A chemical engineer is studying the following reaction: CH₂(g)+2H₂S(g) → CS₂(g) + 4H₂(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.49. The engineer charges ("fills") four reaction vessels with methane and hydrogen sulfide, 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 compound pressure expected change in pressure CH 8.16 atm ↑ increase O decrease O (no change) 2.21 atm Of increase O (no change) O↓ decrease O↓ decrease 2.41 atm Ot increase O (no change) 4.10 atm O↑ increase O decrease O (no change) 8.94 atm O↑ increase O decrease O (no change) 3.77 atm Ot increase O decrease O (no change) 1.63 atm Of increase O (no change) O decrease O decrease 0.97 atm O↑ increase O (no change) 8.34 atm Ot increase decrease O (no change) O (no change) 2.57 atm O O decrease O decrease Ot increase Of increase 2.23 atm O (no change) O (no change) 3.37 atm O decrease Ot increase B C H₂S CS₂ H₂ CHA H₂S CS₂ H₂₂ CHA H₂S CS₂ H₂
A chemical engineer is studying the following reaction: CH₂(g)+2H₂S(g) → CS₂(g) + 4H₂(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.49. The engineer charges ("fills") four reaction vessels with methane and hydrogen sulfide, 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 compound pressure expected change in pressure CH 8.16 atm ↑ increase O decrease O (no change) 2.21 atm Of increase O (no change) O↓ decrease O↓ decrease 2.41 atm Ot increase O (no change) 4.10 atm O↑ increase O decrease O (no change) 8.94 atm O↑ increase O decrease O (no change) 3.77 atm Ot increase O decrease O (no change) 1.63 atm Of increase O (no change) O decrease O decrease 0.97 atm O↑ increase O (no change) 8.34 atm Ot increase decrease O (no change) O (no change) 2.57 atm O O decrease O decrease Ot increase Of increase 2.23 atm O (no change) O (no change) 3.37 atm O decrease Ot increase B C H₂S CS₂ H₂ CHA H₂S CS₂ H₂₂ CHA H₂S CS₂ H₂
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![### Experiment Study on Reaction Equilibrium
A chemical engineer is studying the following reaction:
\[ \text{CH}_4(g) + 2\text{H}_2\text{S}(g) \rightarrow \text{CS}_2(g) + 4\text{H}_2(g) \]
At the selected temperature, the engineer determines that the equilibrium constant \( K_p \) for this reaction is 0.49.
The engineer fills four reaction vessels with methane (\(\text{CH}_4\)) and hydrogen sulfide (\(\text{H}_2\text{S}\)) and initiates the reaction. Over time, they measure the composition of the mixture inside each vessel. The first set of measurements is presented in the table below. The engineer is tasked with predicting the changes in the composition of the mixture for subsequent measurements.
### Table of Measurements and Predictions
| Reaction Vessel | Compound | Pressure (atm) | Expected Change in Pressure | |
|-----------------|----------|----------------|-----------------------------| |
| **A** | \(\text{CH}_4\) | 8.16 | \( \bigcirc \) Increase | |
| **A** | \(\text{H}_2\text{S}\) | 2.21 | \( \bigcirc \) Increase | |
| **A** | \(\text{CS}_2\) | 2.41 | \( \bigcirc \) Increase | |
| **A** | \(\text{H}_2\) | 4.10 | \( \bigcirc \) Increase | |
| | | | | |
| **B** | \(\text{CH}_4\) | 8.94 | \( \bigcirc \) Decrease | |
| **B** | \(\text{H}_2\text{S}\) | 3.77 | \( \bigcirc \) Decrease | |
| **B** | \(\text{CS}_2\) | 1.63 | \( \bigcirc \) Decrease | |
| **B** | \(\text{H}_2\) |](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F20b515c9-5e3a-448e-90a2-ac3b562e1523%2Fe4665029-0baa-459a-ad65-4c075521123f%2Ft7kjemj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Experiment Study on Reaction Equilibrium
A chemical engineer is studying the following reaction:
\[ \text{CH}_4(g) + 2\text{H}_2\text{S}(g) \rightarrow \text{CS}_2(g) + 4\text{H}_2(g) \]
At the selected temperature, the engineer determines that the equilibrium constant \( K_p \) for this reaction is 0.49.
The engineer fills four reaction vessels with methane (\(\text{CH}_4\)) and hydrogen sulfide (\(\text{H}_2\text{S}\)) and initiates the reaction. Over time, they measure the composition of the mixture inside each vessel. The first set of measurements is presented in the table below. The engineer is tasked with predicting the changes in the composition of the mixture for subsequent measurements.
### Table of Measurements and Predictions
| Reaction Vessel | Compound | Pressure (atm) | Expected Change in Pressure | |
|-----------------|----------|----------------|-----------------------------| |
| **A** | \(\text{CH}_4\) | 8.16 | \( \bigcirc \) Increase | |
| **A** | \(\text{H}_2\text{S}\) | 2.21 | \( \bigcirc \) Increase | |
| **A** | \(\text{CS}_2\) | 2.41 | \( \bigcirc \) Increase | |
| **A** | \(\text{H}_2\) | 4.10 | \( \bigcirc \) Increase | |
| | | | | |
| **B** | \(\text{CH}_4\) | 8.94 | \( \bigcirc \) Decrease | |
| **B** | \(\text{H}_2\text{S}\) | 3.77 | \( \bigcirc \) Decrease | |
| **B** | \(\text{CS}_2\) | 1.63 | \( \bigcirc \) Decrease | |
| **B** | \(\text{H}_2\) |
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