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  • For the reaction : <img alt="\mathrm{Ag_{2}O\left ( s \right )\rightarrow 2Ag\left ( s \right )+\frac{1}{2}O_{2}\left ( g \right )}" src="https://entrancecorner.oncodecogs.com/gif.latex?%

For the reaction : \mathrm{Ag_{2}O\left ( s \right )\rightarrow 2Ag\left ( s \right )+\frac{1}{2}O_{2}\left ( g \right )}

The \mathrm{\Delta H} and \mathrm{\Delta S} are \mathrm{30\; kJ/mol}  and \mathrm{60\; J/K.mol}  respectively. Calculate the temperature (in oC) at which the Gibb’s free energy change for the reaction will be zero. 

Option: 1

120


Option: 2

227


Option: 3

500


Option: 4

600


Answers (1)

best_answer

As we have learnt,

\mathrm{\Delta G=\Delta H-T\Delta S}

According to question,

\mathrm{0=\Delta H-T\Delta S}

\mathrm{T=\frac{\Delta H}{\Delta S}}

\mathrm{T=500\; K=227^{\circ}C}

 

Posted by

seema garhwal

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