Calculate the temperature at which `DeltaG=-5.2 kJ``mol^-1`,DeltaH=145.6kJ``mol^-1` and `DeltaS=216 JK^-1` `mol^-1` for a chemical reaction

Calculate the temperature at which DeltaG = -5.2 kJ mol^-1, DeltaH = 145.6 kJ mol^-1 and DeltaS = 216 J K^-1 mol^-1 for a chemical reaction

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

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)

For the reaction at 298 K 2A + B to C DeltaH = 40 kJ "mol"^(-1) and DeltaS = 0.2 kJ K^(-1) "mol"^(-1) . At what temperature will the reaction beccomes sponatneous considering DeltaH and DeltaS to be constant over the temperature range.

For vaporization of water at 1bar, DeltaH=40.63kJ mol^(-1) and DeltaS = 108.8 JK ^(-1) mol^(-1) At what temperature, DeltaG=0 ?

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

For the reaction at 298 K 2A+B rarr C DeltaH=400 kJ mol^(-1) and DeltaS=0.2 kJ K^(-1) mol^(-1) At what temperature will the reaction becomes spontaneous considering DeltaH and DeltaS to be contant over the temperature range.

For the reaction at 298 K 2A+B rarr C DeltaH=400 kJ mol^(-1) and DeltaS=0.2 kJ K^(-1) mol^(-1) At what temperature will the reaction becomes spontaneous considering DeltaH and DeltaS to be contant over the temperature range.