The temperature at which the reaction,Ag2O(s) → 2Ag(s) + 1/2O2(g)Is at equilibrium is …..; Given ∆H=30.5 kJ mol-1 and ∆S=0.066 kJ K-1 mol-1

∆G=∆H-T∆S ∆G=0 at equilibrium ∴ ∆H=T∆S or 30.5 = T × 0.66 T=462.12 K

The temperature at which the reaction,Ag2O(s) → 2Ag(s) + 1/2O2(g)Is at equilibrium is …..; Given ∆H=30.5 kJ mol-1 and ∆S=0.066 kJ K-1 mol-1

∆G=∆H-T∆S ∆G=0 at equilibrium ∴ ∆H=T∆S or 30.5 = T × 0.66 T=462.12 K

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The temperature at which the reaction,
${Ag}_{2} O (s) \overset{}{\to} 2 Ag (s) + 1 / 2 O_{2} (g)$
Is at equilibrium is …..; Given $∆ H = 30.5 kJ {mol}^{- 1} and ∆ S = 0.066 kJ K^{- 1} {mol}^{- 1}$

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$∆ G = ∆ H - T ∆ S ∆ G = 0 at equilibrium ∴ ∆ H = T ∆ S or 30.5 = T \times 0.66 T = 462.12 K$

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The temperature at which the reaction,Ag2O(s) → 2Ag(s) + 1/2O2(g)Is at equilibrium is …..; Given ∆H=30.5 kJ mol-1 and ∆S=0.066 kJ K-1 mol-1

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The temperature at which the reaction,
${Ag}_{2} O (s) \overset{}{\to} 2 Ag (s) + 1 / 2 O_{2} (g)$
Is at equilibrium is …..; Given $∆ H = 30.5 kJ {mol}^{- 1} and ∆ S = 0.066 kJ K^{- 1} {mol}^{- 1}$