$X_{(g)} ⟶ {X^{+}}_{(g)} + e^{-}$ , $Δ H = + 720 k J / m o l$ . Calculate the amount of energy required to convert $110 m g$ of ' $X$ ' atom in gaseous state into $X^{+}$ ion. (Atomic weight for $X = 7 g / m o l$ )

10.4 k J

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12.3 k J

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11.3 k J

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14.5 k J

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Solution

The correct option is D $11.3 k J$
For one mole of X (7 gm of X), required energy is 720 kJ/mol.
So, energy required for 110 mg of X $= (720 / 7) \times 0.110 = 11.3$ kJ.

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