MCQ
$\Delta H^o_f$ of water is $-285.5\, kJ\, mol^{-1}$. if enthalpy of neutralisation of monoacidic strong base is $-57.3\, kJ\, mol^{-1}$, $\Delta H_f^o$ of $OH^-$ ion will be.....$kJ\, mol^{-1}$
- ✓$-228.2$
- B$228.5$
- C$114.5$
- D$-114.5$
✓
Answer
Correct option: A.
$-228.2$
a
$\mathrm{H}_{2}+\frac{1}{2} \mathrm{O}_{2} \rightarrow \mathrm{H}_{2} \mathrm{O} \quad \Delta \mathrm{H}_{1}=-285.5$
$\mathrm{H}_{2}+\frac{1}{2} \mathrm{O}_{2} \rightarrow \mathrm{H}_{2} \mathrm{O} \quad \Delta \mathrm{H}_{1}=-285.5$
$\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{H}^{+}+\mathrm{OH}^{-} \quad \Delta \mathrm{H}_{2}=+57.3$
$\mathrm{H}_{2}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{H}^{+}(\mathrm{aq})+\mathrm{OH}(\mathrm{aq}) \cdot \Delta \mathrm{H}=\Delta \mathrm{H}_{1}+\Delta \mathrm{H}_{2}$
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