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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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The amount of energy released when one mole `(6.022 xx 10^(23))` atoms of chlorine are converted into ions
`=((57.86 xx 10^(-10)J)xx 6.022 xx 10^(25))/(1 xx 10^(10))=348.4 xx 10^(3)J" mol"^(-1)= 348.4" kJ mol"^(-1)`
Electron gain enthalpy in eV per atom `=(1eV//"atom")/((96.47kJ mol^(-1))xx (-3.48.4 xx kJ mol^(-1)))=-3.61 eV//atom`
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