Molar enthalpy of combustion of C_2H_{2(g)},C | vedclass

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(D) The formation reaction for $C_2H_{2(g)}$ is: $2C_{(s)} + H_{2(g)} \rightarrow C_2H_{2(g)}$$\Delta H_f^{\circ} = \Sigma \Delta H_{combustion}^{\cir

Vedclass · Accepted Answer

$+226 \ kJ/mol$

Vedclass · Answer

(D) The formation reaction for $C_2H_{2(g)}$ is: $2C_{(s)} + H_{2(g)} ightarrow C_2H_{2(g)}$$\Delta H_f^{\circ} = \Sigma \Delta H_{combustion}^{\circ}(	ext{reactants}) - \Sigma \Delta H_{combustion}^{\circ}(	ext{products})$$\Delta H_f^{\circ} = [2 	imes \Delta H_c^{\circ}(C_{(s)}) + 1 	imes \Delta H_c^{\circ}(H_{2(g)})] - [1 	imes \Delta H_c^{\circ}(C_2H_{2(g)})]$$\Delta H_f^{\circ} = [2 	imes (-394) + (-286)] - (-1300)$$\Delta H_f^{\circ} = [-788 - 286] + 1300$$\Delta H_f^{\circ} = -1074 + 1300 = +226 \ kJ/mol$

Molar enthalpy of combustion of $C_2H_{2(g)}$,$C_{(s)}$,and $H_{2(g)}$ are $-1300$,$-394$,and $-286 \ kJ/mol$ respectively. The standard enthalpy of formation of $C_2H_{2(g)}$ is $:$

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