A chemical engineer is studying the following reaction: 2 H₂S(g)+30₂(g) → 2 SO₂(g)+2H₂O(g) - At the temperature the engineer picks, the equilibrium constant K for this reaction is 5.0. P The engineer charges ("fills") four reaction vessels with hydrogen sulfide and oxygen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B compound H₂S SO₂ H₂O H₂S SO₂ H₂O H₂S pressure 9.08 atm 1.44 atm atm 8.80 atm 8.96 atm 1.26 atm 10.19 atm 8.92 atm 10.40 atm expected change in pressure Ot increase O decrease Ot increase O decrease Ot increase O decrease O↑ increase Ot increase Ot increase Ot increase Ot increase O decrease O decrease ↓ decrease ↓ decrease O decrease Ot increase O decrease O (no change) O (no change) O (no change) O (no change) O (no change) (no change) O (no change) O (no change) O (no change)

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A chemical engineer is studying the following reaction:
2 H₂S(g)+30₂(g) → 2 SO₂(g) +2H₂O(g)
At the temperature the engineer picks, the equilibrium constant K for this reaction is 5.0.
The engineer charges ("fills") four reaction vessels with hydrogen sulfide and oxygen, and lets the reaction begin. He then
measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the
table below.
Predict the changes in the compositions the engineer should expect next time he measures the compositions.
reaction
vessel
A
B
compound
H₂S
0₂
SO2
H₂O
H₂S
0₂
SO₂
H₂O
H₂S
02
SO₂
H₂O
pressure
9.08 atm
1.44 atm
10.07 atm
8.80 atm
8.96 atm
1.26 atm
10.19 atm
8.92 atm
10.40 atm
3.42 atm
8.75 atm
7.48 atm
expected change in pressure
↑ increase O decrease
↑ increase
↑ increase
↑ increase
↑ increase
↑ increase
↑ increase
↑ increase
↑ increase
↑ increase
O decrease
↑ increase
decrease
O decrease
↑ increase O decrease
↓ decrease
O decrease
↓ decrease
O decrease
O 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)
Transcribed Image Text:A chemical engineer is studying the following reaction: 2 H₂S(g)+30₂(g) → 2 SO₂(g) +2H₂O(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 5.0. The engineer charges ("fills") four reaction vessels with hydrogen sulfide and oxygen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B compound H₂S 0₂ SO2 H₂O H₂S 0₂ SO₂ H₂O H₂S 02 SO₂ H₂O pressure 9.08 atm 1.44 atm 10.07 atm 8.80 atm 8.96 atm 1.26 atm 10.19 atm 8.92 atm 10.40 atm 3.42 atm 8.75 atm 7.48 atm expected change in pressure ↑ increase O decrease ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase O decrease ↑ increase decrease O decrease ↑ increase O decrease ↓ decrease O decrease ↓ decrease O decrease O 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

The direction in which the reaction proceeds to reach equilibrium can be predicted by determining the reaction quotient at given partial pressure of Reaction species.

Reaction quotient is the product of the concentrations of the products, each raised to the power equal to a stoichiometric coefficient divided by the product of the concentrations of the reactant each raised to the power equal to its stoichiometric coefficient at a particular point of time.

If Qp > Kp , then the reaction will shift to the left i.e. towards reactants.
If Qp < Kp, then the reaction will shift to the right i.e.  towards products.
If Qp = Kp, then the reaction is at equilibrium.

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