Suppose a 500. mL flask is filled with 0.20 mol of Cl, and 1.5 mol of HCI. The following reaction becomes possible: H,(g) +Cl, (g) → 2HCI(g) The equilibrium constant K for this reaction is 0.754 at the temperature of the flask. Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places. OM A

Suppose a 500. mL flask is filled with 0.20 mol of Cl, and 1.5 mol of HCI. The following reaction becomes possible: H,(g) +Cl, (g) → 2HCI(g) The equilibrium constant K for this reaction is 0.754 at the temperature of the flask. Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places. OM A

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 38A

See similar textbooks

Similar questions

Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
12.85 In the figure, orange fish are placed in one aquarium and green fish in an adjoining aquarium. The two tanks are separated by a removable partition that is initially closed. Describe what happens in the first few minutes after the partition is opened. WTiat would you expect to see several hours later? How is this system analogous to dynamic chemical equilibrium?
In Section 17.3 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term “closed system,” and why is it necessary for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
5.2. What is the difference between a static equilibrium and a dynamic equilibrium? Give examples difference from the examples in the text. What is similar for the two types of equilibria?
At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
5.19. Assume that a reaction exists such that equilibrium occurs when the partial pressures of the reactants and products are all . If the volume of the system were doubled, all of the partial pressures would be . Would the system still be at equilibrium? Why or Why not?
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Hydrogen, bromine, and HBr in the gas phase are in equilibrium in a container of fixed volume. H2(g) + Br2(g) 2 HBr(g) rH = 103.7 kJ/mol How will each of these changes affect the indicated quantities? Write increase, decrease, or no change.