If the electron affinity of Cl is 348 kJ/mol | vedclass

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(C) The molar mass of $Cl$ is $35.5 \ g/mol$.Given that the electron affinity $(EA)$ for $1 \ mole$ of $Cl$ is $348 \ kJ/mol$,this means $348 \ kJ$ of

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$9.8$

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(C) The molar mass of $Cl$ is $35.5 \ g/mol$.Given that the electron affinity $(EA)$ for $1 \ mole$ of $Cl$ is $348 \ kJ/mol$,this means $348 \ kJ$ of energy is released when $35.5 \ g$ of $Cl$ is converted into $Cl^-$ gas.To find the energy released for $1.0 \ g$ of $Cl$:$	ext{Energy} = \frac{348 \ kJ}{35.5 \ g} 	imes 1.0 \ g$$	ext{Energy} \approx 9.802 \ kJ$Therefore,the energy released is approximately $9.8 \ kJ$.

If the electron affinity of $Cl$ is $348 \ kJ/mol$,then how much energy is released to convert $1.0 \ g$ of $Cl$ into $Cl^-$ gas in $kJ$?

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