Calculating Equilibrium Constants Part A The equilibrium constant, K, of a react

Question

Calculating Equilibrium Constants Part A The equilibrium constant, K, of a reaction ata particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium Phosgene (carbonyl chloride), COC12, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: CO(g) Cl2 (g) COCl2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 477 °C.At equilibrium, the concentrations were measured and the following results obtained For a gaseous reaction with the general form Partial Pressure the Kc and Kp expressions are given by Gas 0.860 1.17 0.170 CO Al Bb COCI2 What is the equilibrium constant, Kp, of this reaction? Express your answer numerically (PA) (PB) The subscript c or p indicates whether K is expressed in terms of concentrations or pressures Equilibrium-constant expressions do not include a term for any pure solids or liquids that may be involved since their composition does not change throughout the reaction. The standard state of a pure substance is the pure substance itself, and although the quantity may change the sample remain pure. The concentration is effectively equal to 1, and will not impact the magnitude of K Submit Hints My Answers Give Up Review Part

Explanation / Answer

PART A)

Kp = Partial Pressure of Products ^p / PArtial PRessures of Reactants ^r

Kp = P-COCl2 / (P-CO)(P-Cl2)

Kp = (0.17)/(0.86*1.17)

Kp = 0.1689

PART B

H2 + I2 <-> 2HI

initially

[H2] = 3.55

[I2] = 2.4

[HI] = 0

in equilibrium

[H2] = 3.55 -x

[I2] = 2.4 - x

[HI] = 0 +x

and

[I2] = 2.4 - x = 0.3

solve for x

x = (0.3 - 2.4)/-1 = 2.1

then

[H2] = 3.55 -2.1 = 1.45

[I2] = 2.4 - 2.1 = 0.3

[HI] = 0 +2.1

Kc = [HI]^2 / [I2][H2]

Kc = (2.1^2)/(0.3*1.45) = 10.13793

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---

---

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