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?

1. The fraction of molecules with energies greater than E_a

2. The collision frequency of reactants, A and B

3. Steric factor

4. The fraction of molecules with energies equal to E_a

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]

An increase in the concentration of the reactants of a reaction leads to a change in:

1. heat of reaction

2. threshold energy

3. collision frequency

4. activation energy

The rate constant for a first order reaction is $4.606\times {10}^{-3} s^{-1}$. The time required to reduce 2.0 g of the reactant to 0.2 g is:

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 \(-1.0 \times 10^4 K \).
The activation energy for the reaction in J mol^-1 is:
(Given R = 8.3 J K^-1 mol^-1)

1. \(4.0 \times 10^2 \)
2. \(4.0 \times 10^{-2} \)
3. \(8.3 \times 10^{-4} \)
4. \(8.3 \times 10^4 \)