A sealed reaction vessel initially contains 1.839×10-2 moles of water vapor and 1.301x10-2 moles of CO(g). H,0(g) +CO(g) =H,(g)+CO,(g) After the above reaction has come to equilibrium, the vessel contains 8.326×103 moles of CO2(g).

A sealed reaction vessel initially contains 1.839×10-2 moles of water vapor and 1.301x10-2 moles of CO(g). H,0(g) +CO(g) =H,(g)+CO,(g) After the above reaction has come to equilibrium, the vessel contains 8.326×103 moles of CO2(g).

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

Suppose a 250. mL flask is filled with 1.6 mol of CH, 1.8 mol of H,O and 0.70 mol of CO. This reaction becomes possible: () +H,0(g) C0(g) +3H,(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity CO. You can leave out the M symbol for molarity. CH, H,0 CO H, initial change equilibrium Explanation Check © 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use| Privacy I Accessibility 口ロ X
A sealed reaction vessel initially contains 1.217×10-2 moles of water vapor and 1.678×10-2 moles of CO(g). H2O(g)+CO(g)H2(g)+CO2(g) After the above reaction has come to equilibrium, the vessel contains 8.326×10-3 moles of CO2(g) What is the value of the equilibrium constant Kc of the reaction at the temperature of the vessel?
Consider the following reactions and their respective equilibrium constants: NO (g) + ½ Brz (g) NOBI (g) K1 = 5.3 2 NO (g) + 02 (g)= N204 (g) K2 = 2.1 x 10-5 N204 (g) = N2 (g) + 2 O2 (g) K3 = 4.8 x 1025 se reactions and their equilibrium constants to predict the equilibrium constant for owing reaction: N2 (g) + O2 (g) + Br2 (g) 2 NOB1 (g)
The equilibrium constant, K, for the following reaction is 9.52x102 at 350 K. CH4 (g) + CCI4 (g) 2 CH,Cl2 (g) Calculate the equilibrium concentrations of reactants and product when 0.262 moles of CH, and 0.262 moles of CCl, are introduced into a 1.00 L vessel at 350 K. [ CH4] [ CC4] [ CH,Cl, ] = M M M
At a certain temperature, the equilibrium constant K for the following reaction is 3.44 x 10°: NO, (g) + CO(g)= NO(g) + CO,(g) Use this information to complete the following table. Suppose a 50. L reaction vessel is filled with 0.81 mol of NO2 and 0.81 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little NO2 and CO. x10 There will be very little NO and CO2. ? Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K =0 NO(g)+CO2(9) NO2(9)+CO(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. = 0 K = 2 NO,(9)+2CO(9) 2 NO(9)+2CO2(9)
The reaction N2(g) + 3 H2(g) ⇀↽ 2 NH3(g), has an equilibrium constant of 4.0 × 108 at 25◦C. What will eventually happen if 44.0 moles of NH3, 0.452 moles of N2, and 0.108 moles of H2 are put in a 10.0 liter container at 25◦C? More N2 and H2 will be formed. Nothing; the system is at equilibrium. More NH3 will be formed.
Calculating an equilibrium constant from a partial equilibrium composition Steam reforming of methane ( CH4 ) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 1.5 L flask with 4.3 atm of methane gas and 1.8 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 3.2 atm. Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K p 11] ☐ x10 ☑ ⑤
Consider the equilibrium system described by the chemical reaction below. For this reaction, Kc = 2.4 x 103 at a particular temperature. If the equilibrium concentrations of H,0 and H, are 0.11 M and 0.019 M, respectively, determine the concentration of O, at equilibrium.. 2 2 H,O(g) = 2 H,(g) + 0,(g) 2 NEXT > If [x] represents the equilibrium concentration of O, set up the equilibrium expression for Kc to solve for the concentration. Do not combine or simplify terms.. 2' K. = = 2.4 x 103 5 RESET [О.11] [0.019] 2[0.11] 2[0.019] [0.11]? [0.019]? [x] [x]? [2x] [2x]?
At a certain temperature, the equilibrium constant K for the following reaction is 6.0 x 10: co(e) + H,0(g) -co,() + H,(g) Use this information to complete the following table. Suppose a 31. L reaction vessel is filled with 1.1 mol of co, and 1.1 mol of H2. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little CO and H,0. O There will be very little Co, and H,. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] Co,(0)+H,(0) CO()+H,O(9) 1. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] 3 CO0g)+3H,0(9) 3 CO,(0)+3H,(9) 1.
Suppose à 250. mL flask is filled with 1.3 mol of CO, 1.8 mol of H,O and 1.6 mol of H,. This reaction becomes possible: co() +H,0(g) =CO,e)+H,(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of H,. You can leave out the M symbol for molarity. CO H,0 Co, H, initial change equilibrium Explanation Check © 2021 McGraw-Hill Education. All Rights Roserved Terms of Use Privacy 1 Ace O Type here to search
When 7.121 x 10-1 mol of NH3 and 7.121 x 10-1 mol of O2 are introduced into a 2.305 L reaction vessel at a certain temperature a chemist finds that at equilibrium the N2 concentration is 1.003 x 10-1 M: 4NH3(g) + 3O2(g) <==> 2N2(g) + 6H2O (g) What is the value of Kc for this reaction ?
Suppose a 500. mL flask is filled with 0.30 mol of SO, and 1.2 mol of SO3. This reaction becomes possible: 2SO, (g) +O,(g) 2SO3 Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O,. You can leave out the M symbol for molarity. so, SO2 O2 initial change equilibrium