The heat of neutralisation of a strong acid and a strong alkali is $57.0$ $k J m o l^{- 1}$ . The heat released when $0.5$ mole of $H N O_{3}$ solution is mixed with $0.2$ mole of KOH is:

57.0 k J

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11.4 k J

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28.5 k J

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34.9 k J

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Solution

The correct option is C $11.4 k J$
$0.2$ mole of KOH will neutralise $0.2$ mole of $H N O_{3}$ .

$H N O_{3} + K O H ⟶ K N O_{3} + H_{2} O$

Thus, heat evolved $= 57 \times 0.2 = 11.4 k J$ .

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The heat of neutralisation of a strong acid and a strong alkali is 57.0 kJmol−1. The heat released when 0.5 mole of HNO3 solution is mixed with 0.2 mole of KOH is:

The correct option is C 11.4 kJ0.2 mole of KOH will neutralise 0.2 mole of HNO3.HNO3+KOH⟶KNO3+H2OThus, heat evolved =57×0.2=11.4 kJ.

The heat of neutralisation of a strong acid and a strong alkali is $57.0$ $k J m o l^{- 1}$ . The heat released when $0.5$ mole of $H N O_{3}$ solution is mixed with $0.2$ mole of KOH is:

The correct option is C $11.4 k J$
$0.2$ mole of KOH will neutralise $0.2$ mole of $H N O_{3}$ .

$H N O_{3} + K O H ⟶ K N O_{3} + H_{2} O$

Thus, heat evolved $= 57 \times 0.2 = 11.4 k J$ .