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 time required for $$80 \%$$ of a first order reaction is "$$y$$" times the half-life period of the same reaction. What is the value of "$$y$$"?
The rate constant for the reaction $$\mathrm{A} \rightarrow \mathrm{B}+\mathrm{C}$$ at $$500 \mathrm{~K}$$ is given as $$0.004 \mathrm{~s}^{-1}$$. At what temperature will the rate constant become $$0.014 \mathrm{~s}^{-1}$$ ? $$\mathrm{E}_{\mathrm{a}}$$ for the reaction is $$18.231 \mathrm{~kJ}$$.
For the reaction $$\mathrm{Cl}_{2(\mathrm{~g})}+2 \mathrm{NO}_{(\mathrm{g})} \rightarrow 2 \mathrm{NOCl}_{(\mathrm{g})}$$, the following data was obtained:
| Experiment No. | Initial concentration of $$\mathrm{Cl_2}$$ ($$\mathrm{M}$$) | Initial concentration of $$\mathrm{NO}$$ ($$\mathrm{M}$$) | Initial reaction rate ($$\mathrm{M}$$/min) |
|---|---|---|---|
| I | 0.15 | 0.15 | 0.60 |
| II | 0.30 | 0.15 | 1.20 |
| III | 0.15 | 0.3 | 2.40 |
| IV | 0.25 | 0.25 | 2.78 |
Identify the order of the reaction with respect to $$\mathrm{Cl}_2, \mathrm{NO}$$ and the value of Rate constant.