Answer
See answer below.
Work Step by Step
a) Enthalpies of formation:
$H_2O(g): -241.83, CO(g): -110.525$
Enthalpy change:
$-110.525- -241.83=+131.58\ kJ/mol$
b) Since $\Delta H_r\gt0$, it's an endothermic reaction.
c) Number of moles of carbon:
$1\times10^6\ g\div 12.011\ g/mol=8.33\times 10^4\ mol$
Heat required:
$131.58\ kJ/mol\times 8.33\times 10^4\ mol=10.95\times10^6\ kJ$
