Consider the reaction:
\[ A \rightarrow B + C \]
Initial pressures:
\[ P_i \quad 0 \quad 0 \]
After reaction:
\[ P_i - x \quad x \quad x \]
Total pressure at time \(t\):
\[ P_t = P_i + x \]
Therefore:
\[ P_i - x = P_i - P_t + P_i \] \[ = 2P_i - P_t \]
Hence,
\[ k = \frac{2.303}{t}\times \log \frac{P_i}{2P_i - P_t} \]
A(g) $ \rightarrow $ B(g) + C(g) is a first order reaction.
The reaction was started with reactant A only. Which of the following expression is correct for rate constant k ?
Rate law for a reaction between $A$ and $B$ is given by $\mathrm{R}=\mathrm{k}[\mathrm{A}]^{\mathrm{n}}[\mathrm{B}]^{\mathrm{m}}$. If concentration of A is doubled and concentration of B is halved from their initial value, the ratio of new rate of reaction to the initial rate of reaction $\left(\frac{\mathrm{r}_{2}}{\mathrm{r}_{1}}\right)$ is
For $\mathrm{A}_{2}+\mathrm{B}_{2} \rightleftharpoons 2 \mathrm{AB}$ $\mathrm{E}_{\mathrm{a}}$ for forward and backward reaction are 180 and $200 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively. If catalyst lowers $\mathrm{E}_{\mathrm{a}}$ for both reaction by $100 \mathrm{~kJ} \mathrm{~mol}^{-1}$. Which of the following statement is correct?
Match List-I with List-II: List-I