4. Indicate whether the following equilibrium mixtures contain mostly products or mostly reactants. (a) CO(g) + Cl2(g) → COC12(g) K= 5.0 x 10-9 (b) 2NO(g) + O2(g) → 2NO2(g) K= 6.0 x 1013 (c) 2H2O(g) → 2H2(g) + O2(g) K= 4.0 x 10-48 5. The equilibrium constant K. for the following reaction is 4.6 x 103. If the equilibrium W.S (0)

4. Indicate whether the following equilibrium mixtures contain mostly products or mostly reactants. (a) CO(g) + Cl2(g) → COC12(g) K= 5.0 x 10-9 (b) 2NO(g) + O2(g) → 2NO2(g) K= 6.0 x 1013 (c) 2H2O(g) → 2H2(g) + O2(g) K= 4.0 x 10-48 5. The equilibrium constant K. for the following reaction is 4.6 x 103. If the equilibrium W.S (0)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

When chlorine gas is reacted with bromine gas an equilibrium will be established with bromine monochloride: Br2(g) + Cl2(g) 2BrCl(g)
Write the equilibrium expression (Ke) for the reaction: PC1s(g) PC13(8) + C12(g)
Number 45
Write the equilibrium expressions 6H20(g) + 6C02(g) C6H1206(s) + 602(g)
6.
6) A mixture of 9.00 moles of A, 10.00 moles of B, and 28 moles of C is placed in a one liter container at room temperature. The reaction is allowed to reach equilibrium at which point the number of moles of B is 18.00. Calculate the equilibrium constant, Kc, for this reaction: A (g) + 2 B (g) « 3 C (g)Kc = ?
The equilibrium 4 NH3(g) + 4 O2(g) ⇆ 2 N2O (g) + 6 H2O(l) ΔHo = −142 kJ/mol Is established in a sealed container with a piston. Which of the following actions will increase the amount of the products present at equilibrium? I Increasing the volume of the container II Reducing the volume of the container III Removing some of the H2O(l) from the container IV Adding some NH3(g) to the container V Adding N2(g) to the container VI Raising the temperature VII Lowering the temperature
Consider the following reaction: A(g) = 3 B(g) A reaction mixture initially contains 1.3 M of A. Determine the equilibrium concentration of B if Kc for the reaction at this temperature is 8.62 x 10. Calculate this based on the assumption that the x value is negligible compared to 1.3.
Using the equilibrium constants given for reactions (1) and (2), what is the equilibrium constant for reaction (3)? 1) 2NO(g) + O2(g) → N2O4(g) Kp = 1.49 × 1013 2) 2NO(g) + O2(g) → 2NO2(g) Kp = 1.66 × 1012 3) N2O4(g) → 2NO2(g) 80.3 0.111 None of the following 8.98 0.0123
6. Hydrogen sulfide is a pollutant found in natural gas. Following its removal, it is converted to sulfur by the reaction: 2H2S(g) + SO2(9) =Ss(s, rhombic) + 2H20(1) What is the equilibrium constant for this reaction? Is the reaction endothermic or exothermic?
(Q106) Consider the decomposition of nitrosyl bromide into nitrogen monoxide and bromide gas, which has an equilibrium constant K. = 6.2 x 105 when the reaction occurs at a certain temperature. If the initial concentration of nitrosyl bromide is 0.832 M, what will be the equilibrium concentration of nitrogen monoxide gas? 2 BRNO (g) 2 NO (g) + Br2 (g)
Consider the reaction: 2 NH3(g) = N₂(g) + 3 H₂(g). At T = 740 K, the equilibrium constant K for this reaction is K₂ = 10. 22. What is the correct form of the equilibrium constant K for this reaction? (A) Kc = (B) Kc = (C) Kc = 2[NH3] [N₂] + 3[H₂] (D) Kc = (E) Kc = [N₂][H₂]³ [N₂] + 3[H₂] 2[NH3] [NH3]² [N₂] [H₂] 3³ 3 [N₂] [H₂]³ 2 [NH3]²