Given the following equilibrium constants at 437°C, 1 Na2O(s) 2 Na(l) + O2(g) K₁ = 3 × 10-25 2 K₂ = 1 x 10-5 K3=9 x 10-29 K4 = 4 x 10-14 1 NaO(g)Na(l) + O₂(g) Na2O2 (s) 2 Na(l) + O₂(g) NaO2 (s) Na(l) + O₂(g) determine the values for the equilibrium constants for the following reactions: a. Na₂O(s) + O₂(g) → Na2O₂ (s) Equilibrium constant = b. NaO(g) + Na2O(s) ⇒ Na₂O₂ (s) + Na(1) Equilibrium constant = c. 2 NaO(g) → Na₂O₂ (s) Equilibrium constant = (Hint: When reaction equations are added, the equilibrium expressions are multiplied.)

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 75.0 L tank with 6.2 mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 6.5 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K-0 C = ☐ x10 ×

Write the equilibrium constant expression for the following reaction:  Fe3O4(s) + 4H2(g) to 3Fe(s) + 4H2O(g)

Consider the following equilibria A(g) → 2 X(g) + C(g) Kc = 1.55 B(g) → X(g) Kc = 25.2 Calculate the equilibrium constant for the following reaction? A(g) 2 B(g) + C(g) Kc = ? 6.10 x 10-4 26.8 2.44 x 10-3 78.1 984 S