7. What change could have been imposed on the system shown at right? A. Reactant was added B. Reactant was removed NH3 C. The temperature was changed D. The volume was decreased H₂ E. The volume was increased N₂ 8. The equilibrium constant for a reaction at equilibrium is 4.00. If the reaction were written in the reverse direction, which number below would be the value of the equilibrium constant? A. 2.00 C. 0.250 B. 16.0 D. 0.500 E. 0.125 9. Which of the following is considered a Brønsted-Lowry base, but not an Arrhenius base? B. potassium hydroxide A. calcium hydroxide C. ammonia D. hydrogen fluoride Concentration (mol/L)

7. What change could have been imposed on the system shown at right? A. Reactant was added B. Reactant was removed NH3 C. The temperature was changed D. The volume was decreased H₂ E. The volume was increased N₂ 8. The equilibrium constant for a reaction at equilibrium is 4.00. If the reaction were written in the reverse direction, which number below would be the value of the equilibrium constant? A. 2.00 C. 0.250 B. 16.0 D. 0.500 E. 0.125 9. Which of the following is considered a Brønsted-Lowry base, but not an Arrhenius base? B. potassium hydroxide A. calcium hydroxide C. ammonia D. hydrogen fluoride Concentration (mol/L)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 2RQ: What is the law of mass action? Is it true that the value of K depends on the amounts of reactants...

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Similar questions

In Section 13.1 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 to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
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The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.
Consider the system 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H20(ℓ) ΔrH° = −1530.4 kJ/mol How will the amount of ammonia at equilibrium be affected by removing O2(g) without changing the total gas volume? adding N2(g) without changing the total gas volume? adding water without changing the total gas volume? expanding the container? increasing the temperature? Which of these changes (i to v) increases the value of K? Which decreases it?
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