Question

1. A key step in the extraction of iron from its ore is

FeO(s) + CO(g) ⇌ Fe(s) + CO₂(g) K_p = 0.403 at 1,000°C

This step occurs in the 700°C to 1,200°C zone within a blast furnace. What are the equilibrium partial pressures of CO(g) and CO₂(g) when 1.1000 atm of CO(g) and excess FeO(s) react in a sealed container at 1000°C?

2. Compound A decomposes according to the equation

    A(g) ⇌ 2 B(g) + C (g)

A sealed 1.00−L container initially contains 1.82 ×10⁻³ mol of A(g), 1.23 ×10⁻³ mol of B(g), and 6.49 ×10⁻⁴ mol of C(g) at 100°C. At equilibrium, [A] is 2.12 ×10⁻³M. Find [B] and [C].

Solve for the equilibrium concentrations of B and C.

3. Nitrogen dioxide decomposes according to the reaction

2 NO₂(g) ⇌ 2 NO(g) + O₂(g)

where K_p = 4.48 ×10⁻¹³ at a certain temperature. If 0.65 atm of NO₂ is added to a container and allowed to come to equilibrium, what are the equilibrium partial pressures of NO(g) and O₂(g)?

4. Even at high temperatures, the formation of NO is not favored:

(K_c = 4.10 × 10⁻⁴ at 2000°C)

N₂(g) + O₂(g) ⇌ 2 NO(g)

What is [NO] when a mixture of 0.20 mol of N₂(g) and 0.24 mol of O₂(g) reach equilibrium in a 1.0−L container at 2,000°C?

Answer 1