`Delta H` and `Delta S` for the reaction, `Ag_(2)O(s)to 2A(s)+(1)/(2)O_(2)(g)`, are 30.56 kJ `mol^(-1)` and 66.0 J `mol^(-1)` respectively. Calculate the temperature at which this reaction will be at equilibrium. Predict whether the forward reaction will be favoured above or below this temperature.

DeltaH and DeltaS for the reaction: Ag_(2)O(s) rarr 2Ag(s) +(1//2)O_(2)(g) are 30.56 kJ mol^(-1) and 66.0 J JK^(-1) mol^(-1) respectively. Calculate the temperature at which free energy change for the reaction will be zero. Predict whether the forward reaction will be favoured above or below this temperature.

DeltaH and DeltaS for the reaction: Ag_(2)O(s) rarr 2Ag(s) +(1//2)O_(2)(g) are 30.56 kJ mol^(-1) and 66.0 J JK^(-1) mol^(-1) respectively. Calculate the temperature at which free energy change for the reaction will be zero. Predict whether the forward reaction will be favoured above or below this temperature.

Delta H and DeltaS for the reaction Ag_2O (s) iff 2Ag(s)+ 1/2O_2(g) are 30.56 kJ mol^-1 and 66.0 JK^-1 respectively. Calculate the temperature at which the reaction would be at equilibrium. Also predict the direction of the reaction above this temperature.

DeltaH and DeltaS for the reaction Ag_(2)O_((s))rarr2Ag_((s))+1/2O_(2_((g))) " are "30.56 kJ mol^(-1) and 66.0 Jk^(-1) mol^(-1) respectively. Calculate the temperature at which the free energy for this reaction will be zero. What will be the direction of reaction at this temperature and at temperature below this and why ? Given: DeltaH=30.56kJ mol^(-1)=30560 J mol^(-1) DeltaS=66.0JK^(-1)mol^(-1) DeltaG=0