List of top Chemistry Questions on Chemical Kinetics asked in UP Board XII

Does the half-life of a first-order reaction depend on the initial concentration of the reaction? Explain.
If the rate law of a reaction is Rate $= K[A]^2 [B]^0$, then what will be the order of the reaction?
In \( 2A \rightarrow \) Product, the reaction concentration of A remains 0.4 mol\(^{-1}\) from 0.5 mol\(^{-1}\) in 10 minutes.
Calculate the velocity of reaction for this period of time.
Prove that the time taken to complete 99.9% reaction is ten times the half-life period $(t_{1/2})$ for a first-order reaction.
Explain order and molecularity of a reaction giving example.
Explain the rate of reaction. Describe the order of reaction with example.
The rate constant for a first–order reaction is $60\ \mathrm{s^{-1}$. How much time will it take to reduce the initial concentration of the reactant to $\dfrac{1}{16}$th?}
Explain with example the difference between molecularity and order of reaction.
Decomposition of NH$_3$ on the surface of platinum is a zero–order reaction. What will be the rate of formation of N$_2$ and H$_2$? \; (Given: $k=2.5\times10^{-4}\ \mathrm{mol\,L^{-1}\,s^{-1}}$)
Write unit of first order reaction. The initial concentration of N$_2$O$_5$ at 318 K was $0.60\times 10^{-2$ mol L$^{-1}$ in the first order reaction, which became $0.20\times 10^{-2}$ mol L$^{-1}$ after 60 min. Calculate the velocity constant at 318 K. (log 3 = 0.4771).}
A first order reaction completes 20% in 10 minutes. Calculate the time taken for 75% completion.
How do the following factors affect the velocity of reaction? (i) Concentration
(ii) Temperature
(iii) Catalyst
Differentiate between:
(x) Order of a reaction and molecularity
(y) Average and instantaneous velocity
Explain the molecularity of reaction with example.
Explain the zero order of reaction by giving examples.
Explain the effect of temperature and concentration on the velocity of a reaction.
For the reaction \( \frac{1}{2} A \rightarrow 2B \), rate of dissociation of \( A \) and rate of formation of \( B \) is related as follows:
Explain velocity (rate) constant of a reaction.
State the difference between molecularity of a reaction and order of a reaction. Write the velocity equation for the reaction \( H_2(g) + Cl_2(g) \rightarrow 2HCl(g) \), which is a zero-order reaction.
The true statement for the formula \( K = Ae^{-E_a / RT} \) is:
Velocity constant for a first order reaction is \( 2 \times 10^{-3} \, \text{s}^{-1} \). The half-life period for this reaction is
The velocity constant for the first order reaction is $6.93 \times 10^{-3}$ min$^{-1}$. Calculate the half-life of this reaction.
The initial concentration of N$_2$O$_5$ in the following first order reaction $N_2O_5(g) \longrightarrow 2NO_2(g) + \tfrac{1}{2} O_2(g)$ was $1.24 \times 10^{-2}$ mol L$^{-1}$ at 318 K. The concentration of N$_2$O$_5$ after 60 minutes was $0.20 \times 10^{-2}$ mol L$^{-1}$. Calculate the rate constant of the reaction at 318 K.
In a first order reaction the concentration of a substance gets dissociated by 99% of the initial concentration in 100 minutes. Calculate the velocity constant of the reaction.
Write the formula of half-life period for first order reaction.