Consider the following reaction: I2(g)+Cl2(g) ⇌ 2ICl(g) Kp= 81.9 at 25 ∘ C. Calculate ΔGrxn for the reaction at 25 ∘...

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Consider the following reaction: I2(g)+Cl2(g) ⇌ 2ICl(g) Kp= 81.9 at 25 ∘ C. Calculate ΔGrxn for the reaction at 25 ∘...

Consider the following reaction:
I2(g)+Cl2(g) ⇌ 2ICl(g)
Kp= 81.9 at 25 ∘ C.
Calculate ΔGrxn for the reaction at 25 ∘ C under each of the following conditions.

Part A. Standard conditions

Part B. At equilibrium

Part C.

PICl= 2.59 atm
PI2= 0.322 atm
PCl2= 0.221 atm

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Answer 1

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Answer #1

Concepts and reason

The reaction is as follows:

1, (g)+Cl, (g) 2CI(g)

Calculate the Gibbs free energy change of the reaction by using the following formula.

|AG= AG° RT InQ

Here, AG is Gibbs free energy change in standard conditions,
R gas constant, T is temperature, and Q is reaction quotient

Calculateby using the following formula.

AG° -RT InK

Here, K is the equilibrium constant of the reaction.

Calculate the reaction quotient as shown below.

Ра
Q
P, Ра,
2
ICI
2

Fundamentals

Change in the Gibbs free energy change when one mole of a substance is formed from its pure elements under standard conditions is called as standard free energy change. The standard conditions are 1atm pressure and 298K temperature.

At equilibrium Gibbs free energy of a reaction will be equal to zero.

(A)

AG° -RT InKp
AG 8.314 J/mol.K x 298K x In(81.9)
-8.314 J/mol x 298 x4.405
= -10913 J/mol
= -10.91 kJ/mol

Thus, standard Gibbs free energy change is -10.91 kJ/mol .

B

At equilibrium Gibbs free energy change is zero.

AG 0

(C)

2
ICI
Pa
(2.59 atm)
(0.221 atm)x(0.322 atm)
=94.26

Now calculate AG by substituting -10.91 kJ/mol for AG°, 8.314 J/mol.K for R,
298K for T, and 94.26 for Q.
AG
гхn
-24.8 kJ/mol

Ans: Part A

Standard Gibbs free energy change of the reaction is -10.91 kJ/mol .

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Answer 2

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