What are spontaneous and non-spontaneous process? Under what conditions will the reaction occur if:
(i) both `DeltaH` and `DeltaS` are positive
(ii) both `DeltaH` and `DeltaS` are negative?

Under what conditions will a reaction be spontaneous if (i) both DeltaH and DeltaS are positive? (ii) both DeltaH and DeltaS are negative?

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

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

DeltaH and DeltaS are +ve . Under what conditions, process will be spontaneous?

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

For a process top be spontaneous, at constant temperature and pressure, there must be decreases in free energy of the system in the direction of the process, i.e. DeltaG_(P.T.)lt0.Delta_(P.T.)=0 implies the equilibrium condition and DeltaG_(P.T.)gt0 corresponding to non-spontaneity. Gibb's Helmholtz equation relates the free energy change to the enthalpy and entropy change of the process as : DeltaG_(P.T.)=DeltaH-TDeltaS ......(i) The magnitude of Delta H does not change much with the change in temperature but the entropy factor TDeltaS changes appreciably. Thus, spontaneity of a process depends very much on temperature. For edothermic proces, both DeltaH "and " DeltaS are positive. The energy factor,the first factor of equation, opposes the spontaneity whereas entropy factor favours it . At low temperature, the favourable factor TDeltaS will be small and may be less than Delta H, DeltaG will have positive value indicating the non-spontaneity of the process. On raising temperature, the factor TDeltaS increases appreciably and when it exceeds DeltaH,DeltaG would become negative and the process would be spontaneous. For an exothermic process, both DeltaH " and " DeltaS would be negative. In this case, the first factor of equation(i) favours the spontaneity whereas the second factor opposes it. At high temperature, when TDeltaSgt DeltaH, DeltaG will have positive value, showing thereby the non-spontaneity of the process. However, on decreasing temperature, the factore TDeltaSlt DeltaH,DeltaG becomes negative and the process occurs spontaneously. Thus, an exothermic process may be spontaneous at low temperature and non-spontaneous at high temperature. For the reaction at 298K, 2A+B toC" " Delta H =100 kcal and DeltaS= 0.050 kcal K^(-1) . If DeltaH " and " DeltaS are assumed to be constant over the temperature range, just above what temperature will be reaction become spontaneous?

Define entropy and free energy of a system.Predict the feasibility of a reaction when : (i) Both DeltaH and DeltaS increase. (ii)Both DeltaH and DeltaS decrease. (iii) DeltaH decreases but DeltaS increases.

Which of the following is true during adsorption? a. DeltaG , DeltaH , and DeltaS all are negative. b. DeltaG is negative, but DeltaH and DeltaS is positive. c. DeltaG and DeltaH are negative, but DeltaS is positive. d. DeltaG and DeltaS are negative, but DeltaH is positive.