A chem ngineer is studying the following reaction: 4 HCl(g) + O₂(g) → 2 H₂O(g) +2C1₂(g) At the temperature the engineer picks, the equilibrium constant Kp for this reaction is 0.17. 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 U с compound H CI 0₂ H₂O C1₂ H CI 0₂ H₂O C1₂ H CI 0₂ H₂O C1₂ pressure 6.10 atm 5.69 atm 9.07 atm 4.08 atm. 6.65 atm. 5.36 atm 7.21 atm 2.91 atm 4.19 atm. 4.74 atm 8.43 atm. 4.13 atm expected change in pressure Ot increase Ot increase ↑ Ot increase Ot increase Ot increase Ot increase Ot increase Ot increase ↑ increase Ot increase Ot increase Ot increase decrease O decrease O decrease Odecrease decrease Odecrease Odecrease Odecrease Odecrease Odecrease decrease Odecrease O(no change) O(no change) O(no change) O(no change) (no change) O(no change) O (no change) (no change) O (no change) O(no change) O(no change) (no change)
A chem ngineer is studying the following reaction: 4 HCl(g) + O₂(g) → 2 H₂O(g) +2C1₂(g) At the temperature the engineer picks, the equilibrium constant Kp for this reaction is 0.17. 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 U с compound H CI 0₂ H₂O C1₂ H CI 0₂ H₂O C1₂ H CI 0₂ H₂O C1₂ pressure 6.10 atm 5.69 atm 9.07 atm 4.08 atm. 6.65 atm. 5.36 atm 7.21 atm 2.91 atm 4.19 atm. 4.74 atm 8.43 atm. 4.13 atm expected change in pressure Ot increase Ot increase ↑ Ot increase Ot increase Ot increase Ot increase Ot increase Ot increase ↑ increase Ot increase Ot increase Ot increase decrease O decrease O decrease Odecrease decrease Odecrease Odecrease Odecrease Odecrease Odecrease decrease Odecrease O(no change) O(no change) O(no change) O(no change) (no change) O(no change) O (no change) (no change) O (no change) O(no change) O(no change) (no change)
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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Transcribed Image Text:A chem ngineer is studying the following reaction:
4 HCl(g) + O₂(g) → 2H₂O(g) + 2Cl₂(g)
At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.17.
P
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
C
compound
HCl
02
H₂O
C1₂
H CI
H₂O
C1₂
H Cl
0₂
H₂O
C12
pressure
6.10 atm
5.69 atm
9.07 atm
4.08 atm
6.65 atm
5.36 atm
7.21 atm
2.91 atm
4.19 atm
4.74 atm
8.43 atm
4.13 atm
expected change in pressure
↑ increase
↑ increase
↑ increase
↑ increase
↑ increase
↑ increase
↑ increase
↑ increase
↑ increase
↑ increase
↑ increase
↑ increase
↓ decrease
decrease
decrease
decrease
↓ decrease
↓ decrease
↓ decrease
↓ decrease
↓ decrease
↓ decrease
↓ decrease
↓ decrease
(no change)
(no change)
(no change)
(no change)
(no change)
(no change)
(no change)
(no change)
(no change)
(no change)
(no change)
(no change)
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 reaction mixture is at equilibrium.
2. When 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 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.
Given that:
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