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(A) To find the value of $x$ for the reaction $C_{(s)} + O_{2(g)} \rightarrow CO_{2(g)}$,we can use Hess's Law by adding the given equations:$(1) H_2O

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$-393 \ kJ$

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(A) To find the value of $x$ for the reaction $C_{(s)} + O_{2(g)} \rightarrow CO_{2(g)}$,we can use Hess's Law by adding the given equations:$(1) H_2O_{(g)} + C_{(s)} \rightarrow CO_{(g)} + H_{2(g)} ; \Delta H_1 = 131 \ kJ$$(2) CO_{(g)} + \frac{1}{2} O_{2(g)} \rightarrow CO_{2(g)} ; \Delta H_2 = -282 \ kJ$$(3) H_{2(g)} + \frac{1}{2} O_{2(g)} \rightarrow H_2O_{(g)} ; \Delta H_3 = -242 \ kJ$Adding equations $(1)$,$(2)$,and $(3)$:$H_2O_{(g)} + C_{(s)} + CO_{(g)} + \frac{1}{2} O_{2(g)} + H_{2(g)} + \frac{1}{2} O_{2(g)}$ $\rightarrow CO_{(g)} + H_{2(g)} + CO_{2(g)} + H_2O_{(g)}$Canceling common terms on both sides gives:$C_{(s)} + O_{2(g)} \rightarrow CO_{2(g)}$Therefore,$x = \Delta H_1 + \Delta H_2 + \Delta H_3 = 131 + (-282) + (-242) = -393 \ kJ$.

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Assertion $(A)$: Formation of $H_2O_{(\ell)}$ from $H_{2(g)}$ and $O_{2(g)}$ is more exothermic than formation of $H_2O_{(g)}$ from $H_{2(g)}$ and $O_{2(g)}$.
Reason $(R)$: $H_2O_{(\ell)}$ has more attraction force than $H_2O_{(g)}$ and it is more stable than $H_2O_{(g)}$.

At $25^{\circ} \text{C}$, the standard enthalpies of combustion of $H_2(g)$, cyclohexene $(C_6H_{10})$, and cyclohexane $(C_6H_{12})$ are $-241 \text{ kJ mol}^{-1}$, $-3800 \text{ kJ mol}^{-1}$, and $-3920 \text{ kJ mol}^{-1}$ respectively. Calculate the heat of hydrogenation of cyclohexene.

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