If for a reaction `Delta H=50(kJ)/(mol)` `Delta S=50J/(K.mol)` then `Delta G` at `500K` will be

In a chemical reaction, Delta H = 150 kJ and Delta S = 100 JK^(-1) at 300 K. Therefore, Delta G will be

Suppose that a reaction has DeltaH=-40kJ and DeltaS =- 50J//K . At what temperature range will it change from spontaneous to non-spontaneous?

For a given reaction, Delta H = 35.5 kJ mol^(-1) and Delta S = 83.6 JK^(-1) mol(-1) . The reaction is spontaneous at : (Assume that Delta H and Delta S do not vary with temperature)

For a given reaction, DeltaH = 35.5 kJ mol^(-1) and Delta S = 83.6 JK^(-1) mol^(-1) . The reaction is spontaneous at (Assume that DeltaH and DeltaS do not vary with temperature)

If a process has Delta H = 548.3 kJ and Delta S = 32 J/mole at 298 K then will the process be spontaneous at this temperature ?

For the reaction 2A (g) + B(g) to C (g) Delta U^(@) = 20 kcal/mole, Delta S^(@) = 100 cal/kmole at 300 K. Hence Delta G^(@) in kcal is __________ [R = 2 cal mol^(-1) K^(-1)]

For a demerization reaction , 2A (g) to A_2 (g) at 298 K, Delta U(Theta) = - 20 kJ"mol"^(-1), Delta S^(Theta) = - 30 JK^(-1) "mol"^(-1) , then the Delta G^(Theta) will be _________J.

For a reaction R_(1), Delta G = x KJ mol^(-1) . For a reaction R_(2), Delta G = y KJ mol^(-1) . Reaction R_(1) is non-spontaneous but along with R_(2) it is spontaneous. This means that

Delta G^(0) and Delta H^(0) for a reaction at 300K is -66.9kJmol^(-1) and -41.8kJmol^(-1) respectively. Delta S^(0) for the same reaction at 300K is

The activation energy for the forward reaction X rarr Y is 60 kJ mol^(-1) and Delta H is -20 kJ mol^(-1) . The activation energy for the reverse reaction is