In a gas-phase equilibrium mixture of H₂, I₂, and HI at 500. K, [HI] = 2.21 * 10^–3 mol · L^–1 and [I₂] = 1.46 * 10^–3 mol · L^–1. Given the value of the equilibrium constant in Table 5G.2, calculate the equilibrium molar concentration of H₂.

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TABLE 5G.2 Equilibrium Constants for Various Reactions Reaction T/K* K 4.0 X 10³1 4.0 X 10¹8 5.1 X 108 H₂(g) + Cl₂(g) = 2 HCl(g) H₂(g) + Br₂(g) + 2 HBr(g) H₂(g) + 1₂(g) 2 HI(g) 2 BrCl(g) Br₂(g) + Cl₂(g) 2 HD(g) H₂(g) + D₂(g) 300 500 1000 300 500 1000 298 500 700 300 500 1000 100 500 1000 1.9 X 10¹7 1.3 X 10¹0 3.8 X 10¹ 794 160 54 377 32 5 0.52 0.28 0.26 KJ 4.0 X 10³1 4.0 X 10¹8 5.1 X 108 1.9 X 10¹7 1.3 X 10¹0 3.8 X 104 794 160 54 377 32 5 0.52 0.28 0.26