The half-life for a zero-order reaction having 0.02 M initial concentration of reactant is 100 s. The rate constant (in mol L^–1 s^–1) for the reaction is:

1. $1.0\times {10}^{-4}$

2. $2.0\times {10}^{-4}$

3. $2.0\times {10}^{-3}$

4. $1.0\times {10}^{-2}$

What does Z_AB represent in the collision theory of chemical reactions?

For a reaction A$\to$B, enthalpy of reaction is $-4.2$ $\mathrm{kJ}\hspace{0.17em}{\mathrm{mol}}^{-1}$ and enthalpy of activation is $9.6$ $\mathrm{kJ}\hspace{0.17em}{\mathrm{mol}}^{-1}$. The correct potential energy profile for the reaction is:

1.		2.
3.		4.

The slope of Arrhenius Plot (ln k v/s $\frac{1}{\mathrm{T}}$) of the first-order reaction is $-5\times {10}^3$ $\mathrm{K}$. The value of E_a of the reaction is:

[Given R = 8.314 JK^–1 mol^–1]

Find the quantity that increases when the concentration of reactants in a reaction is increased.

Which of the following is the time required to reduce the amount of a reactant from 2.0 g to 0.2 g for a first-order reaction with rate constant \(k = 4.606 \times 10^{-3} \, \text{s}^{-1}\)?

For a first-order reaction A \(\rightarrow\) Products, initial concentration of A is 0.1 M, which becomes 0.001 M after 5 minutes. Rate constant for the reaction in min^-1 is

For the reaction, 2A → B, rates= k[A]². If the concentration of reactant is doubled, then the:

Identify the set of correct statements & choose the correct answer from the options given below:

The plot of ln k vs \({1 \over T}\) for the following reaction, \(2N_2O_5(g) \rightarrow 4NO_2 (g) + O_2(g) \) gives a straight line with the slope of the line equal to \(-1.0 \times 10^4 K \).
What is the activation energy for the reaction in J mol^–1 ?
(Given: R = 8.3 J K^–1 mol^–1)