Gibbs Free Energy

In the following questions , a statement of assertion (A) is followed by a statement of reason (R). Br A : For every chemical reaction at equilibrium, the value of standard Gibbs free energy change is zero. R: At constant temperature and pressure for a reaction that direction is preferred for which Gibbs free energy increases.

The change in Gibbs free energy of the system along provides a criterion for the spontaneity of a process at constant temperature and pressure. A change in the free energy of a sytem at constant temperature and pressure will be: DeltaG_("system") = DeltaH_("system") - T DeltaS_("system") For a spontaneous reaction DeltaG , equilibrium constant K and E_("cell")^(0) will be respectively:

Define Gibb.s free energy and free energy change.

For an equilibrium reaction, if the value of standard Gibb's free energy, AG° is zero, then the value of equilibrium constant, K will be equal to

Which of the following can help to predict the rate of reaction if the standard Gibb's free energy of reaction (Delta_rG^@) is known ?

How many of these properties are intensive here Temperature, Refractive index, density, enthalpy, entropy, molar heat capacity, Gibb's free energy, pH.

Reaction A hArr B+3C at 25^(@) C temperature reaction on equilibrium. If equilibrium constant and Gibb’s free energy are Y and X respectively. The Gibb’s free energy for reaction (1)/(2) A hArr (1)/(2) B+(3)/(2) C is :

For the reaction : 4Al+ 3O_(2) + 6H_(2)O+ 4OH^(-) rightarrow4A1(OH)_(4)^(-) E^(@)_(cell) = 2.73V . Standard Gibb's free energy change for the reaction is :

Each question contains STATEMENT-1 (Assertion) and STATEMENT-2( Reason). Examine the statements carefully and mark the correct answer according to the instruction given below: STATEMENT-1: For a reaction at equilibrium, the Gibb's free energy of reaction is minimum at constant temp. and pressure. STATEMENT-2: The Gibb's free energy of both reactants and products increases and become equal at equilibrium.

Show that the reaction CO(g) +(1//2)O_(2)(g) rarr CO_(2)(g) at 300K is spontaneous and exothermic, when the standard entropy change is -0.094 k J mol^(-1) K^(-1) . The standard Gibbs free energies of formation for CO_(2) and CO are -394.4 and -137.2kJ mol^(-1) , respectively.