For the reaction, $2A \rightarrow B$, $\text{rate} = k[A]^2$. If the concentration of reactant is doubled, then the: (a) rate of reaction will be doubled. (b) rate constant will remain unchanged, however rate of reaction is directly proportional to the rate constant. (c) rate constant will change since the rate of reaction and rate constant are directly proportional to each other. (d) rate of reaction will increase by four times. Identify the set of correct statements and choose the correct answer from the options given below:

If the half-life is independent of its initial concentration, then the order of the reaction is:

Which quantity is altered when a catalyst is introduced during a chemical reaction?

The rate of the reaction $2NO + Cl_2 \rightarrow 2NOCl$ is given by the rate equation $\text{rate} = k[NO]^2[Cl_2]$. The value of the rate constant can be increased by:

The rate of a first-order reaction is $1.5 \times 10^{-2} \text{ mol L}^{-1} \text{ min}^{-1}$ at $0.5 \text{ M}$ concentration of the reactant. The half-life of the reaction is:

The activation energy of a reaction can be determined from the slope of the graph between:

The plot of $\ln k$ vs $1/T$ 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 $-1.0 \times 10^4 \text{ K}$. What is the activation energy for the reaction in $\text{J mol}^{–1}$? (Given: $R = 8.3 \text{ J K}^{–1} \text{ mol}^{–1}$)

Consider the reaction $N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)$. The equality relationship between $\frac{d[NH_3]}{dt}$ and $-\frac{d[H_2]}{dt}$ is:

For a chemical reaction, $4A + 3B \rightarrow 6C + 9D$ rate of formation of C is $6 \times 10^{–2} \text{ mol L}^{–1} \text{ s}^{–1}$ and rate of disappearance of A is $4 \times 10^{–2} \text{ mol L}^{–1} \text{ s}^{–1}$. The rate of reaction and amount of B consumed in interval of 10 seconds, respectively will be: