Known Delta G Degree_f at temperature: For the gas phase reaction: H_2 + CO_2 Gr

Question

Known Delta G Degree_f at temperature: For the gas phase reaction: H_2 + CO_2 Grave H_2O + CO Values of Delta G Degree_f 1000 k in J/mol are: H2 = 0, CO2 = -395790, H2O = -192420, CO = -200240 Assume ideal gas. Calculate Delta G_rxn, and K_cq at T = 1000 K. Assuming a reaction feed of 1 mole H_2, 1 mol CO_2, develop an expression of K_eq in terms of the reaction coordinate Epsilon. At what value of Epsilon does the system reach equilibrium? At equilibrium, what are the four yi values for this system?

Explanation / Answer

For the given gas phase reaction,

a) dGrxn = dGo(products) - dGo(reactants)

               = (-192420 - 200240) - (-395790)

               = 3130 J/mol

dGrxn = -RTlnKeq

3030 = -8.314 x 1000 lnKeq

Keq = 0.69

b) Keq = [H2O][CO]/[CO2][H2]

c) when e = 0 , the reaction is at equilibrium

d) 0.69 = x^2/(1 - x)(1 - x)

0.69 - 1.4x + 0.69x^2 = x^2

0.3x^2 + 1.4x - 0.69 = 0

x = 0.45 mol

At equilibrium,

[H2] = 1 - 0.45 = 0.55 mol

[CO2] = 0.55 mol

[H2O] = 0.45 mol

[CO] = 0.45 mol

Related Questions

Navigate

• Browse (All)
• Browse K
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.