The role of a catalyst is to change: 

1. Gibbs energy of the reaction

2. Enthalpy of reaction

3. The activation energy of the reaction 

4. Equilibrium constant

In the presence of a catalyst, the heat evolved or absorbed during the reaction: 

1. Increases.

2. Decreases.

3. Remains unchanged.

4. May increase or decrease.

The activation energy of a chemical reaction can be calculated by:

1. Determining the rate constant at standard temperature.

2. Determining the rate constant at two temperatures.

3. Determining probability of collision.

4. Using the catalyst.

The correct statement based on the graph below is:

Consider the first-order gas-phase decomposition reaction given below.

A(g) → B(g) + C(g)

The initial pressure of the system before the decomposition of A was ${\mathrm{P}}_{\mathrm{i}}$. After the lapse of time t, the total pressure of the system increased by X units and became ${\mathrm{P}}_{\mathrm{t}}$. The rate constant k for the reaction is:

1. $\mathrm{k}=\frac{2.303}{\mathrm{t}}\log \frac{P_{\mathrm{i}}}{P_{\mathrm{i}}-\mathrm{x}}$

2. $\mathrm{k}=\frac{2.303}{\mathrm{t}}\log \frac{P_{\mathrm{i}}}{2P_{\mathrm{i}}-P_{\mathrm{t}}}$

3. $\mathrm{k}=\frac{2.303}{\mathrm{t}}\log \frac{P_{\mathrm{i}}}{2P_{\mathrm{i}}+P_{\mathrm{t}}}$

4. $\mathrm{k}=\frac{2.303}{\mathrm{t}}\log \frac{P_{\mathrm{i}}}{P_{\mathrm{i}}+\mathrm{x}}$

The correct graphical representation of relation between ln k and 1/T is:

1.		2.
3.		4.

Consider the Arrhenius equation given below and choose the correct option:

$k=A{e}^{-\frac{E_a}{RT}}$

A graph of volume of hydrogen released vs time for the reaction between zinc and dil. HCl is given in the graph below. 

The correct statement among the following based on the graph given above is:

$$\begin{gathered} 1. \mathrm{Average} \mathrm{rate} \mathrm{upto} 40s\text{ is }\frac{V_3-V_2}{40} \\ 2. \mathrm{Average} \mathrm{rate} \mathrm{upto} 40s\text{ is }\frac{V_3-V_2}{40-30} \\ 3. \mathrm{Average} \mathrm{rate} \mathrm{upto} 40s\text{ is }\frac{V_3}{40} \\ 4. \mathrm{Average} \mathrm{rate} \mathrm{upto} 40s\text{ is }\frac{V_3-V_1}{40-20} \end{gathered}$$

Which of the following statements is not correct about the order of a reaction?

Consider the graph given in the figure. Which of the following options does not show an instantaneous rate of reaction in the 40s?

$\begin{array}{llll}\text{ 1 }\frac{V_5-V_2}{50-30}& \text{ 2 }\frac{V_4-V_2}{50-30}& \text{ 3 }\frac{V_3-V_2}{40-30}& \text{ 4 }\frac{V_3-V_1}{40-20}\end{array}$