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?

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

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: