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 →Question types
Chemical Kinetics question types
92 questions across 6 question groups — pick any mix to generate a Chemistry paper with step-by-step answer keys.
92
Questions
6
Question groups
5
Question types
01
M.C.Q (1 Marks)
39 Q→021 Marks Question
25 Q→032 Marks Questions
5 Q→043 Marks Question
4 Q→055 Marks Questions
8 Q→06Fill in the blank.
11 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.
Used to express velocity at any instant of time :
- Ainitial velocity
- ✓instantaneous velocity
- Caverage velocity
- Dstandard velocity
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 →Write the order of natural and artificial nuclear (radioactive) decay?
Write the unit of rate constant for zero order reaction.
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?
If two different reactions are carried out at the same temperature and the activation energy for both is also same, then will the rates of these reactions also be the same?
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 →What will be the order of reaction which takes 2 hours for $5 0 \%$ completion and 4 hours for $7 5 \%$ completion?
View full solution →In the reaction $2 A( g )+ B ( g ) \rightleftharpoons 2 C ( g )$, what will be the effect on the reaction rate if the volume of the vessel is increased to its initial volume and what will be the change in order of the reaction due to the change in volume?
View full solution →Explain three differences between the rate constant of reaction and rate of a reaction.
If the value of rate constants are same for three reactions whose orders are 1,2 , and 3 , then what will be the order of the rates of these reactions if the value of concentration is 1 M , less than 1 M and more than 1 M ?
The mechanism of the reaction $2 NO + Br _2 \rightarrow 2 NOBr$ is :
(i) $NO + Br _2 \rightleftharpoons NOBr _2$ (fast term)
(ii) $NOBr _2+ NO \rightarrow 2 NOBr$ (slow term)
Write the rate equation for this reaction.
View full solution →(i) $NO + Br _2 \rightleftharpoons NOBr _2$ (fast term)
(ii) $NOBr _2+ NO \rightarrow 2 NOBr$ (slow term)
Write the rate equation for this reaction.
(a) The molecularity of the slow term of a complex reaction is the molecularity of entire reaction. Explain.
(b) High order reactions generally do not occur, why?
(b) High order reactions generally do not occur, why?
Determine the formula for the half life of a first order reaction and prove that the half life of a first order reaction does not depends on the initial concentration of the reactant.
Differentiate between order and molecularity of a reaction.
(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. $[\log 2=0.3010] \quad$
Derive the equation required for finding the activation energy.
Explain the energy distribution curve of gaseous molecules and also discuss the effect of temperature on it.
Explain the various methods of determining the order of a reaction.
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.
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