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:

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

True statement among the following is:

The correct expression for the rate of reaction given below is:
\(5 \mathrm{Br}^{-}(\mathrm{aq})+\mathrm{BrO}_3^{-}(\mathrm{aq})+6 \mathrm{H}^{+}(\mathrm{aq}) \rightarrow 3 \mathrm{Br}_2(\mathrm{aq})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{l})\)

The correct representation of an exothermic reaction is:

1.		2.
3.		4.	Both 1 and 2

Rate law for the reaction \(A+2 B \rightarrow C\) is found to be
Rate = k[A][B]
If the concentration of reactant 'B' is doubled, keeping the concentration of A constant, then the value of the rate of the reaction will  be:

An incorrect statement about the collision theory of chemical reaction is:

A first-order reaction is 50 % completed in 1.26 x 10¹⁴ s. The time required for 100 % completion
of the reaction will be:

1. 1.26 × 10¹⁵ s

2. 2.52 × 10¹⁴ s

3. 2.52 × 10²⁸ s

4. Infinite

An incorrect statement regarding the catalyst is: