Consider the following single step reaction in gas phase at constant temperature. $2 \mathrm{~A}_{(\mathrm{g})}+\mathrm{B}_{(\mathrm{g})} \rightarrow \mathrm{C}_{(\mathrm{g})}$ The initial rate of the reaction is recorded as $\mathrm{r}_1$ when the reaction starts with $1.5 \mathrm{~atm}$…

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Consider the following single step reaction in gas phase at constant temperature. $2 \mathrm{~A}_{(\mathrm{g})}+\mathrm{B}_{(\mathrm{g})} \rightarrow \mathrm{C}_{(\mathrm{g})}$ The initial rate of the reaction is recorded as $\mathrm{r}_1$ when the reaction starts with $1.5 \mathrm{~atm}$ pressure of $\mathrm{A}$ and $0.7 \mathrm{~atm}$ pressure of $\mathrm{B}$. After some time, the rate $\mathrm{r}_2$ is recorded when the pressure of $\mathrm{C}$ becomes $0.5 \mathrm{~atm}$. The ratio $\mathrm{r}_1: \mathrm{r}_2$ is ______ $\times 10^{-1}$. (Nearest integer)

Aicharya · Accepted Answer

$2 \mathrm{~A}(\mathrm{~g})+\mathrm{B}(\mathrm{g}) \longrightarrow \mathrm{C}(\mathrm{g})$
$\begin{array}{ll} \mathrm{r}_1 & 1.5 \mathrm{~atm} \quad 0.7 \mathrm{~atm} \\ \mathrm{r}_2 & 0.5 \mathrm{~atm} \quad 0.2 \mathrm{~atm} \quad 0.5 \mathrm{~atm} \\ & \because \mathrm{r}=\mathrm{K}\left[\mathrm{P}_{\mathrm{A}}\right]^2\left[\mathrm{P}_{\mathrm{B}}\right] \\ & \mathrm{r}_1=\mathrm{K}[1.5]^2[0.7] \\ & \mathrm{r}_2=\mathrm{K}[0.5]^2[0.2] \\ & \frac{\mathrm{r}_1}{\mathrm{r}_2}=9 \times \frac{7}{2}=31.5=315 \times 10^{-1} \end{array}$ Ans. 315

Consider the following single step reaction in gas phase at constant temperature. \(2…

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