Review I Constants I Periodic TablePart BThe following reaction was carried out in a 4.00 L reaction vessel at 1100 K:C(s) + H20(g) =CO(g)+H2(g)If during the course of the reaction, the vessel is found to contain 6.75 mol of C, 14.0 mol of H,O, 3.70 mol of CO, and 8.80 mol of H2, what is thereaction quotient Q?Enter the reaction quotient numerically.• View Available Hint(s)Q =SubmitPart CThe reaction2CH4(g) = C2H2(g) + 3H2(g)has an equilibrium constant ofK = 0.154.If 6.40 mol of CH, 4.20 mol of C,H2, and 11.70 mol of H2 are added to a reaction vessel with a volume of 5.10 L, what net reaction will occur?> View Available Hint(s)O The reaction will proceed to the left to establish equilibrium

As per the guideline, Since you have asked multiple questions, we have solved the first question for…

Answered: Part B The following reaction was…

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...

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Consider the following reaction that has a Kc = 2.4 x 10^-3 at 1000K: N2(g) + 3 H2(g) = 2NH3(g) in a reaction vessel that is 5.0 x 10^3 L, 250 moles of N2, 250 mol of H2, and 50.0 mol of NH3 are mixed. write the reaction quotient. Calculate Qc.
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. (The system is considered in equilibrium if Kc and Qc are within 5% of each other.) (a) 2 NH3(g) equalibrium arrow N2(g) + 3 H2(g), [NH3]i = 0.400 M, [N2]i = 0.155 M, [H2]i = 0.110 M, Kc = 16 What is the reaction quotient? What direction will the reaction shift to? (b) 2 NH3(g) equalibrium arrow N2(g) + 3 H2(g), Pi(NH3) = 2.10 atm, Pi(N2) = 10.70 atm, Pi(H2) = 10.70 atm, Kp = 8.3 ✕ 104 What is the reaction quotient? What direction will the reaction shift to? (c) 2 SO3(g) equalibrium arrow 2 SO2(g) + O2(g), [SO3]i = 1.90 M, [SO2]i = 1.90 M, [O2]i = 1.90 M, Kc = 0.23 What is the reaction quotient? What direction will the reaction shift to? (d) 2 SO3(g) equalibrium arrow 2 SO2(g) + O2(g), Pi(SO3) = 0.100 atm, Pi(SO2) =…
Consider the gas-phase reaction for the synthesis of methanol from CO(g) and H₂(g) CO(g) + 2 H₂(0)=CH₂OH(g) The value of the equilibrium constant Kp at 495 K is 1.42 x 10-2. Initially equimolar amounts of CO(g) and H₂(g) are introduced into the reaction vessel. Determine the value of Sea/no at equilibrium at 495 K and 29 bar. X
For the following reaction: A(g) + 3 B(g) magnitude of Kp (don't report the units) assuming the following composition at equilibrium: PA = 0.735 bar PB = 0.603 bar Pc = 0.627 bar PD 0.87 bar = 2 C(g) + D(g) Calculate the =
Given the following equilibrium constants at 700K, 2 N2O(g) (double arrow) 2 N2 (g) + O2(g) K1 = 8.2 x 1033NO2(g) (double arrow) 1⁄2 N2(g) + O2(g) K2 = 2.44 x 108N2O4(g) (double arrow) 2 NO2(g) K3 = 4.6 x 10-3 determine the values of the equilibrium constants for the following reaction. Show your equation-buildingprocess and your calculations. 2 N2O4(g) (double arrow) 2 N2O(g) + 3 O2(g) K =
A mixture of 0.04096 mol of C₂H6, 0.05994 mol of N₂, 0.04520 mol of NH3, and 0.02898 mol of C₂H4 is placed in a 1.0-L steel pressure vessel at 1900 K. The following equilibrium is established: 3 C₂H6(9) + 1 N₂(9)=2 NH3(g) + 3 C₂H4 (9) At equilibrium 0.02365 mol of C₂H4 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of C₂H6, N₂, NH3, and C₂H₁. Peq(C₂H6) Peq(N₂) = Peq(NH3)= Peq(C₂H4)= (b) Calculate Kp for this reaction. Kp =
25. Professor Schwartz runs the same reaction given in problem 23, but starts from different initial concentrations of the reactants and products. He places 1.0 mol of NH3, 1.0 mol of N2, and 2.0 mol of H₂ and in a sealed 1.0 L container at T = 740 K. What is the initial value of the reaction quotient in Professor Schwartz' experiment? (A) Qc = 0.125 (B) Qc = 0.50 (C) Qc = 1.0 (D) Qc = 2.0 (E) Qc = 10.0
6. Consider the following reaction: CO(g) + H2O(g) CO2(g) + H2(g) Ko = 0.58 at 1273 K* A sealed 4.00L vessel initially contains 1.00 mole CO2(g), 1.00 mole H2(g), 0.600 moles CO(g), and 0.600 moles of H2O(g). Calculate the moles of H2(g) present at equilibrium. The NG Reference: General Chemistry 8th Ed: Ebbing and Gammon: 2005 by Houghton Mifflin. New York. page 654, print 68
A mixture of 0.02233 mol of C2H6, 0.02937 mol of N2, 0.03719 mol of NH3, and 0.03411 mol of C2H4 is placed in a 1.0-L steel pressure vessel at 2646 K. The following equilibrium is established: 3 C2H6(g) + 1 N2(g) 2 NH3(g) + 3 C2H4(g) At equilibrium 0.01682 mol of C2H6 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of C2H6, N2, NH3, and C2H4.Peq(C2H6) = Peq(N2) = Peq(NH3) = Peq(C2H4) = (b) Calculate KP for this reaction.KP =
For the equilibrium reaction. 2IBr (g) I2 (g) + Br2 (g) Kc=.0085. If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components. Consider the decomposition reaction at 555 K 4POCl3 (g) P4 (g) + 2O2 (g) + 6Cl2 (g) If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm. Find Kp and Kc.
A methanol synthesis reaction will be run in a container with a moveable piston to allow for changes in volume. The gas phase reaction is illustrated below: CO(g) + 2H2(g) = CH3OH(g) At equilibrium, the reaction is run at 400K in a 10L flask; there are 3.09 moles of CO and 1.11 moles H₂ initially. At constant volume, 0.830 mol H2(g) is added to the reaction. Solve for the partial pressures of the gases in the container when the reaction returns to equilibrium. Really not sure how I should solve this problem, please help me out my showing step by step what I should do. Thanks :)
A mixture of 0.02993 mol of O2, 0.02165 mol of NOCl, 0.02691 mol of NO2, and 0.01037 mol of Cl2 is placed in a 1.0-L steel pressure vessel at 2385 K. The following equilibrium is established: 1 O2(g) + 2 NOCl(g) 2 NO2(g) + 1 Cl2(g) At equilibrium 0.008268 mol of Cl2 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of O2, NOCl, NO2, and Cl2.Peq(O2) = .Peq(NOCl) = .Peq(NO2) = .Peq(Cl2) = .(b) Calculate KP for this reaction.KP = .

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