What would be the effect of increasing the temperature on each of the following systems at...
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) ---------->2HI(g) 1) Calculate the equilibrium concentrations of reactants and product when 0.309 moles of H2 and 0.309 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = M? [I2] = M? [HI] = M? 2.The equilibrium constant, K, for the following reaction is 1.20×10-2 at 500 K: PCl5(g)------->PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a...
1. Write the equilibrium constant expressions (Kc) for the following reactions: (a) CO (g) + H2O (g) ⮂ CO2 (g) + H2 (g) (b) CH4 (g) + 2H2S (g) ⭢ CS2 (g) + 4H2 (g) (c) COCl2 (g) ⮂ Cl2 (g) + CO (g) (d) 2HI (g) ⮂ H2 (g) + I2 (g) (e) PCl3 + Cl2 (g) ⮂ PCl5 (g) (f) 2H2 (g) + O2 (g) ⮂ ...
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. 2NH3(g)⇌N2(g)+3H2(g)Kc=17; [NH3] = 0.20 M, [N2] = 1.00 M, [H2] = 1.00 M (b) 2NH3(g)⇌N2(g)+3H2(g)KP=6.8×104; NH3 = 3.0 atm, N2 = 2.0 atm, H2 = 1.0 atm (c) 2SO3(g)⇌2SO2(g)+O2(g)Kc=0.230; [SO3] = 0.00 M, [SO2] = 1.00 M, [O2] = 1.00 M (d) 2SO3(g)⇌2SO2(g)+O2(g)KP=16.5; SO3 = 1.00...
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (d) 2SO3 (g) ⇌ 2SO2 (g) + O2 (g) KP = 16.5; initial pressures: SO3 = 1.00 atm, SO2 = 1.00 atm, O2 = 1.00 atm (e) 2NO(g) + Cl2 (g) ⇌ 2NOCl(g) Kc = 4.6 × 104 ; [NO] = 1.00 M, [Cl2] = 1.00...
(A) Does the equilibrium mixture contain products, reactants, both or none? (A1) 2O3(g) ⇌ 3O2(g) K = 5.9 x 1012 (A2) H2(g) + I2(g) ⇌ 2HI(g) K = 54 (C) Write the expression for Kc (C Part 1) PCl3(l) +Cl2(g) ⇌ PCl5(s) (a) Kc = [PCl5]/([PCl3] [Cl2]) (b) Kc = ([PCl3] [Cl2])/[PCl5] (c) Kc = 1/([PCl3] [Cl2]) (d) Kc = 1/[Cl2] (C Part 2) Fe3O4(s) + 4H2(g) ⇌ 3Fe(s) + 4H2O(g) (a) Kc = ([Fe]3[H2O]4)/( [Fe3O4] [H2]4) (b) Kc =...
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCl3(g) + Cl2(g) = PCl5(g) Calculate the equilibrium concentrations of reactant and products when 0.249 moles of PCl3 and 0.249 moles of Cl2 are introduced into a 1.00 L vessel at 500 K. [PCl3] = M [Cl2] = M [PCl5] = M The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) = H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and...
Please answer ALL of the parts! Thank you and hope you're staying safe :) A) Consider the following reaction: PCl5(g) PCl3(g) + Cl2(g) If 7.65×10-3 moles of PCl5, 0.257 moles of PCl3, and 0.284 moles of Cl2 are at equilibrium in a 18.1 L container at 616 K, the value of the equilibrium constant, Kp, is __________. B) Consider the following reaction: 2HI(g) H2(g) + I2(g) If 1.44 moles of HI, 0.258 moles of H2, and 0.211 moles of I2...
1. The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and use it to determine the direction in which each system will proceed to reach equilibrium. Write "R" if the reactions shifts to the right towards products or "L" if it shifts left towards reactants. A. {NO} = 1.00 M, {Cl2} = 1.00 M, {NOCl} = 0.00 M; K = 4.6 x 104 2NO(g)+Cl2(g)<->2NOCl(g) B. {SO3} = 2.00...
8. Which of the following reactions cannot proceed through a single elementary step in view of the experimental rate law given? (a) NO(g) + O3(g) ⟶ NO2(g) + O2(g) rate = k[NO][O3] (b) 2HI(g) ⟶ H2(g) + I2(g) rate = k[HI]2 (c) C4H8(g) ⟶ 2C2H4(g) rate = k[C4H8] (d) 2NO(g) + H2(g) ⟶ N2(g) + H2O(g) rate = k[NO][H2] (e) 2NO(g) + Cl2(g) ⟶ 2NOCl(g) rate = k[NO]2[Cl2] The worksheet says that the answer is D, but I don’t get...
1) The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) H2(g) + I2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 698 K contains 0.311 M HI, 4.18×10-2 M H2 and 4.18×10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 2.85×10-2 mol of I2(g) is added to the flask? 2) The equilibrium constant, K, for the following reaction is 1.20×10-2 at...