Suppose a 250. mL flask is filled with 1.8 mol of Cl₂, 1.0 mol of HCl and 1.1 mol of CCI. The following reaction becomes possible: Cl₂(g) + CHCl3(g) → HCl(g) +CCI(g) The equilibrium constant K for this reaction is 0.480 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places. M

Suppose a 250. mL flask is filled with 1.8 mol of Cl₂, 1.0 mol of HCl and 1.1 mol of CCI. The following reaction becomes possible: Cl₂(g) + CHCl3(g) → HCl(g) +CCI(g) The equilibrium constant K for this reaction is 0.480 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places. M

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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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 2.0 L flask with 4.7 atm of sulfur dioxide gas and 0.67 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 0.80 atm. Calculate the pressure 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 = 0 P 0 x10
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6.
Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 5.96 × 104: H₂(g) + Cl₂(g) →2 HCl(g) Use this information to complete the following table. Suppose a 46. L reaction vessel is filled with 1.8 mol of HCI. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 HCl(g) H₂(g) + Cl₂(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 H₂(g)+2Cl₂(g) 4 HCl(g) ܢܢ There will be very little H₂ and Cl₂. There will be very little HCI. Neither of the above is true. K = 0 K = 0 x10 X 0/3 ? olo 18 Ar BA
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Suppose a 250. mL flask is filled with 1.2 mol of OCl,, 1.9 mol of BrOCl and 1.6 mol of BrCl. The following reaction becomes possible: Br,(g) +OCl,(g) BROCI(g) +BrC1(g) The equilibrium constant K for this reaction is 1.94 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places.
Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 924.: CO(g) + H₂O(g) → CO₂(g) + H₂(g) Use this information to complete the following table. Suppose a 17. L reaction vessel is filled with 0.75 mol of CO₂ and 0.75 mol of H₂. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. CO₂(g) + H₂(9) CO(g)+H₂O(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 3 CO(g) + 3H₂O(g) P 3 CO₂(g) + 3H₂(9) There will be very little CO and H₂O. There will be very little CO2 and H₂. Neither of the above is true. K = 0 K = 0 ■ x10 X ? 00. Ar 8.
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N₂(g) + 3 H₂ (g) 2 NH₂ (g) K₂= 6. × 10¯6 He fills a reaction vessel at this temperature with 5.0 atm of nitrogen gas and 2.4 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NH3 at right. Round your answer to 1 significant digit. yes no atm x₁ x10 × Ś
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Suppose a 500. ml. flask is filled with 0.60 mol of Br₂, 0.70 mol of BrOCI and 0.20 mol of BrCl. The following reaction becomes possible: Br₂(g) +OCI, (8) BrOCI(g) + BrCI(g) The equilibrium constant K for this reaction is 7.17 at the temperature of the flask Calculate the equilibrium molarity of OCI, Round your answer to two decimal places. M