Used to express velocity at any instant of time :
- Ainitial velocity
- ✓instantaneous velocity
- Caverage velocity
- Dstandard velocity
Answer: B.
View full solution →Question types
Chemical Kinetics question types
122 questions across 7 question groups — pick any mix to generate a Chemistry paper with step-by-step answer keys.
122
Questions
7
Question groups
5
Question types
01
M.C.Q [1M]
39 Q→02Fill in the blank. [1M]
11 Q→031 Marks Question
26 Q→04Short Answer Type Questions [2M]
9 Q→053 Marks Question
14 Q→06Long Answer Type Questions [5M]
19 Q→074 Marks Questions
4 Q→Sample Questions
Chemical Kinetics questions
One sample from each question group in this chapter. Select any group above to see the full set with answer keys.
It is used to express rate at any instant of time $\qquad$ ?
- Ainitial rate
- ✓instantaneous rate
- Caverage rate
- Dstandard rate
Answer: B.
View full solution →The graph between $\ln [R]$ and $t$ for the first order reaction is :
- ✓
- B
- C
- D
Answer: A.
View full solution →The graph between in $[R]$ and $t$ for the first order reaction is :
- ✓
- B
- C
- D
Answer: A.
View full solution →What is the order of integral rate reaction with expression $k =\frac{2.303}{t} \log \frac{[ R ]_0}{[ R ]}$ ?
- AZero order
- ✓First order
- CSecond order
- DThird order
Answer: B.
View full solution →The kinetic energy of maximum fraction of reactant molecules is called _____________ .
The concentration of a reactant decreases from 20 mol to 10 mol or from 10 mol to 5 mol . There will be _____________ time for both.
In half-life, the concentration of reactions have remained _____________ .
Value of activation energy _____________in the presence of catalyst.
The speed of activation energy _____________ in the presence of catalyst.
Write the order of natural and artificial nuclear (radioactive) decay?
Write the unit of rate constant for zero order reaction.
In a pseudo first order reaction in water, the following results were obtained :
Calculate the average rate of reaction between the time interval 30 to 60 seconds.
| t/s | 0 | 30 | 60 | 90 |
| [A] mol L-1 | 0.55 | 0.31 | 0.17 | 0.085 |
For a reaction, if $t_{1 / 2} \propto[ R ]_0$ is 0 , then what will be the order of reaction?
View full solution →What is effective collision?
A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is :
(i) doubled (ii) reduced to half ?
(i) doubled (ii) reduced to half ?
The decomposition of dimethyl ether leads to the formation of CH4, H2 and CO and the reaction rate is given by
Rate $= k \left[ CH _3 OCH _3\right]^{3 / 2}$
The rate of reaction is followed by increase in pressure in a closed vessel, so the rate can also be expressed in terms of the partial pressure of dimethyl ether, i.e.,
Rate $= k \left( p _{ CH _3 OCH _3}\right)^{3 / 2}$
If the pressure is measured in bar and time in minutes, then what are the units of rate and rate constants?
View full solution →Rate $= k \left[ CH _3 OCH _3\right]^{3 / 2}$
The rate of reaction is followed by increase in pressure in a closed vessel, so the rate can also be expressed in terms of the partial pressure of dimethyl ether, i.e.,
Rate $= k \left( p _{ CH _3 OCH _3}\right)^{3 / 2}$
If the pressure is measured in bar and time in minutes, then what are the units of rate and rate constants?
The rate constant for a first order reaction is 60 s-1. How much time will it take to reduce the initial concentration of the reactant to its 1/16th value?
Calculate the half-life of a first order reaction from their rate constants given below :
(i) $200$ $s^{-1}$
(ii) $2$ $min^{-1}$
(iii) 4 year $^{-1}$
View full solution →(i) $200$ $s^{-1}$
(ii) $2$ $min^{-1}$
(iii) 4 year $^{-1}$
The experimental rate equation of a reaction $2 N _2 O \rightarrow 2 N _{ 2 }+ O _2$ is as follows: rate $= k \left[ N _2 O \right]$. Write the mechamism of the reaction.
View full solution →A reaction is first order in A and second order in B.
(i) Write the differential rate equation.
(ii) How is the rate affected on increasing the concentration of B three times?
(iii) How is the rate affected when the concentration of both A and B are doubled?
(i) Write the differential rate equation.
(ii) How is the rate affected on increasing the concentration of B three times?
(iii) How is the rate affected when the concentration of both A and B are doubled?
What is the effect of temperature on the rate constant of a reaction? How can this effect of temperature on rate constant be represented quantitatively?
The rate of a reaction quadruples when the temperature changes from 293 K to 313 Κ. Calculate the energy of activation of the reaction assuming that it does not change with temperature.
The decomposition of NH3 on platnium surface is zero order reaction. What are the rates of production of N2 and H2 if = 2.5 × 10-4 mol L-1 s-1?
The decomposition of hydrocarbon follows the equation
$k =\left(4.5 \times 10^{11} s^{-1}\right) e ^{-28000 K / T }$ Calculate Ea.
View full solution →$k =\left(4.5 \times 10^{11} s^{-1}\right) e ^{-28000 K / T }$ Calculate Ea.
(i) Define the order of a reaction.
(ii) Explain the effect of concentration of reactant on the rate constant.
(iii) For a first order reaction, if the rate constant at 500 K and 600 K are $0.03 s^{-1}$ and $0.06 s^{-1}$ respectively, then calculate the activation energy.
$
\left[R=8.314 JK^{-1} mol^{-1}, \log 2=0.3010\right]
$
View full solution →(ii) Explain the effect of concentration of reactant on the rate constant.
(iii) For a first order reaction, if the rate constant at 500 K and 600 K are $0.03 s^{-1}$ and $0.06 s^{-1}$ respectively, then calculate the activation energy.
$
\left[R=8.314 JK^{-1} mol^{-1}, \log 2=0.3010\right]
$
(i) Define molecularity of a reaction.
(ii) Explain the effect of presence of catalyst on the rate of reaction.
(iii) In a first order reaction at 300 K , the initial concentration of the reactant was $1.0 \times 10^{-2} mol L ^{-1}$, which decreased to $0.5 \times 10^{-2} molL ^{-1}$ after 30 minutes at 300 K . Calculate the rate constant of the reactant at 300 K. $[\log 2=0.3010] \quad$
View full solution →(ii) Explain the effect of presence of catalyst on the rate of reaction.
(iii) In a first order reaction at 300 K , the initial concentration of the reactant was $1.0 \times 10^{-2} mol L ^{-1}$, which decreased to $0.5 \times 10^{-2} molL ^{-1}$ after 30 minutes at 300 K . Calculate the rate constant of the reactant at 300 K. $[\log 2=0.3010] \quad$
The time required for 10% completion of a first order reaction at 298 K is equal to that required for its 25% completion at 308 K. If the value of A is 4 × 1010 s-1 Calculate k at 318 K and Ea.
The rate constant for the first order decomposition of H2O2 is given by the following euqation :
$\log k=14.34-1.25 \times 10^4 K / T$
Calculate $E_{a}$ for this reaction and at what temperature will its half-period be 256 minutes?
View full solution →$\log k=14.34-1.25 \times 10^4 K / T$
Calculate $E_{a}$ for this reaction and at what temperature will its half-period be 256 minutes?
The rate constant for the decompositon of N2O5 at various temperatures is given below :
Draw a graph between In k and 1/T and calculate the values of A and Ea. Predict the rate constant at $30^{\circ}$ and $50^{\circ}C$.
View full solution →| $T /{ }^{\circ} C$ | 0 | 20 | 40 | 60 | 80 |
| $10^5 \times k / s ^{-1}$ | 0.0787 | 1.70 | 25.7 | 178 | 2140 |
Mention the factors that affect the rate of a chemical reaction.
The decomposition of A into product has value of k as $4.5 \times 10^3 s^{-1}$ at $10^{\circ} C$ and energy of activation $60 kJ mol ^{-1}$. At what temperature would k be $1.5 \times 10^4 s^{-1} ?$
View full solution →Sucrose decomposes in acid solution into glucose and fructose according to the first order rate law, with $t_{1 / 2}$ = 3.00 hours. What fraction of sample of surcrose after 8 hours?
View full solution →The rate constant for the decomposition of hydrocarbons is 2.418 × 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?
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