For a reaction,
`Ag_(2)O(s)hArr2Ag(s)+(1)/(2)O_(2)(g)`
`DeltaH,DeltaS and T ` are 40.63 kJ `mol^(-1)`, 108.8 J `K^(-1)mol^(-1) and 373.3K` respectively. Predict the feasibility of the reaction:

For the reaction, Ag_(2)O(s)hArr2Ag(s)+(1)/(2)O_(2)(g) DeltaH,DeltaS and T are 40.63 kJ mol^(-1) , 108.8 JK^(-1)mol^(-1) and 373.4K respectively. Free energy change DeltaG of the reaction will be:

For the reaction, Ag_(2)O_((s)) hArr 2Ag_((s)) + (1)/(2) O_(2(g)) Delta H, Delta S and T are 40.63 kJ mol^(-1), 108.8 JK^(-1) mol^(-1) and 373K respectively. Free energy change Delta G of the reaction will be _____

Enthalpy and entropy changes of reaction are 40.63 kJ mol^(-1) and 108.8 J K^(-1) mol^(-1) , respectively. Predict the feasibility of the reaction at 27^(@)C .

Enthalpy and entropy changes of reaction are 40.63 kJ mol^(-1) and 108.8 J K^(-1) mol^(-1) , respectively. Predict the feasibility of the reaction at 27^(@)C .

For the reaction, Ag_(2)O(s)rarr2Ag(s)+(1)/(2)O_(2)(g),DeltaH,DeltaS and T are 40kJ, 100J and 380K respectively. Hence DeltaG in kJ is :

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.

Enthalpy and entropy changes of a reaction are 40.63 kJ/mol and 108.8 Jk^-1mol^-1. Predict the feasibility of the reaction atr 27^oC.

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