11) Calculate AG° for: H₂O(g) +1/202(g) = H₂O₂(g) at 600. K using the following data: H(g)+O,H,O,(g) K=2.3 X 10° at 600. K 2H2(g) + O(g) 2H,O(g) K = 1.8 X 10 at 600. K #

Calculate AG° at 605 K for H2O(g) + 1/2 O2(g) H2O2(g) using the following data: H2(g) +O2(g) S H2O2(g) K = 8.9 x 106 at 605 K 2H2(g) + O2(g) = 2H20(g) K = 2.0 x 10° at 605 K AG° kJ/mol

Calculate AG° for H20(g) + 02(g) = H2O2 (g) at 595 K, using the following data: H2 (9) + O2 (9) = H2O2(g) K = 3.7 x 1037 at 595 K 2H2 (9) + O2 (9) = 2H2O(g) K = 2.6 × 10® at 595 K AG kJ/mol

Calculate K for the reaction Ag₂ Q(8) + CO(g) ⇒ 2 Ag(s) + CO₂ (g) given the following information: K = Ag₂ O(s) + H₂ (g) ≥ 2 Ag(s) + H₂O(g) K₁ = 1.01 X 10¹3 H₂ (g) + CO₂ (g) ⇒ H₂ O(g) + CO(g) K2 = 0.771

Given the reaction shown below, with K=4.10x1018 occurring at 300 K;  H2(g) + Br2(g) to 2HBr(g)  calculate the equilibrium constant for the reaction shown:  2HBr(g) to H2(g) + Br2(g)

Given: 2N2(g)+ O2(g) = 2N20(g); Ke(1) = 5.8 x 10-36 and N2(g) + O2(g) = 2NO(g); K(2) = 4.1 x 10-31 What is the equilibrium constant for the reaction? 2N20(g) + O2(g) = 4NO(g)

3. Hydrogen can react with elemental sulfur to give the toxic gas H₂S according to the equation H2(g) + 1/8 S8(s) = H2S(g) If the equilibrium constant Kc for this reaction is 7.6 x 105 at 25°C, determine the value for the equilibrium constant for the reaction written as 2 H₂(g) + 4 S8(s) = 2 H2S(g) Ans: 5.8 x 1011 2022 S'2303 0 BIO-Focused CH 1244018

Calculate Kc or Kp:CH4(g)+H2O(g)->CO(g)+3H2(g) Kp=7.7x10^24 (at 298 K)

The equilibrium constant, Kc, for the following reaction is 18.1 at 773 K. 2NH3 (9) ⇒ N₂(g) + 3H₂(g) Calculate Ke at this temperature for the following reaction: 1/2N2(g) + 3/2H₂ (9) ⇒ NH3 (9) Kc =

Consider the reaction in the Haber process 3H2 (g) + N2 (g) → 2NH3 (g)where delta H° = -91.8 kJ/mol and delta S° = -197 J/(mol*K). What is the value of the equilibrium constant (K) at a temperature of 125°C?