The following data was recorded for the decomposition of XY compound at 750K
| [XY] mol / L | Rate of decomposition of XY mol / L s |
|---|---|
| 0.4 | $$5.5\times10^{-7}$$ |
| 0.8 | $$22.0\times10^{-7}$$ |
| 1.2 | $$49.5\times10^{-7}$$ |
What is the order of reaction with respect to decomposition of XY?
The Activation energy for the reaction $$A \rightarrow B+C$$, at a temperature $$\mathrm{TK}$$ was $$0.04606 \mathrm{~RT} \mathrm{~J} / \mathrm{mol}$$. What is the ratio of Arrhenius factor to the Rate constant for this reaction?
The temperature $$(\mathrm{T})$$ and rate constant $$(\mathrm{k})$$ for a first order reaction $$\mathrm{R} \rightarrow \mathrm{P}$$, was found to follow the equation $$\log \mathrm{k}=-(2000) \frac{1}{\mathrm{~T}}+8.0$$. The pre-exponential factor '$$\mathrm{A}$$' and activation energy $$\mathrm{E}_{\mathrm{a}}$$, respectively are: [Given: $$\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$$]
Given below a first order reaction in the gas phase
$$\mathrm{A}(\mathrm{g}) \rightarrow \mathrm{B}(\mathrm{g})+\mathrm{C}(\mathrm{g})$$
If the initial pressure of the system is $$\mathrm{P}_{\mathrm{i}}$$ and the total pressure at $$\mathrm{t}$$ seconds is $$\mathrm{P}_{\mathrm{t}}$$, the rate constant $$\mathrm{k}$$ for the reaction is: