At 298 K, `Delta H and Delta S` for a reaction are `-65.49 " kJ and " -145 J. K^(-1)` respectively. Calculate `Delta G, Delta S_("univ") and Delta S_("surr")` at that temperature.

The values of Delta H and Delta S for the reaction are 170 kJ and 170 J K^(-1) , respectively. This reaction will be spontaneous at

In a reversible process, Delta S_(sys) + Delta S_(surr) is

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

In the conversion of lime stone to lime, CaCO_(3(s)) rarr CaO_((s)) + CO_(2(g)) , the values of Delta H^(@) and Delta S^(@) are + 179.1 kJ mol^(-1) and 160.2 JK^(-1) mol^(-1) respectively at 298K and 1 bar. Assuming, Delta H^(@) and Delta S^(@) do not change with temperature, temperature above which conversion of lime stone to lime will be spontaneous is

For a hypothetical reaction nX to mY , the value of DeltaH =-133 kJ and DeltaS = -145 J K^(-1) . Calcualte value of DeltaS_("surr".) and DeltaS_("univ")

Delta S_("surr") for an exothermic reaction is

In a reversible process, the value of Delta S _(sys) + Delta S_(surr) is

In a reversible process, the value of Delta S _(sys) + Delta S_(surr) is