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CBSE Questions for Class 12 Engineering Chemistry Chemical Kinetics Quiz 13 - MCQExams.com

A reaction requires 60 minutes and 20 minutes to complete 50% at 27oC and 47oC respectively. calculate activation energy of the reaction.
  • 45678 cal
  • 26789 cal
  • 10480 cal
  • None of these
What will be the initial rate of a reaction if its rate constant is 103min1 and the concentration of reactant is 0.2 mol.dm1. Also, the amount of reactant converted into products in 200 minutes is:
  • 2×104mol.dm3min1, 81.97%
  • 2×104mol.dm3min1, 18.03%
  • 2×104mol.dm3min1, 76%
  • 2×104mol.dm3min1, 24%
75% of a first-order reaction is completed in 30 minutes. What is the time required for 93.75% of the reaction (in minutes) ?
  • 45
  • 120
  • 90
  • 60
When the initial concentration of the reactant doubled, the half-life period of the reaction is also doubled. Hence the order of the reaction is
  • one
  • two
  • fraction
  • zero
A reaction  PQ  is  25%  complete in  25min,   50%  complete in  25min  if  [P]  is halved. The reaction is  25%  completed in   50min  if  [P]  is doubled. The order of reaction is
  • 1
  • 2
  • 0
  • 3
The initial concentration of N2O5 in the following first order reaction  N2O5(g)2NO2(g)+12O2(g) was 1.24×102 molL1 at 318 K. The concentration of N2O5 after 60 min was 0.20×102 molL1. Calculate the rate constant of the reaction at 318 K.
  • 0.0104min1
  • 0.0204min1
  • 0.0304min1
  • 0.0404min1
Reaction AB follows second order kinetics. Doubling the concentration of A will increase the rate of formation of B by a factor of:
  • 1/4
  • 1/2
  • 2
  • 4
The half-life of a first-order reaction is 10 min. If the initial amount is 0.08 mol/L and the concentration at some instant is 0.01mol/L then time will be:
  • 10 min
  • 30 min
  • 20 min
  • 40 min
Consider the following first order competing reaction :
XK1A+B and YK2C+D 
if 50% of the reaction of X was completed when 96% of the reaction of Y was completed , the ratio of their rate constant (K2/K1) is:
  • 4.06
  • 0.215
  • 1.1
  • 4.65
The curves M and N represent the variation of energy with reaction coordinates for the reaction A(g)+B(g)C(g)+D(g) in absence and presence of negative catalyst
Of the curves M and N, which represents the Ea for the backward reaction in the presence of catalyst 
1286328_f1e31d0ed60f4b9f82ecf6d0160731e4.png
  • P
  • Q
  • S+P
  • P+Q
In a first order reaction, 0.16 moles of reactant decrease to 0.02 moles in 144 minutes, its half life is ?
  • 24
  • 12
  • 72
  • 48
For a zero order reaction:
  • t12a
  • t121a
  • t12a2
  • t121a2
A graph of log10k is plotted against 1/T for a reaction with order 2.If the activation energy is 10 kJ/mol, then magnitude of the slope will be: 
  • 4.34×103
  • 5.2×102
  • 1.2×104
  • 6.8×103
In a zero order reaction 47.5% of the reactant remains at the end of 2.5 hours. The amount of reactant consumed in one hour is 
  • 10.5%
  • 32.0%
  • 52.6%
  • 21.0%
The decomposition of A follows first order kinetics by the following equation:

4A(g)ΔB(g)+2C(g)

If initially, the total pressure was 800 mm of Hg and after 10 minutes it is found to be 650 mm of Hg. What is the half-life of A?
(Assume only A is present initially)
  • 10 minutes
  • 5 minutes
  • 7.5 minutes
  • None of these
For a reaction
2A+BC+D, the active mass of B is kept constant but that of A is tripled. The rate of reaction will -
  • Decrease by 3 times
  • Increased by 9 times
  • Increase by 3 times
  • Unpredictable
For a reaction: nA product, the rate constant and rate of reactions are equal, What is the order of the reaction ?
  • 0
  • 1
  • 2
  • 3
The time taken for the completion of 90% of a first order reaction is 't' min. What is the time (in sec) taken for the completion of 99% of the reaction ?
  • 2t
  • t/30
  • 120t
  • 60t
For zero  order reaction, A,a graph of rate vs time has slope equal to:( where k=rate of reaction)
  • k
  • -k
  • zero
  • -2.303 k
For a homogeneous reaction A3B, if pressure after sometime t was Pt and after completion of reaction, pressure was P.Then select the correct relation.
  • K×t = ln (2P3(PPt))
  • K×t = ln (7P3(PPt))
  • K×t = ln (3P2(PPt))
  • K×t = ln (5P2(PPt))
The general integrated rate equation for first-order reaction is given by:
  • k=2.303tln[A]0[A]t
  • k=1tln[A]0[A]t
  • k=2.303tlog10[A]0[A]t
  • k=1tln[A]0[A]t
The first order reaction has half-life of 18 hrs. What percentage of the reactant will remain after 24hrs  (log2=0.3,log2.5=0.4)
  • 20%
  • 40%
  • 45.5%
  • 68.2%
The rates of most reactions doubled when their temperature is raised from 298 K to 308 K, calculate their activation energy?
  • 42.0 kJ
  • 5.29 kJ
  • 4.2 kJ
  • 52.9 kJ
A first order reaction goes upto 8% in 10 min. What time will it take to complete 99%
  • 555.55min
  • 305.52 min
  • 158.32 min
  • 155.55 min
The rate constant of a reaction increased by 5 when temperature is raised from 27o to 28o C. The activation energy of the reaction is (log 7=0.8450)
  • 36.5 KJ
  • 16.5 KJ
  • 47.5 KJ
  • 27.5 KJ
The catalysts decrease the Ea from 100KJmol1 to 80KJmol1. At what temperature the rate of reaction in the absence of catalyst at 500 K will be equal to the rate of reaction in the presence of a catalyst .
  • 400K
  • 625K
  • 1000K
  • +1000K
At least how half-lives should elapse for a I order reaction A products so that the reaction is at least 95 completed ? (log2=0.3)
  • 6
  • 5
  • 4
  • 7
The reaction, XY is an exothermic reaction. Activation energy of the reaction for conversation of x into Y is 150kJmol1. Enthalpy is 135kJmol1. The activation energy for the reverse reaction, YX will be
  • 280kJmol1
  • 285kJmol1
  • 270kJmol1
  • 15kJmol1
The rate constant of the first-order reaction may be described by following equation:

log K = 14.341.25×104T, calculate energy of activation.
  • 239.34kJ
  • 239.34 kcal
  • 239.34J
  • 239.34 cal.
Which one of the following plots is correct for a first order reaction:
If the concentration of reactant is reduced by n times, then the value of rate constant of the first order will 
  • Increase by n times
  • Decrease by n times
  • Not change 
  • Increase by 2n times
The initial concentration of cane sugar in presence of an acid was reduced from 0.20 to 0.10 M in 5 hours and to 0.05 M in 10 hours, what is the value of K? (in hr1)
  • 0.0693
  • 1.386
  • 0.1386
  • 3.465
For a first order reaction, the ratio of time for the completion of 99.9% and half of the reaction is
  • 8
  • 2
  • 6.6
  • 10
 If a reaction follows the Arrhenius equation, the plot lnK vs 1(RT)  gives a straight line with a gradient (y) unit. The energy required to activate the reactant is : 
  • y unit
  • -y unit
  • yR unit
  • y/R unit

The concentration of N2O5 in liquid bromine varied with time as follows:


t/s



0



100



300



500



[N2O5]M



0.12



0.088



0.049



0.026


What will be the rate constant and order of reaction?

  • k=2×103s1, order=1st
  • k=3.06×103s1, zero
  • k=4×103s1, zero
  • None of these
The rate  law of the reaction A + 2B product is given by d(product)dt=k[A]2[B]. If A is taken in large excess, the order of the reaction will be:
  • 1
  • 2
  • 3
  • 0
Consider the following in respect of zero-order reaction
i. t12 is directly proportional to the initial concentration
ii. Time taken for the completion of the reaction is twice its t1/2
iii. Concentration of the reactant decreases linearly with time
Which of the statements given above are correct?
  • I&II only
  • I&III only
  • II & III only
  • I, II & III
Activation energy of forward and backward process of reaction are 60 kJ and 40 kJ mol1 respectively . Which of the following are true statements ?
  • It is endothermic reaction.
  • It is exothermic reaction.
  • Heat of reaction is +20 kJ mol1
  • Thershold enregy of reaction is 100 kJmol1
If the values of enthalpies of reactants and products are p and q J/mol respectively. If the activation energy for the backward reaction is r J/mol, then the activation energy for forward reaction will be in (J/mol) (take only magnitudes)
  • p-q-r
  • p-q+r
  • q-p-r
  • q-p+r
Activation energy of the backward reaction is 10 kcal and ΔH= 2.813 kcal.

Activation energy of the forward reaction is ___________ kcal.
  • 128.13
  • 12.813
  • 12813
  • none of these
Decomposition of HI (g) on Gold surface is zero order reaction.Initially few moles of H2 are present in container then which of the following graph is correct?
For the decomposition of N2O5(g) it is given that - 2N2O5(g)4NO2(g) Activation energy = Ea, N2O5(g)2NO2(g)+12O2(g) activation energy =Eathen 
  • Ea=2Ea
  • Ea>Ea
  • Ea<Ea
  • Ea=Ea
For a particular gaseous reaction a graph was plotted as shown. It shows that the reaction of A is
1386948_e50d9dd12d744070a54c2afdc4076584.PNG
  • Zero order w.r.t A
  • 1st order w.r.t A
  • Second order w.r.t A
  • a non-integer order w.r.t A
For a first order reaction, AP,t1/2(half -life)  is 10 days. The time required for 14th conversion of A(in days) is : (ln2 = 0.693,  ln3 = 1.1)
  • 4.1
  • 5
  • 2.5
  • 3.2
For the chemical reaction, A products, the following logK=16.3982800T
Arrhenius factor for the reaction is______________
  • 2.5×1016
  • 5×1016
  • 109
  • None of these 
According to the Arrhenius equation, 
  • a high activation energy usually implies a fast reaction
  • rate constant increases with increase in temperature. This is due to a greater number of collisions whose energy exceeds the activation energy
  • higher the magnitude of activation energy, stronger is the temperature dependence of the rate constant.
  • the pre-exponential factor is a measure of the rate at which collisions occure, irrespective of their energy.
For a gaseous equilibrium : 2A(g)2B(g)+C(g)  Kp  has a value 1.8 at 700 K.  The value of Kc  for the equilibrium : 2B(g+C(g)2A(g)  at that temperature is about  _________.
  • 0.031
  • 32
  • 57.4
  • 103.3
In the following first order competing reaction:
A+Reagent Product B+Reagent Product
The ratio of K1/K2 if only 50% of B will have been reacted when 94% of A has been reacted is:
  • 4.06
  • 0.246
  • 2.06
  • 0.06
AB first order reaction A is optical active and B is optically inactive, a series of experiment were conducted on a solution of A
Time060 min
optical rotation82o77o2o
Assume some impurity present calculate the optical rotation after 5 hours
(Given in 1.066=0.064,e0.16=1.17)
  • 60
  • 30
  • 20
  • 120
For an exothermic reaction Ea,Ea are the activation energies of the forward and backward reactions respectively. Then which is always false:
  • Ea<Ea
  • Ea>H
  • Ea<H
  • Ea<H
0:0:2


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