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The amount of energy released when 1 xx1...

The amount of energy released when `1 xx10^10` atoms of chlorine in vapour state are converted to `Cl^(–1)` ions according to the equation, `Cl(g) + e^(-) to Cl^(-) (g) " is " 57.86 xx 10^(-10) J`
Calculate the electron gain enthalpy of chlorine atom in terms of `kJ "mol"^(–1 )` and eV per atom.

Text Solution

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For `10^10 ` atom `Cl_(g) + e^(-) to Cl^(-) , ` energy released ` = 57.86 xx 10^(-10) J`
For 1 atom ` rArr ` energy released ` = 57.86 xx 10^(-10) xx 10^(-10) J ` , energy released ` = 57.86 xx 10^(-20) J`
For 1 mole i.e. for ` 6.023 xx 10^23` atom energy released ` = 57.86 xx 10^(-20) xx 6.023 xx 10^23 J = 348.49 ` kJ/mole
energy released in eV ` = 57.86 xx N_A // 1.6 xx 10^(-19) xx 217.81 xx 10^22 eV `
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