Suppose a 250. mL flask is filled with 1.6 mol of CO, 2.0 mol of H,0 and 0.90 mol of CO,. The following reaction becomes possible:(3)H+(3)0ɔ= (3)0°H+(3)0)The equilibrium constant K for this reaction is 0.735 at the temperature of the flask.Calculate the equilibrium molarity of CO. Round your answer to two decimal places.OM

Moles of CO = 1.6 molMoles of H2O = 2.0 molMoles of CO2 =0.9 molK = 0.735

Suppose a 250. mL flask is filled with 1.6 mol of CO, 2.0 mol of H,0 and 0.90 mol of CO,. The following reaction becomes possible: Co (g) + H,O(g) – Co,g)+H,(g) The equilibrium constant K for this reaction is 0.735 the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.

Suppose a 250. mL flask is filled with 1.6 mol of CO, 2.0 mol of H,0 and 0.90 mol of CO,. The following reaction becomes possible: Co (g) + H,O(g) – Co,g)+H,(g) The equilibrium constant K for this reaction is 0.735 the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.

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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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
O KINETICS AND EQUILIBRIUM 1/5 Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 1.1 mol of Cl,, 0.20 mol of HCl and 0.80 mol of CCl,. The following reaction becomes possible: Cl,(g) +CHCI, (g) = HCl(g)+CCl, (g) The equilibrium constant K for this reaction is 9.65 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. | M II
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General Chemistry 4th Edition McQuarrie Rock Gallogly University Science Books presented by Macmillan Learning For the chemical equation SO, (g) + NO, (g) = SO,(g) + NO(g) the equilibrium constant at a certain temperature is 2.10. At this temperature, calculate the number of moles of NO, (g) that must be added to 2.64 mol SO, (g) in order to form 1.20 mol SO, (g) at equilibrium. 3 moles of NO,(g): mol 2. Question Source: MRG - General Chemistry | Publish privacy policy | help terms of use contact us about us careers (? ^ N EV prime video W
Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 125. L tank with 11. mol of sulfur dioxide gas and 35. mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 7.7 mol. Calculate the concentration equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K. = |
Suppose a 250. ml. flask is filled with 0.20 mol of NO,, 1.6 mol of CO and 0.90 mol of NO. The following reaction becomes possible: NO,()+co(2) NO()+co,@) The equilibrium constant K for this reaction is 0.402 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
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