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(A) The chemical equation for the hydrogenation of ethene is: $CH_2=CH_2 + H_2 \rightarrow CH_3-CH_3$ From the stoichiometry,$1 \ mole$ of ethene ($C_

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$0.2$

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(A) The chemical equation for the hydrogenation of ethene is: $CH_2=CH_2 + H_2 ightarrow CH_3-CH_3$ From the stoichiometry,$1 \ mole$ of ethene ($C_2H_4$,molar mass $28 \ g/mol$) produces $1 \ mole$ of ethane ($C_2H_6$,molar mass $30 \ g/mol$). The molar mass of ethane $(C_2H_6)$ is $(2 	imes 12) + (6 	imes 1) = 30 \ g/mol$. To prepare $6.0 \ g$ of ethane,the number of moles of ethane required is $n = \frac{mass}{molar \ mass} = \frac{6.0 \ g}{30 \ g/mol} = 0.2 \ mol$. Since $1 \ mole$ of ethene produces $1 \ mole$ of ethane,$0.2 \ mole$ of ethene is required to produce $0.2 \ mole$ of ethane.

How many moles of ethene are required to prepare $6.0 \ g$ of ethane by the hydrogenation process (in $mole$)?

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