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Electron Gain Enthalpy

In the proces...

Question

In the process $C l_{(g)} + e^{-} Δ H - - \to C l^{-} (g), Δ H$ is :

A

positive

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B

negative

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C

zero

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D

none

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Solution

The correct option is D negative
$C l_{(g)} + e^{-} Δ H - - \to C l^{-}$
Chlorine has great affinity for electron to attain the stable gas configuration. If chlorine attains stability then it will release energy. So, $Δ H$ for the reaction will be negative.

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Similar questions

C l (g) + e^{-} Δ H - - \to C l^{-} (g)

In the above process

Δ H

Q. How much heat is liberated when one mole of gaseous

N a^{\oplus}

combines with one mole of

C l^{⊖}

ion to form solid

N a C l

Use the data given below:

N a (s) + \frac{1}{2} C l_{2} (g) ⟶ N a C l (s)

Δ H = - 98.23 k c a l

N a (s) ⟶ N a (g)

Δ H = + 25.98 k c a l

N a (g) ⟶ N a^{\oplus} + e^{-}

Δ H = + 120.0 k c a l

C l_{2} (g) ⟶ 2 C l (g)

Δ H = + 58.02 k c a l

C l^{⊖} (g) ⟶ C l (g) + e^{-}

Δ H = + 87.3 k c a l

Q. The first IE of lithium is

5.4

eV and first electron affinity of

C l

3.6

eV. The value of

Δ H

for the reaction

L i_{(g)} + C l_{(} g) \to L i_{(g)}^{+} + C l_{(g)}^{-}

Q. The first IP of lithium is

5.41 e V

and electron affinity of

C l

- 3.61 e V

Δ H

k J

{m o l}^{- 1}

for the reaction:

{L i}_{(g)} + {C l}_{(g)} \to {L i}_{(g)}^{+} + {C l}_{(g)}^{-}

I E

5.41 e V

and first electron affinity of

C l

3.61 e V

Δ H

(nearest integer value) in

k J {m o l}^{- 1}

for the reaction

L i (g) + C l (g) ⟶ {L i}^{+} (g) + {C l}^{-} (g)

[Take nearest integer]

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