In the presence of a catalyst at a given temperature of $$27^{\circ} \mathrm{C}$$, the Activation energy of a specific reaction is reduced by $$100 \mathrm{~J} / \mathrm{mol}$$. What is the ratio between the rate constants for the catalysed $$(\mathrm{k}_2)$$ and uncatalysed $$(\mathrm{k}_1)$$ reactions?
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 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 "$$y$$"?