(A) In Example 15-5, equal masses of CO, H₂O, CO₂, and H₂ are mixed at a temperature of about 1100 K. When equilibrium is established, which substance(s) will show an increase in quantity and which will show a decrease compared with the initial quantities?

(B) For the reaction PCl₅(g) ⇌ PCl₃(g) + Cl₂(g), K_c = 0.0454 at 261 °C. If a vessel is filled with these gases such that the initial partial pressures are P_PCl3 = 2.19 bar, P_Cl2 = 0.88 bar, P_PCl5 = 19.7 bar, in which direction will a net change occur?

Example 15-5

To increase the yield of H₂(g) in the water–gas reaction—the reaction of C(g) and H₂O(g) to form CO(g) and H₂(g)—a follow-up reaction called the “water–gas shift reaction” is generally used. In this reaction, some of the CO(g) of the water gas is replaced by H₂(g).

K_c = 1.00 at about 1100 K. The following amounts of substances are brought together and allowed to react at this temperature: 1.00 mol CO, 1.00 mol H₂O, 2.00 mol CO₂ and 2.00 mol H₂. Compared with their initial amounts, which of the substances will be present in a greater amount and which in a lesser amount when equilibrium is established?

Transcribed Image Text:

CO(g) + H₂O(g) = CO₂(g) + H₂(g)