Consider the following reaction:C_{(s)} + O_{ | vedclass

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(C) The heat of formation of $CO_{(g)}$ corresponds to the reaction: $C_{(s)} + \frac{1}{2}O_{2(g)} 	o CO_{(g)}$.Given:$(1) \ C_{(s)} + O_{2(g)} 	o

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$ (y - x) \ kJ/mol $

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(C) The heat of formation of $CO_{(g)}$ corresponds to the reaction: $C_{(s)} + \frac{1}{2}O_{2(g)} 	o CO_{(g)}$.Given:$(1) \ C_{(s)} + O_{2(g)} 	o CO_{2(g)} \quad \Delta H = -x \ kJ/mol$$(2) \ CO_{(g)} + \frac{1}{2}O_{2(g)} 	o CO_{2(g)} \quad \Delta H = -y \ kJ/mol$Subtracting equation $(2)$ from equation $(1)$:$(C_{(s)} + O_{2(g)}) - (CO_{(g)} + \frac{1}{2}O_{2(g)}) = CO_{2(g)} - CO_{2(g)}$$C_{(s)} + \frac{1}{2}O_{2(g)} - CO_{(g)} = 0$$C_{(s)} + \frac{1}{2}O_{2(g)} 	o CO_{(g)}$The enthalpy change for this reaction is $\Delta H = (-x) - (-y) = (y - x) \ kJ/mol$.

Consider the following reaction:
$C_{(s)} + O_{2(g)} \to CO_{2(g)} + x \ kJ$
$CO_{(g)} + \frac{1}{2}O_{2(g)} \to CO_{2(g)} + y \ kJ$
The heat of formation of $CO_{(g)}$ is:

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Consider the following reaction:$C_{(s)} + O_{2(g)} \to CO_{2(g)} + x \ kJ$$CO_{(g)} + \frac{1}{2}O_{2(g)} \to CO_{2(g)} + y \ kJ$The heat of formation of $CO_{(g)}$ is: