In a reaction `DeltaG` and `DeltaH` both are positive. The reaction would not be spontaneous if :

Assertion : If both DeltaH^(@) and DeltaS^(@) are positive then reaction will be spontaneous at high temperature. Reason : All processes with positive entropy chang are spontaneous.

Assertion : If both DeltaH^(@) and DeltaS^(@) are positive then reaction will be spontaneous at high temperature. Reason : All processes with positive entropy change are spontaneous.

In a reaction, DeltaH and DeltaS both are more than zero. In which of the following cases, the reaction would not be spontaneous?

In a reaction DeltaH and DeltaS both are more than zero. In which of the following cases, the reaction would not be spontaneous?

In a reaction DeltaH and DeltaS both are more than zero. In which of the following cases, the reaction would not be spontaneous?

In a reaction, DeltaH and DeltaS both are more than zero. In which of the following cases, the reaction would not be spontaneous?

DeltaG of the system alone provides a criterion for the spontaneity of a process at constant temperature & pressure, DeltaG system lt 0 (spontaneous) DeltaG system = 0 (equilibrium) DeltaG system gt 0 {(non-spontaneous) Again DeltaG^@ is related to the equilibrium constant as follows : DeltaG^@ = 2.303 RT log K_e If both DeltaH and Delta S are negative, the reaction will be spontaneous

For a reaction both DeltaH and DeltaS are positive.Under what conditions does the reaction occur spontaneously?