The chemical reaction : A `rarr` P, `Delta H^(@)` = 2.8 kJ is spontaneous only above 400 K. Therefore `Delta S` of reaction must be at leat `(JK^(-1))`.

The chemical reaction : A rarr P, Delta H^(@) = 2.8 kJ is spontaneous only above 400 K. Therefore Delta S of reaction must be at least (JK^(-1)) .

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

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

In a chemical reaction triangleH =150kJ and triangleS = 100JK^-1 at 300K. The triangleG for the reaction is :

A reaction becomes spontaneous only at 500K. If Delta H at 500 K is 3.0 kJ, the change in entropy at 500 K

A reaction has value of Delta H = -40 kcal mol^(-1) at 400 K. Below 400 K the reaction is spontaneous and above 400 K it is not. The value of DeltaG and Delta S at 400 K are respectively

For a chemical reaction, DeltaS = -0.035 kJ//K and DeltaH = -20 kJ . At what temperature does the reaction turn spontaneous?