O Kinetics and EquilibriumCalculating equilibrium composition from an equilibrium constantSuppose a 500. mL flask is filled with 0.50 mol of H2 and 2.0 mol of Cl₂. The following reaction becomes possible:H2(g) +Cl₂(g)2HCl(g)The equilibrium constant K for this reaction is 4.39 at the temperature of the flask.Calculate the equilibrium molarity of HCl. Round your answer to two decimal places.ОмMхS0/5

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Answered: O Kinetics and Equilibrium Calculating…

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 a 250.mL flask is filled with 0.50mol of CO , 0.10mol of NO and 1.6mol of CO2 . The following reaction becomes possible: +NO2gCOg +NOgCO2g The equilibrium constant K for this reaction is 7.24 at 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 1.0 mol of NO₂, 0.20 mol of NO and 1.7 mol of CO₂. The following reaction becomes possible: NO₂(g) +CO(g) NO(g) +CO, (g) The equilibrium constant K for this reaction is 5.54 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M Images X
Setting up a reaction table Suppose a 250. mL flask is filled with 2.0 mol of SO₂ and 1.1 mol of SO3. This reaction becomes possible: 2SO₂(g) + O₂(g)2SO₂ (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 O₂. You can leave out the M symbol for molarity. initial change equilibrium SO2 3 0₂ 0 X SO3 X Ś 000 18 Ar 8.
Suppose a 250. mL flask is filled with 2.0 mol of NO and 1.0 mol of NO₂. The following reaction becomes possible: NO₂(g)+NO(g) — 2NO₂(g) The equilibrium constant K for this reaction is 2.73 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places. M S
Suppose a 500. mL flask is filled with 1.5 mol of H₂O, 0.10 mol of CO₂ and 1.7 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 0.980 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. M X
Suppose a 250. mL flask is filled with 1.2 mol of Br₂, 0.50 mol of BrOCl and 1.9 mol of BrC1. The following reaction becomes possible: Br₂(g) + OC1₂(g) → BrOC1 (g) + BrC1 (g) The equilibrium constant K for this reaction is 0.156 at the temperature of the flask. Calculate the equilibrium molarity of OC12. Round your answer to two decimal places. |] M X Ś ?
Suppose a 250. mL flask is filled with 0.90 mol of Cl₂, 1.2 mol of HCl and 2.0 mol of CC14. The following reaction becomes possible: Cl2(g) + CHCl3(g) → HCl(g) + CCl4(g) The equilibrium constant K for this reaction is 0.702 at the temperature of the flask. Calculate the equilibrium molarity of CHC13. Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 1.7 mol of CO, 0.50 mol of CO2 and 0.90 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) → CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 1.14 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X Ś
Suppose a 250. mL flask is filled with 1.2 mol of NO and 0.90 mol of NO 2. The following reaction becomes possible: NO3(g) + NO(g) = 2NO2(g) The equilibrium constant K for this reaction is 0.661 at the temperature of the flask. Calculate the equilibrium molarity of NO 3. Round your answer to two decimal places. Ом ☑
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Chemistry
Suppose a 500. mL flask is filled with 1.9 mol of N, and 0.20 mol of NO. The following reaction becomes possible: N₂(g) + O₂(g) → 2NO(g) The equilibrium constant K for this reaction is 3.27 at the temperature of the flask. Calculate the equilibrium molarity of N₂. Round your answer to two decimal places.

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