Suppose a 250. mL flask is filled with 0.50 mol of H2 and 0.60 mol of 12. The following reaction becomes possibleH2(g) +12(g) 2HI (g)The equilibrium constant K for this reaction is 9.83 at the temperature of the flask.Calculate the equilibrium molarity of H2. Round your answer to two decimal places.ОмX

Answered: Image /qna-images/answer/5ad55358-b54c-44b1-a7ed-bd91864e6170.jpg

Answered: Suppose a 250. mL flask is filled with…

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 1.8mol of I2 and 1.4mol of HI. The following reaction becomes possible: +H2(g)+I2(g)--->2HI(g) The equilibrium constant K for this reaction is 1.03 at the temperature of the flask. Calculate the equilibrium molarity of I2 . Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 1.9 mol of H, and 1.1 mol of NH,. This reaction becomes possible: N2 (g) +3H,(g) = 2NH,(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 N,. You can leave out the M symbol for molarity. N2 H, NH, initial change х equilibrium
Suppose a 500. mL flask is filled with 1.0 mol of H₂ and 1.7 mol of I₂. The following reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) ܢܢ The equilibrium constant K for this reaction is 6.78 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places. M 3
Suppose a 250. ml. flask is filled with 1.1 mol of N₂ and 1.4 mol of O₂. The following reaction becomes possible: N₂(g) + O₂(g) 2NO(g) The equilibrium constant K for this reaction is 3.80 at the temperature of the flask. Calculate the equilibrium molarity of N₂. Round your answer to two decimal places. OM pak X
Suppose a 500. mL flask is filled with 1.8 mol of H₂ and 1.5 mol of HI. The following reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) The equilibrium constant K for this reaction is 9.08 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 1.7 mol of N₂ and 1.3 mol of NO. The following reaction becomes possible: N₂(g) + O₂(g) 2NO(g) The equilibrium constant K for this reaction is 0.788 at the temperature of the flask. Calculate the equilibrium molarity of N₂. Round your answer to two decimal places. 3
Suppose a 250. mL flask is filled with 0.90 mol of N, and 1.7 mol of NO. The following reaction becomes possible: N,(g) +0,(g) = 2NO(g) The equilibrium constant K for this reaction is 0.694 at the temperature of the flask. Calculate the equilibrium molarity of 0,. Round your answer to two decimal places. 21
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
Suppose a 250. mL flask is filled with 0.60 mol of NO, and 0.80 mol of O,. This reaction becomes possible: 2NO,(g) = 2NO(g)+O,(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 O,. You can leave out the M symbol for molarity. NO, NO O2 initial change equilibrium 미미
Suppose a 500. mL flask is filled with 1.2 mol of H, and 2.0 mol of HCl. The following reaction becomes possible: H,(2) + Cl,(g) = 2HCI(g) The equilibrium constant K for this reaction is 0.641 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. ?
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 250. mL flask is filled with 1.5 mol of CO, 0.30 mol of H,O and 1.3 mol of H,. The following reaction becomes possible: CO(g) +H,0(g)– CO2(g)+H,(g) The equilibrium constant K for this reaction is 1.25 at the temperature of the flask. Calculate the equilibrium molarity of H,O. Round your answer to two decimal places. OM

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