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Standard XII

Chemistry

Equilibrium Constant and Standard Free Energy Change

Δ G⊖ standard...

Question

$Δ G^{⊖}$ (standard free energy change) is free energy change for the process at what temperature of when reactants react completely to form products.

298 K

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398 K

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0 K

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None of these

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Solution

The correct option is A $298 K$
The free-energy change $Δ G^{⊖}$ for a reaction occurring under a set of standard conditions: temperature, $298 K$ ; pressure, 1 atm or $101.3 k P a$ ; and all solutes at $1 M$ concentration.

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Similar questions

Δ G^{⊖}

(standard free energy change) is free energy change for the process at what temperature of when reactants react completely to form products.(in K)

Q. Standard Free Energy and Equilibrium constant: The change in free energy for a reaction taking place between gaseous reactants and products represented by general equation.

Δ G = Δ G^{\circ} + R T l n Q_{P}

the condition for a system to be at equilibrium is that

Δ G = 0 and Q_{p} = K_{P}

Thus at equilibrium

Δ G^{\circ} = - R T l n K_{P}

Note: In the reaction, where all gaseous reactants and products;

K represents K_{P}

, we may conclude that for standard reactions, i.e., at

1 M or 1 atm

When

Δ G^{\circ} = - v e or K > 1 : forward reaction is feasible

Δ G^{\circ} = + v e or K < 1 : reverse reaction is feasible

Δ G^{\circ} = 0 or K = 1 : reaction is at equilibrium (very rare)

K_{c}

for reaction

N_{2} O_{4} ⇌ 2 N O_{2}

in chloroform at

291 K

1.14

. Calculate the free energy change of the reaction when the concentration of the two gases are

0.5 {mol dm}^{- 3}

each at the same temperature. (

R = 0.082 {lit atm K}^{- 1} {mol}^{- 1}

)

Q. The relationship between the free energy change

(Δ G)

and entropy change

(Δ S)

at constant temperature

(T)

Q. What is the free energy change

(Δ G)

when 1.0 mole of water at

100^{\circ} C

and 1 atm pressure?

Q. Standard Free Energy and Equilibrium constant: The change in free energy for a reaction taking place between gaseous reactants and products represented by general equation.

Δ G = Δ G^{\circ} + R T l n Q_{P}

the condition for a system to be at equilibrium is that

Δ G = 0 and Q_{p} = K_{P}

Thus at equilibrium

Δ G^{\circ} = - R T l n K_{P}

Note: In the reaction, where all gaseous reactants and products;

K represents K_{P}

, we may conclude that for standard reactions, i.e., at

1 M or 1 atm

When

Δ G^{\circ} = - v e or K > 1 : forward reaction is feasible

Δ G^{\circ} = + v e or K < 1 : reverse reaction is feasible

Δ G^{\circ} = 0 or K = 1 : reaction is at equilibrium (very rare)

For the equilibrium

N i O (s) + C O (g) ⇌ N i (s) + C O_{2} (g), Δ G^{\circ} ({J Mol}^{- 1}) = - 20700 - 11.97 T .

. Calculate the temperature at which the product gases at equilibrium at

1 atm

will conatin

400 ppm

of carbon monoxide.

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ΔG⊖ (standard free energy change) is free energy change for the process at what temperature of when reactants react completely to form products.

The correct option is A 298KThe free-energy change ΔG⊖ for a reaction occurring under a set of standard conditions: temperature, 298K; pressure, 1 atm or 101.3kPa; and all solutes at 1M concentration.

$Δ G^{⊖}$ (standard free energy change) is free energy change for the process at what temperature of when reactants react completely to form products.

The correct option is A $298 K$
The free-energy change $Δ G^{⊖}$ for a reaction occurring under a set of standard conditions: temperature, $298 K$ ; pressure, 1 atm or $101.3 k P a$ ; and all solutes at $1 M$ concentration.