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Standard XII

Chemistry

Ionization Energy and Electron Affinity

The electron ...

Question

The electron gain enthalpy of chlorine is 3.7 eV. How much energy in kcal is released when 2g of chlorine is completely converted to $C l^{-}$ ion in a gaseous state? ( 1eV = 23.06 kcal mol $^{- 1}$ )

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Solution

$C l + e \to C l^{-} + 3.7 e V$

Energy released for 1 mol (or 35.5g) $= 3.7 \times 23.06 k c a l / m o l$

$∴$ Energy released for conversion of 2g gaseous chlorine into $C l^{-}$ ions

$= \frac{3.7 \times 23.06}{35.5} \times 2 = 4.8 k c a l$

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The electron gain enthalpy of chlorine is 3.7 eV. How much energy in kcal is released when 2g of chlorine is completely converted to Cl− ion in a gaseous state? ( 1eV = 23.06 kcal mol−1 )

Cl+e→Cl−+3.7eVEnergy released for 1 mol (or 35.5g) =3.7×23.06 kcal/mol∴ Energy released for conversion of 2g gaseous chlorine into Cl− ions =3.7×23.0635.5×2=4.8 kcal

The electron gain enthalpy of chlorine is 3.7 eV. How much energy in kcal is released when 2g of chlorine is completely converted to $C l^{-}$ ion in a gaseous state? ( 1eV = 23.06 kcal mol $^{- 1}$ )

$C l + e \to C l^{-} + 3.7 e V$

Energy released for 1 mol (or 35.5g) $= 3.7 \times 23.06 k c a l / m o l$

$∴$ Energy released for conversion of 2g gaseous chlorine into $C l^{-}$ ions

$= \frac{3.7 \times 23.06}{35.5} \times 2 = 4.8 k c a l$