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(C) The hydrogenation of benzene $(C_6H_6)$ requires $3 	ext{ equivalents}$ of $H_2$ to fully reduce it to cyclohexane $(C_6H_{12})$.$C_6H_6 + 3H_2 \

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$A$ mixture of $0.66 	ext{ eqv. of } C_6H_6$ and $0.33 	ext{ eqv. of cyclohexane}$.

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(C) The hydrogenation of benzene $(C_6H_6)$ requires $3 	ext{ equivalents}$ of $H_2$ to fully reduce it to cyclohexane $(C_6H_{12})$.$C_6H_6 + 3H_2 ightarrow C_6H_{12}$In this reaction, we are given $1 	ext{ equivalent}$ of benzene and only $1 	ext{ equivalent}$ of $H_2$.Since the stoichiometry requires $3 	ext{ equivalents}$ of $H_2$ for $1 	ext{ equivalent}$ of benzene, $1 	ext{ equivalent}$ of $H_2$ will react with $1/3$ $(0.33)$ of the benzene molecules to fully reduce them to cyclohexane, while $2/3$ $(0.66)$ of the benzene molecules will remain unreacted.Therefore, the final mixture will contain $0.66 	ext{ equivalents}$ of unreacted benzene and $0.33 	ext{ equivalents}$ of cyclohexane.

The product of the following hydrogenation reaction is:
$C_6H_6 + H_2 \xrightarrow{\text{Catalyst, High temperature and pressure}} ?$
Given: $1 \text{ eqv. of } C_6H_6$ and $1 \text{ eqv. of } H_2$.

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The product of the following hydrogenation reaction is:$C_6H_6 + H_2 \xrightarrow{\text{Catalyst, High temperature and pressure}} ?$Given: $1 \text{ eqv. of } C_6H_6$ and $1 \text{ eqv. of } H_2$.