**Exercise #105**---**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.

To find volume of hydrogen gas.

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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Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

**Exercise #105**

---

**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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