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State changes such as evaporation can also be described as equilibrium reactions. For example: AB2 (1) AB2 (9) Kc = 1.40 x 10³ at 25°C Question 9: A scientist adds 0.450 mol of liquid AB₂ (1) and 0.0100 mol of the vapour AB₂ (g) to an empty 10.0 L container at 25°C. Assumptions: the container as a fixed volume once filled and sealed, no matter can escape from the container the volume occupied by the liquid inside the container is very small A student is asked to answer the following two questions on the exam: a. Which direction must be favored by the system to reach equilibrium? b. What will be the final amounts of both compounds once equilibrium is reached? To solve the problem, the student set up the ICE table below. Analyze the student work. Do you agree or disagree with the approach? If you disagree, how would you modify it and why? • • Are the +/-signs for the "change" row properly set up? Is the equation to solve x properly set up? Initial AB₂ (1) 0.450 mol Change Equilibrium (0.450 - x) mol - X AB; (g) 0.0100 mol (0.0100 + x) mol 1.40 x 10³ = (0.0100 + x) mol (0.450 - x) mol Comments: When you've analyzed the student work, finish solving the problem and find the final amounts of each compound present in the container once the equilibrium state is reached. Amount of AB₂ (I) = Amount of AB₂ (g) =

State changes such as evaporation can also be described as equilibrium reactions. For example: AB2 (1) AB2 (9) Kc = 1.40 x 10³ at 25°C Question 9: A scientist adds 0.450 mol of liquid AB₂ (1) and 0.0100 mol of the vapour AB₂ (g) to an empty 10.0 L container at 25°C. Assumptions: the container as a fixed volume once filled and sealed, no matter can escape from the container the volume occupied by the liquid inside the container is very small A student is asked to answer the following two questions on the exam: a. Which direction must be favored by the system to reach equilibrium? b. What will be the final amounts of both compounds once equilibrium is reached? To solve the problem, the student set up the ICE table below. Analyze the student work. Do you agree or disagree with the approach? If you disagree, how would you modify it and why? • • Are the +/-signs for the "change" row properly set up? Is the equation to solve x properly set up? Initial AB₂ (1) 0.450 mol Change Equilibrium (0.450 - x) mol - X AB; (g) 0.0100 mol (0.0100 + x) mol 1.40 x 10³ = (0.0100 + x) mol (0.450 - x) mol Comments: When you've analyzed the student work, finish solving the problem and find the final amounts of each compound present in the container once the equilibrium state is reached. Amount of AB₂ (I) = Amount of AB₂ (g) =

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 113QRT
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A scientist adds 0.450 mol of liquid AB 2 (l) and 0.0100 mol of the vapour AB 2 (g) to an empty 10.0 L
container at 25°C.

State changes such as evaporation can also be described as equilibrium reactions. For example: AB2 (1) AB2 (9) Kc = 1.40 x 10³ at 25°C Question 9: A scientist adds 0.450 mol of liquid AB₂ (1) and 0.0100 mol of the vapour AB₂ (g) to an empty 10.0 L container at 25°C. Assumptions: the container as a fixed volume once filled and sealed, no matter can escape from the container the volume occupied by the liquid inside the container is very small A student is asked to answer the following two questions on the exam: a. Which direction must be favored by the system to reach equilibrium? b. What will be the final amounts of both compounds once equilibrium is reached? To solve the problem, the student set up the ICE table below. Analyze the student work. Do you agree or disagree with the approach? If you disagree, how would you modify it and why? • • Are the +/-signs for the "change" row properly set up? Is the equation to solve x properly set up? Initial AB₂ (1) 0.450 mol Change Equilibrium (0.450 - x) mol - X AB; (g) 0.0100 mol (0.0100 + x) mol 1.40 x 10³ = (0.0100 + x) mol (0.450 - x) mol Comments: When you've analyzed the student work, finish solving the problem and find the final amounts of each compound present in the container once the equilibrium state is reached. Amount of AB₂ (I) = Amount of AB₂ (g) =
Transcribed Image Text:State changes such as evaporation can also be described as equilibrium reactions. For example: AB2 (1) AB2 (9) Kc = 1.40 x 10³ at 25°C Question 9: A scientist adds 0.450 mol of liquid AB₂ (1) and 0.0100 mol of the vapour AB₂ (g) to an empty 10.0 L container at 25°C. Assumptions: the container as a fixed volume once filled and sealed, no matter can escape from the container the volume occupied by the liquid inside the container is very small A student is asked to answer the following two questions on the exam: a. Which direction must be favored by the system to reach equilibrium? b. What will be the final amounts of both compounds once equilibrium is reached? To solve the problem, the student set up the ICE table below. Analyze the student work. Do you agree or disagree with the approach? If you disagree, how would you modify it and why? • • Are the +/-signs for the "change" row properly set up? Is the equation to solve x properly set up? Initial AB₂ (1) 0.450 mol Change Equilibrium (0.450 - x) mol - X AB; (g) 0.0100 mol (0.0100 + x) mol 1.40 x 10³ = (0.0100 + x) mol (0.450 - x) mol Comments: When you've analyzed the student work, finish solving the problem and find the final amounts of each compound present in the container once the equilibrium state is reached. Amount of AB₂ (I) = Amount of AB₂ (g) =
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