Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium pressure of H₂. D₂(g) + H₂(g) ⇌ 2HD(g) K_p = 1.80
P(D₂) _eq = 1.1 × 10^-3bar P(HD) _eq = 2.7 × 10^-3 bar

Question

Quizplus · Accepted Answer

The equilibrium constant expression for the reaction is:K_p = P(HD)² / P(D₂)P(H₂)Substituting the given equilibrium concentrations into the expression, we get:1.80 = (2.7 × 10^-3 bar)² / (1.1 × 10^-3 bar)P(H₂)Solving for P(H₂), we get:P(H₂) = (2.7 × 10^-3 bar)² / (1.80 × 1.1 × 10^-3 bar) = 3.7 × 10^-3 barTherefore, the equilibrium pressure of H₂ is 3.7 × 10^-3 bar.

Consider the Following Reaction, Equilibrium Concentrations, and Equilibrium Constant at a Particular