The heats of combustion of carbon and carbon | vedclass

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

Vedclass · Accepted Answer

$-110$

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(B) The heat of formation of $CO$ corresponds to the reaction: $C_{(s)} + \frac{1}{2} O_{2(g)} \rightarrow CO_{(g)}$.Given reactions:$1) C_{(s)} + O_{2(g)} \rightarrow CO_{2(g)}; \Delta H_1 = -393.5 \ kJ \ mol^{-1}$$2) CO_{(g)} + \frac{1}{2} O_{2(g)} \rightarrow CO_{2(g)}; \Delta H_2 = -283.5 \ kJ \ mol^{-1}$To obtain the target reaction,subtract equation $(2)$ from equation $(1)$:$(C_{(s)} + O_{2(g)}) - (CO_{(g)} + \frac{1}{2} O_{2(g)}) \rightarrow CO_{2(g)} - CO_{2(g)}$$C_{(s)} + \frac{1}{2} O_{2(g)} \rightarrow CO_{(g)}$Therefore,$\Delta H_f = \Delta H_1 - \Delta H_2 = -393.5 - (-283.5) = -110 \ kJ \ mol^{-1}$.

The heats of combustion of carbon and carbon monoxide are $-393.5 \ kJ \ mol^{-1}$ and $-283.5 \ kJ \ mol^{-1},$ respectively. The heat of formation (in $kJ \ mol^{-1}$) of carbon monoxide per mole is:

Similar Questions

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