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Q.

The enthalpy of combustion at 25⁰C of H₂(g) cyclohexane ( $l$ ) and cyclohexene( $l$ ) are -241, -3920 and -3800KJ/mol respectively. The enthalpy of hydrogenation of cyclohexene ( $l$ ) is

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a

+121KJ/mol

b

-121KJ/mol

c

-242KJ/mol

d

+242/KJ/mol

answer is A.

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Detailed Solution

$Δ {H_{r}}_{(H y d r o g e n a t i o n)} = \sum Δ H_{C o m b u s t i o n o f r e a c \tan t s} - \sum Δ H_{\begin{array}{l} C o m b u s t i o n o f products \end{array}}$
$Δ H = Δ H_{c o m b (C_{6} H_{10})} + Δ H_{c o m b (H_{2})} - Δ H_{c o m b (C_{6} H_{12})}$
$C_{6} H_{10} + H_{2} \to C_{6} H_{12} Δ H = ?$
$= (- 3800) + (- 241) - (- 3920) = - 121 KJ / mole$

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The enthalpy of combustion at 250C of H2(g) cyclohexane (l ) and cyclohexene( l) are -241, -3920 and -3800KJ/mol respectively. The enthalpy of hydrogenation of cyclohexene ( l) is