Methane and water vapor are converted into hydrogen and carbon monoxide

in a catalytic reactor at $1$atm. The $C\frac{H_4}{H_2}O$ ratio in the feed stream is $0\mathrm{.}5$ and

the feed temperature is $105C.$ When the product outlet temperature is $900C,$

complete conversion of methane is achieved. Assuming that the heat loss to

the environment is $6\%$ of the total heat energy, calculate the heat $(kJ)$ required

for $1000\frac{m^3}{?}$ day hydrogen production.

$C{H}_4+H_{2}O(g)CO+3H_2$