Question

$X_{\left(g\right)}\to X_{\left(g\right)}^{+}+e^{-},\Delta H=+720kJmo{l}^{-1}$. Calculate the amount of energy required to convert 110 mg of ''X'' atom in gaseous state into $X^{+}$ ion. (Atomic wt. for X=7 g/mol)

• A. 10.4 kJ
• B. 12.3 kJ
• C. 11.3 kJ
• D. 14.5 kJ

Answer 1

Answer: (C)

11.3 kJ

Solution:- (C) $11.3kJ$

$X_{\left(g\right)}⟶{X^{+}}_{\left(g\right)}\Delta H=+720kJ/mol$

Given:-

At. wt. of $X=7g$

Given wt. of $X=110mg=0.11g$

No. of moles in $0.11g$ of $X=\frac{0.11}{7}\text{mole}$

Now from the given reaction,

Amount of energy required to convert $1$ mole of $X=720kJ$

Therefore,

Amount of energy required to convert $\frac{0.11}{7}$ mole of $X=720\times \frac{0.11}{7}=11.3kJ$

Hence the amount of energy required to convert $110mg$ of ''$X$'' atom in gaseous state into $X^{+}$ ion is $11.3kJ$.