The enthalpy of combustion at 25,^{circ}C of | vedclass

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Question

(A) The combustion reactions are: $(i) \ H_2(g) + 1/2 O_2(g) 	o H_2O(l), \Delta H_1 = -241 \ kJ/mol$ $(ii) \ C_6H_{10}(l) + 17/2 O_2(g) 	o 6CO_2(g)

Vedclass · Accepted Answer

$-121$

Vedclass · Answer

(A) The combustion reactions are: $(i) \ H_2(g) + 1/2 O_2(g) 	o H_2O(l), \Delta H_1 = -241 \ kJ/mol$ $(ii) \ C_6H_{10}(l) + 17/2 O_2(g) 	o 6CO_2(g) + 5H_2O(l), \Delta H_2 = -3800 \ kJ/mol$ $(iii) \ C_6H_{12}(l) + 9O_2(g) 	o 6CO_2(g) + 6H_2O(l), \Delta H_3 = -3920 \ kJ/mol$ The hydrogenation reaction is: $C_6H_{10}(l) + H_2(g) 	o C_6H_{12}(l)$ This can be obtained by: $(i) + (ii) - (iii)$ $\Delta H_{hydrogenation} = \Delta H_1 + \Delta H_2 - \Delta H_3$ $\Delta H_{hydrogenation} = -241 + (-3800) - (-3920)$ $\Delta H_{hydrogenation} = -4041 + 3920 = -121 \ kJ/mol$.

The enthalpy of combustion at $25\,^{\circ}C$ of $H_2$,cyclohexene $(C_6H_{10})$ and cyclohexane $(C_6H_{12})$ are $-241$,$-3800$ and $-3920 \ kJ/mol$ respectively. The heat of hydrogenation of cyclohexene is.....$kJ/mol$.

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