Carbon dioxide $(C{O}_2)$ and water $(H_{2}O)$ is produced from the reaction of methane gas $(C{H}_4)$ with oxygen

gas $(O_2).$

$C{H}_4+2O_{2}C{O}_2+2H_{2}O$

The isothermal and isobaric irreversible reaction consisting of $25mo{l}_{C}C{H}_4,50$mol$\%O_2$ and the balance

nitrogen gas $(N_2)$ is carried out in a $45\mathrm{.}0L$ batch reactor at $500K$ initially. The initial partial pressure of

$C{H}_4$ is $82\mathrm{.}0$atm. From a prior study, it is determined that the reaction obeys elementary rate law. Given

the reaction rate constant as $10\mathrm{.}0\frac{L^2}{m}o{l}^2.$ min at $800K$ with activation energy of $20\mathrm{.}000\frac{J}{m}o{l}^{.}C{H}_4$ must

be used as the basis of calculations.

a$.$ Construct a stoichiometric table for the above reaction. All values should be in function of conversion,

$x$ only by evaluating numerically all other symbols $($e$.$g$.,,).$

b$.$ Determine the rate of disappearance of $C{O}_2$ if the conversion is $50$

note : write the answer in steps and details please