In a chemical reaction `DeltaH` is 150 kJ and `DeltaS` is `100 J K^(-1)` at 300 K then `DeltaG` is :-

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 :

Determine whether the reactions with the following AH and AS values are spontaneous or non-spontaneous. State whether they are exothermic or endothermic: DeltaH =- 40 kj and DeltaS = + 135J K-1 at 300 K DeltaH = -60 kj and DeltaS = -160 JK-1 at 400K

For the reaction, X_(2)O_(4)(I) rightarrow 2XO_(2)(g) Delta cup = 2.1 k cal, Delta S = 20 cal K^(-1) at 300 K hence, DeltaG is

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

For a reaction DeltaG^@ = -51.4 KJ/mol and Delta H^@ = 49.4 KJ/mol at 300K, then value of DeltaS^@ in J/K is

For a hypothetical reaction nX to mY , the value of DeltaH =-133 kJ and DeltaS = -145 J K^(-1) . Calcualte the value of DeltaG at 700 K.