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A chemical engineer is studying the following reaction: 4 HC1(g) + 0₂(g) →2 H₂O(g)+2C1₂(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.31. The engineer charges ("fills") four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel A B с compound HCI 0₂ H₂O Cl₂ HCI %₂ H₂O C1₂ HCI 0₂ H₂O Cl₂ pressure 5.09 atm 5.63 atm 3.31 atm 4.48 atm 3.91 atm 5.34 atm 3.90 atm 5.07 atm 2.74 atm 5.05 atm 4.48 atm 5.65 atm expected change in pressure O↑ increase O ↑ increase ↑ increase increase ↑ increase O↑ increase ↑ increase Ot increase ↑ increase ↑ increase O † increase Ot increase O↓ decrease O↓ decrease O↓ decrease O↓ decrease O ↓ decrease O↓ decrease O↓ decrease O↓ decrease ↓decrease ↓ decrease O ↓ decrease O↓ decrease O (no change) O (no change) O (no change) O (no change) O (no change) O (no change) (no change) O (no change) (no change) (no change) O (no change) O (no change)

A chemical engineer is studying the following reaction: 4 HC1(g) + 0₂(g) →2 H₂O(g)+2C1₂(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.31. The engineer charges ("fills") four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel A B с compound HCI 0₂ H₂O Cl₂ HCI %₂ H₂O C1₂ HCI 0₂ H₂O Cl₂ pressure 5.09 atm 5.63 atm 3.31 atm 4.48 atm 3.91 atm 5.34 atm 3.90 atm 5.07 atm 2.74 atm 5.05 atm 4.48 atm 5.65 atm expected change in pressure O↑ increase O ↑ increase ↑ increase increase ↑ increase O↑ increase ↑ increase Ot increase ↑ increase ↑ increase O † increase Ot increase O↓ decrease O↓ decrease O↓ decrease O↓ decrease O ↓ decrease O↓ decrease O↓ decrease O↓ decrease ↓decrease ↓ decrease O ↓ decrease O↓ decrease O (no change) O (no change) O (no change) O (no change) O (no change) O (no change) (no change) O (no change) (no change) (no change) O (no change) O (no change)

Chemistry
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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**Kinetics and Equilibrium: Using an Equilibrium Constant to Predict the Direction of a Reaction** A chemical engineer is studying the following reaction: \[ 4 \text{HCl}(g) + \text{O}_2(g) \rightarrow 2 \text{H}_2\text{O}(g) + 2 \text{Cl}_2(g) \] At the temperature the engineer picks, the equilibrium constant \( K_p \) for this reaction is 0.31. The engineer charges four reaction vessels with hydrogen chloride and oxygen, allowing the reaction to begin. She measures the composition of the mixture inside each vessel periodically. The first set of measurements is shown in the table below. Predict how the compositions will change the next time she measures them. | Reaction Vessel | Compound | Pressure (atm) | Expected Change in Pressure | |:---------------:|:--------:|:--------------:|:---------------------------:| | A | HCl | 5.09 | ☐ increase ☐ decrease ☐ (no change) | | | O₂ | 5.63 | ☐ increase ☐ decrease ☐ (no change) | | | H₂O | 3.31 | ☐ increase ☐ decrease ☐ (no change) | | | Cl₂ | 4.48 | ☐ increase ☐ decrease ☐ (no change) | | B | HCl | 3.11 | ☐ increase ☐ decrease ☐ (no change) | | | O₂ | 5.34 | ☐ increase ☐ decrease ☐ (no change) | | | H₂O | 3.90 | ☐ increase ☐ decrease ☐ (no change) | | | Cl₂ | 5.07 | ☐ increase ☐ decrease ☐ (no change) | | C | HCl | 2.74 | ☐ increase ☐ decrease ☐ (no change) | | | O₂ | 5.05 | ☐ increase ☐ decrease ☐ (no change) | | | H₂O | 4.48 | ☐ increase
Transcribed Image Text:**Kinetics and Equilibrium: Using an Equilibrium Constant to Predict the Direction of a Reaction** A chemical engineer is studying the following reaction: \[ 4 \text{HCl}(g) + \text{O}_2(g) \rightarrow 2 \text{H}_2\text{O}(g) + 2 \text{Cl}_2(g) \] At the temperature the engineer picks, the equilibrium constant \( K_p \) for this reaction is 0.31. The engineer charges four reaction vessels with hydrogen chloride and oxygen, allowing the reaction to begin. She measures the composition of the mixture inside each vessel periodically. The first set of measurements is shown in the table below. Predict how the compositions will change the next time she measures them. | Reaction Vessel | Compound | Pressure (atm) | Expected Change in Pressure | |:---------------:|:--------:|:--------------:|:---------------------------:| | A | HCl | 5.09 | ☐ increase ☐ decrease ☐ (no change) | | | O₂ | 5.63 | ☐ increase ☐ decrease ☐ (no change) | | | H₂O | 3.31 | ☐ increase ☐ decrease ☐ (no change) | | | Cl₂ | 4.48 | ☐ increase ☐ decrease ☐ (no change) | | B | HCl | 3.11 | ☐ increase ☐ decrease ☐ (no change) | | | O₂ | 5.34 | ☐ increase ☐ decrease ☐ (no change) | | | H₂O | 3.90 | ☐ increase ☐ decrease ☐ (no change) | | | Cl₂ | 5.07 | ☐ increase ☐ decrease ☐ (no change) | | C | HCl | 2.74 | ☐ increase ☐ decrease ☐ (no change) | | | O₂ | 5.05 | ☐ increase ☐ decrease ☐ (no change) | | | H₂O | 4.48 | ☐ increase
Expert Solution
Step 1: Relation between reaction quotient and equilibrium constant

Answer:

Relation between reaction quotient QP and equilibrium constant KP is shown below:

1. When Q subscript P equals K subscript P reaction mixture is at equilibrium.

2. When Q subscript P less than K subscript P reaction mixture is not be at equilibrium and to establish the equilibrium reaction will move forward so that QP can increase and become equal to KP.

3. When Q subscript P greater than K subscript P reaction mixture is not at equilibrium and to establish the equilibrium reaction will move in reverse direction so that QP can decrease and become equal to KP.


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