A certain organic compound $\mathrm{A}$A decomposes by two parallel first order mechanism

 

If ${\mathrm{k}}_1:{\mathrm{k}}_2=1:9$ and ${\mathrm{k}}_1=1.3\times {10}^{-5}{ \mathrm{s}}^{-1}$

Calculate the concentration ratio of $\mathrm{C}$ to $\mathrm{A}$, if experiment is started with only $\mathrm{A}$ and allowed to run for one hour.

The catalytic decomposition of formic acid may take place in two ways :

(a) $\mathrm{HCOOH}={\mathrm{H}}_2\mathrm{O}+\mathrm{CO}$

(b) $\mathrm{HCOOH}={\mathrm{H}}_2+{\mathrm{CO}}_2$

The rate constant and activation energy for reaction (a) are $2.79\times {10}^{-3}{ \min }^{-1}$ at $236°\mathrm{C}$ and $12.0$ kcal ${\mathrm{mole}}^{-1}$ . respectively and for reaction (b) are $1.52\times {10}^{-4}{ \min }^{-1}$ at $237°\mathrm{C}$ and $24.5{\mathrm{kcalmole}}^{-1}$ respectively. Find the temperature which will give a product made up of equimolar quantities of water vapour, carbon monoxide, hydrogen and carbon dioxide.

For the following first order gaseous reaction

The initial pressure in a container of capacity $\mathrm{V}$ litres is $1 \mathrm{atm}$. Pressure at time $\mathrm{t}=10\sec$ is $1.4 \mathrm{atm}$ and after infinite time it becomes $1.5$ atmosphere. Find the rate constant ${\mathrm{k}}_1$ and ${\mathrm{k}}_2$ for the appropriate reactions.