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)

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

Calculate the value of DeltaG at 700K for the reaction, nX to mB . Given that value of DeltaH=-113kJ mol^(-1) and DeltaS=-145JK^(-1)mol^(-1).

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

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

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

(i) State hess's law. (ii) For the following reaction at 298K 2X+Y to Z DeltaH=300kJ*mol^(-1) and DeltaS=0.2kJ*K^(-1)*mol^(-1) At what temperature will the reaction become spontaneous considering DeltaH and DeltaS to be constant over the temperature range?

For a given reaction , Delta H = 3.5 kJ mol^(-1) and Delta S = 83.6 J * K^(-1) mol^(-1) . The reaction is spontaneous at (assume DeltaH and Delta S do not vary with temperature) -