The temperature of K at which `Delta`G =0 for a given reaction with `Delta`H= -20.5 kJ `mol^(-1)`and` Delta`S =- 50.0 `JK^(-1)mol^(-1)`

The temperature in K at which DeltaG=0 for a given reaction with DeltaH=-20.5 kJ mol^(-1) and DeltaS=-50.0 JK^(-1) mol^(-1) is

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

At the temperature T(K) for the reaction X_(2)O_(4) (l) rarr 2XO_(2)(g) Delta U = x kJ mol^(-1), Delta S = y JK^(-1) mol^(-1) . Gibbs energy change for the reaction is (Assume X_(2)O_(4), XO_(2) are ideal gases) Delta U = x kJ mol^(-1), Delta S = y JK^(-1) mol^(-1)

Calculate the temperature at which liquid water will be in equilibrium with water vapour. Delta_(vap)H = 40.00 kJ mol^(-1) and Delta_(vap)S = 0.100 kJ mol^(-1)K^(-1)

Judge the spontaneity of the following reaction at 298 K temperature and at a particular pressure: Br_2(1) + Cl_2 (g) rarr 2BrCl (g) . Given : Delta H = 29.3 kJ mol^(-1) and Delta S = 104.1 JK^(-1) mol^(-1)