Home
Class 11
CHEMISTRY
Under which of the conditions the proces...

Under which of the conditions the process will be spontaneous?

A

`DeltaG =- ve`

B

`Delta_("Total")S =+ve`

C

`Delta_("Total")S =-ve`

D

`Delta_("Total")S = 0`

Text Solution

AI Generated Solution

To determine under which conditions a process will be spontaneous, we can analyze the Gibbs free energy change (ΔG) using the Gibbs-Helmholtz equation: \[ \Delta G = \Delta H - T \Delta S \] ### Step 1: Understand Spontaneity A spontaneous process is one that occurs naturally without needing to be driven by an external force. For a process to be spontaneous, the change in Gibbs free energy (ΔG) must be negative: ...
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    CENGAGE CHEMISTRY ENGLISH|Exercise Multiple correct Answer Type|2 Videos

  • THERMODYNAMICS

    CENGAGE CHEMISTRY ENGLISH|Exercise Exercises (Single Correct)|62 Videos

  • THERMODYNAMICS

    CENGAGE CHEMISTRY ENGLISH|Exercise Exercises (Linked Comprehension)|74 Videos

  • STOICHIOMETRY

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Subjective|33 Videos

Similar Questions

Explore conceptually related problems

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

For a process to be spontaneous :

If Delta G gt 0 , then the nature of the process will be (spontaneous/non-spontaneous)?

If Delta G gt 0, then the nature of the process will be (spontaneous/non-spontaneous)?

Dependence of Spontaneity on Temperature: For a process to be spontaneous , at constant temperature and pressure , there must be decrease in free energy of the system in the direction of the process , i.e. DeltaG_(P.T) lt 0. DeltaG_(P.T) =0 implies the equilibrium condition and DeltaG_(P.T) gt 0 corresponds to non- spontaneity. Gibbs- Helmholtz equation relates the free energy change to the enthalpy and entropy changes of the process as : " "DeltaG_(P.T) = DeltaH-TDeltaS" ""..."(1) The magnitude of DeltaH does not change much with the change in temperature but the entropy factor TDeltaS change appreciably . Thus, spontaneity of a process depends very much on temperature. For endothermic process, both DeltaH and DeltaS are positive . The energy factor, the first factor of equation, opposes the spontaneity whereas entorpy factor favours it. At low temperature the favourable factor TDeltaS will be small and may be less than DeltaH, DeltaG will have positive value indicated the nonspontaneity 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 expthermic process, both DeltaH and DeltaS would be negative . In this case the first factor of eq.1 favours the spontaneity whereas the second factor opposes it. At high temperature , when T DeltaS gt DeltaH, DeltaG will have positive value, showing thereby the non-spontaneity fo the process . However , on decreasing temperature , the factor , TDeltaS decreases rapidly and when TDeltaS lt 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. The enthalpy change for a certain rection at 300 K is -15.0 K cal mol^(-1) . The entropy change under these conditions is -7.2 cal K^(-1)mol^(-1) . The free energy change for the reaction and its spontaneous/ non-spontaneous character will be

Which of the following processes is a non-spontaneous process?

Which of the natural process is spontaneous

In which case, process will be spontaneous at all temperature?

In which case, process will be spontaneous at all temperature?

Under what condition can the process of steam distillation be used ?