Consider the reaction: i2(g)+cl2(g)⇌2icl(g) kp= 81.9 at 25 ∘c. calculate δgrxn for the reaction at 25 ∘c under each condition: -(part 1) at standard conditions -(part 2) picl= 2.63atm ; pi2= 0.324atm ; pcl2= 0.217atm .

Part 1: - 1.091 x 10⁴ J/mol.

Part 2: - 1.137 x 10⁴ J/mol.

Explanation:

Part 1: At standard conditions:

At standard conditions Kp= 81.9.

∵ ΔGrxn = -RTlnKp

∴ ΔGrxn = - (8.314 J/mol.K)(298.0 K)(ln(81.9)) = - 1.091 x 10⁴ J/mol.

Part 2: PICl = 2.63 atm; PI₂ = 0.324 atm; PCl₂ = 0.217 atm.

For the reaction:

I₂(g) + Cl₂(g) ⇌ 2ICl(g).

Kp = (PICl)²/(PI₂)(PCl₂) = (2.63 atm)²/(0.324 atm)(0.217 atm) = 98.38.

∵ ΔGrxn = -RTlnKp

∴ ΔGrxn = - (8.314 J/mol.K)(298.0 K)(ln(98.38)) = - 1.137 x 10⁴ J/mol.

a. ΔG°rxn at standard conditions : -1.09.10⁴ J/mol

b. ΔG°rxn at  PICl= 2.63atm ; PI2= 0.324atm ; PCl2= 0.217atm  =  -1.14.10⁴ J/mol

The equilibrium constant is the ratio of the concentration or pressure between the result of the reaction / product and the reactant with each reaction coefficient raised

The equilibrium constant is based on the concentration (Kc) in a reaction

pA + qB -----> mC + nD

Whereas the equilibrium constant is based on partial pressure  (Kp)

The value of Kp and Kc can be linked to the formula

R = gas constant = 0.0821 L.atm / mol.K

Δn = number of product coefficients-number of reactant coefficients

Gibbs (Free) Energy = ΔGrxn when connected to Kc / Kp:

ΔG°rxn is the standard Gibbs free energy of reaction,

ΔGrxn = ΔG°rxn + RTlnQ

At equilibrium, Q = K and ΔGrxn = 0

ΔG°rxn = -RTlnK

ΔG°rxn = -RTlnK

ΔG°rxn = - 8,314. 298 ln 81.9 = -10914.94 J / mol  = -1.09.10⁴ J/mol

Kp = 98.3799

ΔG°rxn = -RTlnK

ΔG°rxn =  - 8,314. 298 ln 98.3799

ΔG°rxn = -11369.1728 J/mol = -1.14.10⁴ J/mol

calculate kc for reaction 2 at the same temperature.

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the ka reaction of hcn

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the three most acidic hydrogen atoms

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Keywords : kc, kp, ΔGrxn,Gibbs (Free) Energy, standard conditions

i think it's c. i'm not sure but i think so.