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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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