The reaction,
`MgO(s) + C(s) to Mg(s) + CO(g),` for which `Delta_(r)H^(@)= +491.1 " " kJ " " mol^(-1)` and `Delta_(r)S^(@)= 198.0 JK^(-1)mol^(-1)`, is not feasible at 289 K . Temperature above which reaction will be feasible is :

Predict whether it is possible or not to reduce magnesium oxide using carbon at 298K according to the reaction. MgO(s) +C(s) rarr Mg(s) +CO(g) Delta_(r)H^(Theta) = +491.18 kJ mol^(-1) and Delta_(r)S^(Theta) = 197.67 J K^(-1) mol^(-1) If not at what temperature, the reaction becomes spontaneous.

Predict whether it is possible or not to reduce magnesium oxide using carbon at 298K according to the reaction. MgO(s) +C(s) rarr Mg(s) +CO(g) Delta_(r)H^(Theta) = +491.18 kJ mol^(-1) and Delta_(r)S^(Theta) = 197.67 J K^(-1) mol^(-1) If not at what temperature, the reaction becomes spontaneous.

For the reaction, CaCO_(3)(s)toCaO(s)+CO_(2)(g),DeltaH^(0)=+179.1kJ*mol^(-1) and DeltaS^(0)=160.2J*K^(-1) . If DeltaH^(0) and DeltaS^(0) are temperature independent, then temperature above which the reaction will be spontaneous is equal to-

Given PbO _((s)) + C _((s)) to Pb _((s)) + CO _((g)) , Delta H = 108 kJ mol ^(-1) and Delta S = 190 JK ^(-1) mol ^(-1, reduction of PbO _((s)) is spontaneous

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 300 K A(g)hArrV(g)+S(g) Delta_(r)H^(@)=- 30 kJ//mol, Delta_(r)S^(@)=-0.1K^(-1).mol^(-1) What is the value of equilibrium constant ?