## Chemistry and Chemical Reactivity (9th Edition)

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: $131.58\ kJ/mol\times 8.33\times 10^4\ mol=10.95\times10^6\ kJ$