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Standard XIII

Chemistry

Electron Affinity

The electron ...

Question

The electron gain enthalpy of chlorine is $- 349 k J m o l^{- 1}$ . How much energy in $k J$ is released when $3.55 g$ of chlorine is converted completely into $C l^{- 1}$ ion in the gaseous state?
34.9

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Solution

The correct option is A 34.9
Electron gain enthalpy of chlorine is $- 349 kJ / mol$
it means, $349 k J$ energy is released when $1$ mole of chlorine is converted into $C l^{-}$ ion in the gaseous state.
so energy released when $3.55 g$ of chlorine is converted into $C l^{-}$ ion , $E = 349 \times$ no of moles of Cl
$= 349 \times (\frac{3.55 g}{35.5 g / m o l})$
$= 34.9 k J$
Therefore, $34.9 k J$ energy is released when $3.55 g$ of chlorine is converted completely into $C l^{-}$ ion in the gaseous state.

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The electron gain enthalpy of chlorine is –349 kJ mol−1. How much energy in kJ is released when 3.55 g of chlorine is converted completely into Cl−1 ion in the gaseous state? 34.9

The electron gain enthalpy of chlorine is $- 349 k J m o l^{- 1}$ . How much energy in $k J$ is released when $3.55 g$ of chlorine is converted completely into $C l^{- 1}$ ion in the gaseous state?
34.9