On the basis of the following thermochemical data :

\left ( \Delta _{f}G^{0}H^{+}_{aq}= 0 \right ).

H_{2}O_{\left ( l \right )}\rightarrow H^{+}_{\left ( aq \right )}+OH^{-}_{\left ( aq \right )};\Delta H= 57.32 kJ

H_{2\left ( g \right )}+\frac{1}{2}O_{2(g)}\rightarrow H_{2}O\left ( l \right );\Delta H= -286 .2 kJ

The value of enthalpy of formation of OH^{-} ion at 25°C is

  • Option 1)

    – 22.88 kJ

  • Option 2)

    – 228.88 kJ

  • Option 3)

    + 228.88 kJ

  • Option 4)

    – 343.52 kJ

 

Answers (1)

As we learnt in

Heat of Reaction -

It is defined as the amount of  Enthalpy change in the reaction for given amount of reaction.

- wherein

C_{(s)}+O_{2(g)}\rightarrow CO_{2(g)}+393.5 KJ 

 

 H_{2} \:(g)+\frac{1}{2}O_{2}\:(g)\rightarrow H^{+} \:(aq)+OH^{-}\:(aq)\\ \Delta H_{1}^{o}=-228.88KJ


Option 1)

– 22.88 kJ

This option is incorrect 

Option 2)

– 228.88 kJ

This option is correct 

Option 3)

+ 228.88 kJ

This option is incorrect 

Option 4)

– 343.52 kJ

This option is incorrect 

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