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The enthalpy of combustion of cyclohexane, cyclohexene and $H_2$ are respectively -3920, -3800 and -241 kJ/mol. The heat of hydrogenation of cyclohexane is


(a) -121 kJ/mol
(b) +121 kJ/mol
(c) -242 kJ/mol
(d) +242 kJ/mol

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Answer: -121 kJ/mol
$C_6H_{12} + 9 O_2 \rightarrow 6CO_2 + 6H_2O$ ; $\Delta H_1= -3920$ kJ/mol
$C_6H_{10} + \frac{17}{2} O_@ \rightarrow 6 CO_2 + 5H_2O$ ; $\Delta H_2 = -3800$ kJ/mol
$H_2 + \frac{1}{2}O_2 \rightarrow H_2O$ ; $\Delta H_3 = -241$ kJ/mol
Now operate as, ($\Delta H_2 + \Delta H_3 - \Delta H_1$) will give the value of $\Delta H$ for the reaction
$C_6H_10 + H_2 \rightarrow C_6H_12$ ; $\Delta H = -121 $ kJ/mol
answered Feb 28, 2014 by mosymeow_1
 

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