Given the following data:
Reaction Energy Change (in $kJ$) $Li_{(s)} \to Li_{(g)}$ $161$ $Li_{(g)} \to Li^{+}_{(g)}$ $520$ $\frac{1}{2} F_{2(g)} \to F_{(g)}$ $77$ $F_{(g)} + e^- \to F^{-}_{(g)}$ (Electron gain enthalpy) $Li^{+}_{(g)} + F^{-}_{(g)} \to LiF_{(s)}$ $-1047$ $Li_{(s)} + \frac{1}{2} F_{2(g)} \to LiF_{(s)}$ $-617$
Based on the data provided,the value of electron gain enthalpy of fluorine would be $kJ\ mol^{-1}$.
| Reaction | Energy Change (in $kJ$) |
| $Li_{(s)} \to Li_{(g)}$ | $161$ |
| $Li_{(g)} \to Li^{+}_{(g)}$ | $520$ |
| $\frac{1}{2} F_{2(g)} \to F_{(g)}$ | $77$ |
| $F_{(g)} + e^- \to F^{-}_{(g)}$ | (Electron gain enthalpy) |
| $Li^{+}_{(g)} + F^{-}_{(g)} \to LiF_{(s)}$ | $-1047$ |
| $Li_{(s)} + \frac{1}{2} F_{2(g)} \to LiF_{(s)}$ | $-617$ |
Based on the data provided,the value of electron gain enthalpy of fluorine would be $kJ\ mol^{-1}$.
- A$-300$
- B$-350$
- C$-328$
- D$-228$
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$(iii) \ KOH_{(s)} + aq \rightarrow KOH_{(aq)} ; \Delta H = -14.0 \, kcal$
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