At equilibrium
`DeltaG=0`
`DeltaG=+ve`
`DeltaG=-ve`
`DeltaU=0`

Which of the following conditions may lead to a non-spontaneous change? a. DeltaH " and "DeltaS " both "+ve b. DeltaH=-ve,DeltaS=+ve c. DeltaH=+ve,DeltaS=-ve d. DeltaH=-ve,DeltaS=-ve

For the equilibrium , DeltaG = - RT In K .

What is significance of T DeltaS in DeltaG = DeltaH - T DeltaS ?

Derive the equation, DeltaG = DeltaH - T DeltaS .

The efficiency of a fuel cell is given by: DeltaG//DeltaS , DeltaG//DeltaH , DeltaS//DeltaG , DeltaH//DeltaG

Free enegry , G = H - TS , is state function that indicates whther a reaction is spontaneous or non-spontaneous. If you think of TS as the part of the system's enegry that is disordered already, then (H -TS) is the part of the system's energy that is still ordered and therefore free to cause spontaneous change by becoming disordered. Also, DeltaG = DeltaH - T DeltaS From the second law of thermodynamics, a reaction is spontaneous if Delta_("total")S is positive, non-spontaneous if Delta_("total")S is negative, and at equilibrium if Delta_('total")S is zero. Since, -T DeltaS = DeltaG and since DeltaG and DeltaS have opposite sings, we can restate the thermodynamic criterion for the spontaneity of a reaction carried out a constant temperature and pressure. IF DeltaG lt 0 , the reaction is spontaneous. If DeltaG gt 0 , the reaction is non-spontaneous. If DeltaG = 0 , the reaction is at equilibrium. Read the above paragraph carefully and answer the following questions based on the above comprehension. For the spontaneity of a reaction, which statement is true?

A contributions of both heat (enthalpy) and randomness(entropy) shall be considered to the overall spontaneity of process.When deciding about the spontaneity of a chemical reaction or other process, we define a quantity called the Gibb's energy change (DeltaG) . DeltaG=DeltaH-TDeltaS where, DeltaH =Enthalpy change, DeltaS =Entropy change , T=Temperature in kelvin. If DeltaGlt0 , Process is spontaneous , DeltaG=0 , Process is at equilibrium , DeltaGgt0 , Process is non-spontaneous. 5 mol of liquid water is compressed from 1 bar to 10 bar at constant temperature.Change is Gibb's energy (DeltaG) in Joule is:[Density of water = 1000 kg//m^3 ]

A contributions of both heat (enthalpy) and randomness(entropy) shall be considered to the overall spontaneity of process.When deciding about the spontaneity of a chemical reaction or other process, we define a quantity called the Gibb's energy change (DeltaG) . DeltaG=DeltaH-TDeltaS where, DeltaH =Enthalpy change, DeltaS =Entropy change , T=Temperature in kelvin. If DeltaGlt0 , Process is spontaneous , DeltaG=0 , Process is at equilibrium , DeltaGgt0 , Process is non-spontaneous. For the change H_2O(s),(273 K ,2 atm) to H_2O(l) ,(273 K, 2 atm), choose the correct option.

Free enegry , G = H - TS , is state function that indicates whther a reaction is spontaneous or non-spontaneous. If you think of TS as the part of the system's enegry that is disordered already, then (H -TS) is the part of the system's energy that is still ordered and therefore free to cause spontaneous change by becoming disordered. Also, DeltaG = DeltaH - T DeltaS From the second law of thermodynamics, a reaction is spontaneous if Delta_("total")S is positive, non-spontaneous if Delta_("total")S is negative, and at equilibrium if Delta_('total")S is zero. Since, -T DeltaS = DeltaG and since DeltaG and DeltaS have opposite sings, we can restate the thermodynamic criterion for the spontaneity of a reaction carried out a constant temperature and pressure. IF DeltaG lt 0 , the reaction is spontaneous. If DeltaG gt 0 , the reaction is non-spontaneous. If DeltaG = 0 , the reaction is at equilibrium. Read the above paragraph carefully and answer the following questions based on the above comprehension. A particular reaction has a negative value for the free energy change. Then at ordinary temperature

Free enegry , G = H - TS , is state function that indicates whther a reaction is spontaneous or non-spontaneous. If you think of TS as the part of the system's enegry that is disordered already, then (H -TS) is the part of the system's energy that is still ordered and therefore free to cause spontaneous change by becoming disordered. Also, DeltaG = DeltaH - T DeltaS From the second law of thermodynamics, a reaction is spontaneous if Delta_("total")S is positive, non-spontaneous if Delta_("total")S is negative, and at equilibrium if Delta_('total")S is zero. Since, -T DeltaS = DeltaG and since DeltaG and DeltaS have opposite sings, we can restate the thermodynamic criterion for the spontaneity of a reaction carried out a constant temperature and pressure. IF DeltaG lt 0 , the reaction is spontaneous. If DeltaG gt 0 , the reaction is non-spontaneous. If DeltaG = 0 , the reaction is at equilibrium. Read the above paragraph carefully and answer the following questions based on the above comprehension. Which of the following is true for the reaction? H_(2)O(l) hArr H_(2)O(g) at 100^(@)C and 1 atmosphere