For a reaction both `Delta H` and `Delta S` are positive,under what condition will the reaction occur spontaneously?

A reaction occurs spontaneously if

The condition for a reaction to occur spontaneously is -

If the value of DeltaH and DeltaS are of following type, then at what condition a reaction will occur spontaneously? (i) DeltaH gt0 and DeltaSgt0 (ii) DeltaH lt0 and DeltaS gt0

For endothermic reaction Delta H value is-

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

Under what conditions will a bimolecular reaction be of the first order?

At 300 K, the enthalpy change and entropy change of a reaction are -10 kcal and -30 " cal". K^(-1) respectively. Does the reaction occur spontaneously at 400 K ? If not, then calculate the maximum temperature at which the reaction will occur spontaneously ?

For a given reaction , Delta H = 3.5 kJ mol^(-1) and Delta S = 83.6 J * K^(-1) mol^(-1) . The reaction is spontaneous at (assume DeltaH and Delta S do not vary with temperature) -

Delta G = O at equilibrium is satisfied under condition