.303\quad R }
  • -\frac { \Delta H }{ \quad R }
Activation Energy is defined as the least possible amount of energy (minimum ) which is required to start a reaction or the amount of energy available in a chemical system for a reaction to take place.
State whether it is True or False: 
  • True
  • False
The activation energy for a certain reaction is 334.4 kJ mol^{-1}. How many times larger is the rate constant at 610 K than the rate constant at 600 K?
  • Two times
  • Three times
  • Four times
  • None of these

 In a first-order reaction the concentration of the reactant is decreased from 1.0{\text{ M to 0}}{\text{.25 M }}  in 20 min.The rate constant of the reaction would be:

  • 10{\text{ mi}}{{\text{n}}^{ - 1}}
  • 6.931{\text{ mi}}{{\text{n}}^{ - 1}}
  • 0.6931{\text{ mi}}{{\text{n}}^{ - 1}}
  • 0.06931{\text{ mi}}{{\text{n}}^{ - 1}}
A first order reaction is half-completed in 45 minutes. How long does it need for 99.9\% of the reaction to be completed?
  • 20 hours
  • 10 hours
  • 7\ \dfrac{3}{10} hours
  • 5 hours
For a first order reaction, 

(A) \rightarrow products, 

the concentration of A changes from 0.1M to 0.025M in 40 minutes. The rate of reaction when the concentration of A is 0.01 M is:
  • 1.73\times 10^{-4} mol dm^{-3} min^{-1}
  • 1.73\times 10^{-5} mol dm^{-3} min^{-1}
  • 3.47\times 10^{-4} mol dm^{-3} min^{-1}
  • 3.47\times 10^{-5} mol dm^{-3} min^{-1}
The reaction : X \rightarrow product, follows first-order kinetics in 20 minutes, the concentration of X changes from 0.1 M to 0.05\ M then rate of reaction when concentration of X is 0.02\ mol/ L is:
  • 1.73 \times 10^{-4} M/min
  • 3.47 \times 10^{-5} M/min
  • 6.94 \times 10^{-4} M/min
  • 1.73 \times 10^{-5} M/min
For zero order reactions, the linear plot was obtained for [A] vs t. The slope of the line is equal to:
  • k_{0}
  • -k_{0}
  • \dfrac {0.693}{K_{o}}
  • -\dfrac {K_{o}}{2.303}
Rate of formation of { SO }_{ 3 } according to the reaction 2{ SO }_{ 2 }+O_{ 2 }\rightarrow 2{ SO }_{ 3 }\quad is\quad 1.6\times { 10 }^{ -3 }kg\quad min^{ -1 }. Hence rate at which SO_{ 2 } reacts is:
  • 1.6\times { 10 }^{ -3 }kg\quad { min }^{ -1 }
  • 8.0\times { 10 }^{ -4 }kg\quad { min }^{ -1 }
  • 3.2\times { 10 }^{ -3 }kg\quad { min }^{ -1 }
  • 1.28\times { 10 }^{ -3 }kg\quad { min }^{ -1 }
An endothermic reaction A\rightarrow B has an activation energy 15kcal/mole and the heat of reaction is 5kcal/mole. The activation energy of reaction B\rightarrow A is:
  • 20kcal/mole
  • 15kcal/mole
  • 10kcal/mole
  • zero
The rate of chemical reaction is directly proportional to the equilibrium constant.
In which of the following process reaction will be completed first?
  • K=10
  • K=1
  • K={ 10 }^{ 3 }
  • K={ 10 }^{ -2 }
In a reaction involving one single reactant, the fraction of the reactant consumed may be defined as f=\left(1-\dfrac {C}{C_{0}}\right) where C_{0} and C are the concentrations of the reactant at the after time, t. For a first order reaction:
  • \dfrac {df}{dt}=k(1-f)
  • -\dfrac {df}{dt}=kf
  • -\dfrac {df}{dt}=k(1-f)
  • \dfrac {df}{dt}=kf
In a first order reaction the amount of reactant decayed in three half lives (let a be is initial amount) would be:
  • 7a/8
  • a/8
  • a/6
  • 5a/6
If a first order reaction is completed to the extent of 75% and 50% in time interval, {t}_{1} and {t}_{2}, what is the ratio {t}_{1}:{t}_{2}?
  • \ln {2}
  • \cfrac{\ln{(3/4)}}{\ln{2}}
  • 2
  • 1/2
For the consecutive unimolecular-type first order reaction A \xrightarrow{k_1} R \xrightarrow{k_2} S, the concentration of component R, C_R at any time t is given by : C_R = C_{AO} K_1 \left[\dfrac{e^{k_1t}}{(k_2 - k_1)} + \dfrac{e^{-k_2t}}{(k_1 - k_2)}\right] if C_A = C_{AO}, CR = C_{RO} = 0 at t = 0 the time at which the maximum concentration of R occurs is:
  • t_{max} = \dfrac{k_2 - k_1}{ln(k_2/k_1)}
  • t_{max} = \dfrac{ln(k_2/k_1)}{k_2 - k_1}
  • t_{max} = \dfrac{e^{k_2/k_1}}{k_2 - k_1}
  • t_{max} = \dfrac{e^{k_2 - k_1}}{k_2 - k_1}
The time for half-life period of a certain reacting A\rightarrow product is an hour. How much time does it take for its concentration to come from 0.50 to 0.25 mol { L }^{ -1 } if it is a zero order reaction?
  • 0.25h
  • 1h
  • 4h
  • 0.5h
The rate constant, the activation energy and the arrhenius parameter of a chemical reaction at { 25 }^{ 0 }C are 3\times { 10 }^{ 14 }{ sec }^{ -1 }:\ 104.4J{ mol }^{ -1 } and 6.0\times { 10 }^{ 14 }{ sec }^{ -1 } respectively, the value of the rate constant as T\rightarrow \infty is:
  • 2\times { 10 }^{ 8 }{ sec }^{ -1 }
  • 6\times { 10 }^{ 14 }{ sec }^{ -1 }
  • \infty
  • 3.6\times { 10 }^{ 30 }{ sec }^{ -1 }
In the following first-order competing reactions. 

A+ \text{Reagent}\rightarrow \text{Product},\quad B+ \displaystyle{\text{Reagent}} \rightarrow \text{Product}

The ratio of { K }_{ 1 }/{ K }_{ 2 } if only 50% of B will have been reacted, When 94% of A has been reacted is?
  • 4.07
  • 0.246
  • 2.06
  • 0.06
For a firt order reaction A\to P, the temperature (T) dependent rate constant (k) was found to follow the equation \log k = -(2000)\dfrac{1}{T}+6.0. The pre-exponential factor A and the activation energy E_a, respectively, are?
  • 1.0\times 10^6s^{-1} and 9.2kJ\ mol^{-1}
  • 6.0^{-1} and 16.6kJ\ mol^{-1}
  • 1.0\times 10^6s^{-1} and 16.6kJ\ mol^{-1}
  • 1.0\times 10^6s^{-1} and 38.3kJ\ mol^{-1}
 T (in \,K) \dfrac{1}{T} (in \, K^{-1}) \log_{10} K
 7691.3\times 10^{-3} 2.9
 667 1.5\times 10^{-3} 1.1
From the following data: the activation energy for the reaction (cal/mol)  { H }_{ 2 }+{ I }_{ 2 }\rightarrow 2HI
  • 4\times { 10 }^{ 4 }
  • 2\times { 10 }^{ 4 }
  • 8\times { 10 }^{ 4 }
  • 3\times { 10 }^{ 4 }
For a reaction A \rightarrow B + C.. it was found that at the end of 10 minutes from the start, the total optical rotation of the system was 50^o and when the reaction was completed a was 100^o Assuming that  "A" a optically inactive. 'B' dextro rotatory and 'C' is laevo rotatory rate constant of this first order reaction is ?
  • 0.069 \,min^{-1}
  • 0.69 \,min^{-1}
  • 2.303 \,min^{-1}
  • 4.6 \,min^{-1}
At 373\ K, a gaseous reaction A\rightarrow 2B+C is found to be first order. Starting with pure A, the total pressure at the end of 10\ min. was 176\ mm and after a long time when A was completely dissociated, it was 270\ mm. The pressure of A at the end of 10 minutes was:
  • 94\ mm
  • 47\ mm
  • 43\ mm
  • 90\ mm
In the case of a zero-order reaction, the ratio of time required for 75% completion to 50 % completion is:
  • ln 2
  • 2
  • 1.5
  • none
Which integrated equation is correct for the following 1^{st} order reaction started with only A(g) in a closed rigid vessel?
A(g)\rightarrow B(g) + C(g)+ D(g)

where, P_i= initial pressure ;\quad   P_t= total pressure at time t
  • K=\dfrac { 2.303 }{ t } \log _{ 10 } \left[\dfrac { P_i }{P_t } \right]
  • K=\dfrac { 2.303 }{ t } \log _{ 10 } \left[\dfrac { P_t }{P_i } \right]
  • K=\dfrac { 2.303 }{ t } \log _{ 10 } \left[\dfrac { 2P_i}{3P_i-P_t} \right]
  • K=\dfrac { 2.303 }{ t } \log _{ 10 } \left[\dfrac { 3P_i}{2P_i-3P_t} \right]
If the concentration of reactants is reduced by n times then the value of rate constant of the first order will?
  • Increase by n times
  • Decrease by factor of n
  • Not change
  • None of these
The time elapsed of a certain between 33% and 67% completion of a first order reaction is 30 minutes. What is the time needed for 25% completion?
  • 150.5 minutes
  • 12.5 minutes
  • 180.5 minutes
  • 165.5 minutes

For which order reaction a straight line is obtained along with x - axis by plotting a graph between half-life \left( {{t_{1/2}}} \right) and initial concentration 'a'.

  • 1
  • 2
  • 3
  • 0
For the decomposition of HI the following logarithmic plot is shown: [R=1.98\ cal/mol-K]
The activation energy of the reaction is about?

1099536_1e30fd508e3740fb82ca5c5a32c949e6.png
  • 45600\ cal
  • 13500\ cal
  • 24600\ cal
  • 32300\ cal
How much faster would a reaction proceed at 25^0C than at 0^0C if the activation energy is 65 kJ?
  • 2 times
  • 16 times
  • 11 times
  • 6 times
A reaction of first - order completed 90\% in 90 minutes , hence , it is completed 50\% in approximately : 
  • 50 min
  • 54 min
  • 27 min
  • 62 min
Collision frequency of a gas at 1\ atm pressure is Z. Its value at 0.5\ atm will be:
  • 0.25Z
  • 2Z
  • 0.50Z
  • Z
Collision diameter is least in case of:
  • { H }_{ 2 }
  • He
  • { CO }_{ 2 }
  • { N }_{ 2 }
The half-life of a zero-order reaction is 30 minutes. What is the concentration of the reactant left after 60 minutes?
  • 25%
  • 50%
  • 6.25%
  • 0
A certain zero order reaction has k = 0.025 M s^{-1} for the disappearance of A. What will be the concentration of A after 15 seconds if the initial concentration is 0.50 M ? 
  • 0.50 M
  • 0.375 M
  • 0.125 M
  • 0.060 M
The rate constant for a recation is 10.8 \times 10^{-5} mol L^{-1}S^{-1}. The reaction obeys:
  • First order
  • Zero order
  • Second order
  • All are wrong
If 60\% of a first order reaction was completed in 60 minute, 50\% of the same reaction would be completed in approximately?
  • 46 minute
  • 60 minute
  • 40 minute
  • 50 minute
t_{1/2} v/s \dfrac{1}{a^2} is straight line graph then determine the order of a reaction:
  • zero order
  • first order
  • second order
  • third order
For a first order reaction rate constant is given as \log K = 14 - \dfrac{1.2 \times 10^4}{T} then what will be value of temperature if its half life period is 6.93 \times 10^{-3}\ min?
  • 100\ K
  • 1000\ K
  • 720\ K
  • 327\ K
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