The heat of reaction for C _ 10 H _ 8 (s) + 12 O _ 2 (g) ⟶ 10 CO _...

Heat of reaction at constant pressure is represented by& ΔH

Heat of reaction at constant volume is represented by& ΔU

${C}_{10}{H}_{8}\left(s\right) + 12{O}_{2}\left(g\right) ⟶ 10{CO}_{2}\left(g\right) + 4{H}_{2}O$

We known that $\Delta H = \Delta E + {Δn}_{g}RT$

${Δn}_{g} = 10 - 12 = - 2$

$\Delta H = - 1228. 2 \times {10}^{3} + \left(- 2\right) \times 2 \times 298$

$= - 1229393Cal$

$= - 1229. 39kcal$