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 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 :)

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

The reaction N204(g) 2NO2(g) has a K, = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N204 was 0.127 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of NO2 = i atm (b) What was the total pressure of the mixture of gases? total pressure = i atm
A mixture of 0.06529 mol of CH4, 0.04045 mol of H2S, 0.06585 mol of CS2, and 0.03325 mol of H2 is placed in a 1.0-L steel pressure vessel at 1304 K. The following equilibrium is established: 1 CH4(g) + 2 H2S(g) 1 CS2(g) + 4 H2(g) At equilibrium 0.01420 mol of H2 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2.Peq(CH4) = ______ .Peq(H2S) = ______ .Peq(CS2) = ______ .Peq(H2) = _______ .(b) Calculate KP for this reaction.KP = _______ .
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) =…
A closed 1.00 L system initially containing 0.00200 mol H₂ and 0.00500 mol 1₂ at a given temperature is allowed to reach equilibrium Analysis of the equilibrium mixture shows that the amount of HI present at equilibrium is 0.00371 mol. Calculate the Kc at this temperature for the reaction. State whether the equilibrium is product-favored or reactant- favored at this temperature. H₂(g) +1₂(g) 2H1(g) Kc 31: The equilibrium is product-favored. Kc 31: The equilibrium is reactant-favored. Kc 0.032; The equilibrium is reactant-favored. Kc - 0.032; The equilibrium is product-favored.
A student ran the following reaction in the laboratory at 479 K: PCI3(g) + Cl₂(g) =PC15(g) When she introduced PCI3(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of PCI3 was 2.13 atm and the initial partial pressure of Cl₂ was 1.34 atm, she found that the equilibrium partial pressure of PCI5 was 1.12 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp Submit Answer Retry Entire Group 8 more group attempts remaining
As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C
please indiciate whether the pressure will decrease, increase, or not change. Also please indicate what the shift in equilibrium will be
The reaction N204(s) * 2NO2(3) has a K, = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N204 was 0.183 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of N02 = atm (b) What was the total pressure of the mixture of gases? total pressure = atm