The amount of heat evolved when 0.50 mole of $H C l$ is mixed with 0.30 mole of NaOH solution is :QUEUE

57.1 kJ

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28.55 kJ

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11.42 kJ

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17.13 kJ

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Solution

The correct option is A 17.13 kJ
0.50 mol of HCl $\equiv$ 0.50 mol of $H^{+}$ and 0.30 mol of NaOH $\equiv$ 0.30 mol of $O H^{-}$
$H^{+} + O H^{-} \to H_{2} O$ (Neutralisation Reaction)

Also, 0.30 mol of HCl $\equiv$ 0.30 mol of $H^{+}$

Since $O H^{-}$ is the limiting reagent here, 0.30 mol of $H^{+}$ reacts with 0.30 mol of $O H^{-}$ .

Heat evolved with 1 mol $H^{+} = 57.1 k J$ (Heat of neutralisation of $H^{+}$ and $O H^{-}$ ions)

Heat evolved with 0.30 mol $H^{+} = 57.1 \times 0.30 k J = 17.13 k J$

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The amount of heat evolved when 0.50 mole of HCl is mixed with 0.30 mole of NaOH solution is :QUEUE

The amount of heat evolved when 0.50 mole of $H C l$ is mixed with 0.30 mole of NaOH solution is :QUEUE