Methanol (CH3OH) can be synthesized by the reaction: CO (g) + 2 H2 (g) → CH;OH (g) What volume (in L) of H2 at a temperature of 355 K and a pressure of 738 mm Hg is needed to produce 35.7 g of CH;OH?
Methanol (CH3OH) can be synthesized by the reaction: CO (g) + 2 H2 (g) → CH;OH (g) What volume (in L) of H2 at a temperature of 355 K and a pressure of 738 mm Hg is needed to produce 35.7 g of CH;OH?
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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![**Exercise #105**
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**Methanol (CH₃OH) can be synthesized by the reaction:**
\[ \text{CO (g) + 2 H}_2 \text{(g)} \rightarrow \text{CH}_3\text{OH (g)} \]
What volume (in liters) of H₂ at a temperature of 355 K and a pressure of 738 mm Hg is needed to produce 35.7 grams of CH₃OH?
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**Explanation:**
This exercise involves the stoichiometric calculation in a chemical reaction, coupled with the application of the Ideal Gas Law to find the required volume of hydrogen gas (H₂) needed for the reaction at specified temperature and pressure conditions.
To solve this problem:
1. **Convert grams of methanol to moles**:
- Use the molar mass of CH₃OH to find the number of moles.
2. **Use stoichiometry of the reaction**:
- Determine the number of moles of H₂ required using the mole ratio from the balanced chemical equation.
3. **Apply the Ideal Gas Law (PV = nRT)**:
- Calculate the volume of H₂ gas using the given temperature, pressure, and the number of moles of H₂ found in step 2.
There are no graphs or diagrams in this particular exercise. The focus is purely on textual chemical information and calculations.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff5387081-05af-4c61-b379-73a2f6a67bdc%2F86a619ea-7ac0-430b-9ed1-6a638252f3cc%2Fwo1d9gc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Exercise #105**
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**Methanol (CH₃OH) can be synthesized by the reaction:**
\[ \text{CO (g) + 2 H}_2 \text{(g)} \rightarrow \text{CH}_3\text{OH (g)} \]
What volume (in liters) of H₂ at a temperature of 355 K and a pressure of 738 mm Hg is needed to produce 35.7 grams of CH₃OH?
---
**Explanation:**
This exercise involves the stoichiometric calculation in a chemical reaction, coupled with the application of the Ideal Gas Law to find the required volume of hydrogen gas (H₂) needed for the reaction at specified temperature and pressure conditions.
To solve this problem:
1. **Convert grams of methanol to moles**:
- Use the molar mass of CH₃OH to find the number of moles.
2. **Use stoichiometry of the reaction**:
- Determine the number of moles of H₂ required using the mole ratio from the balanced chemical equation.
3. **Apply the Ideal Gas Law (PV = nRT)**:
- Calculate the volume of H₂ gas using the given temperature, pressure, and the number of moles of H₂ found in step 2.
There are no graphs or diagrams in this particular exercise. The focus is purely on textual chemical information and calculations.
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