Methanol can be formed by the following UNBALANCED equation below. What is the mass in grams of methanol that can be formed from 183 molecules of CO? H₂(g) + CO(g) → CH3OH(I). 4
Methanol can be formed by the following UNBALANCED equation below. What is the mass in grams of methanol that can be formed from 183 molecules of CO? H₂(g) + CO(g) → CH3OH(I). 4
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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![**Methanol Formation and Calculation**
Methanol can be formed by the following **unbalanced** chemical equation:
\[ \text{H}_2(g) + \text{CO}(g) \rightarrow \text{CH}_3\text{OH}(l) \]
**Problem Statement**
What is the mass in grams of methanol that can be formed from 183 molecules of CO?
**Explanation**
To solve this problem, we follow these steps:
1. **Balance the Equation:** First, ensure the equation is balanced to determine the correct stoichiometry.
\[ 2\text{H}_2(g) + \text{CO}(g) \rightarrow \text{CH}_3\text{OH}(l) \]
2. **Calculate Molecules of Methanol:**
- 1 molecule of CO combines with H₂ to produce 1 molecule of CH₃OH according to the balanced equation.
- Therefore, 183 molecules of CO will produce 183 molecules of CH₃OH.
3. **Convert to Moles:**
- Use Avogadro’s number \( (6.022 \times 10^{23} \text{ molecules/mol}) \) to convert molecules to moles.
- Mole of methanol \( = \frac{183}{6.022 \times 10^{23}} \).
4. **Calculate Mass:**
- Determine the molar mass of methanol (CH₃OH):
- Carbon (C) = 12.01 g/mol
- Hydrogen (H) = 1.01 g/mol (×4)
- Oxygen (O) = 16.00 g/mol
- Total = 12.01 + 4.04 + 16.00 = 32.05 g/mol
- Multiply moles of methanol by its molar mass to find the mass in grams.
The answer will provide the mass of methanol formed from 183 molecules of CO.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F75c7225b-0db1-4c1a-927e-b9120981a291%2F3f4470d2-a9e4-42ec-a2f3-f0cb7e1f89f1%2Fyeqfquo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Methanol Formation and Calculation**
Methanol can be formed by the following **unbalanced** chemical equation:
\[ \text{H}_2(g) + \text{CO}(g) \rightarrow \text{CH}_3\text{OH}(l) \]
**Problem Statement**
What is the mass in grams of methanol that can be formed from 183 molecules of CO?
**Explanation**
To solve this problem, we follow these steps:
1. **Balance the Equation:** First, ensure the equation is balanced to determine the correct stoichiometry.
\[ 2\text{H}_2(g) + \text{CO}(g) \rightarrow \text{CH}_3\text{OH}(l) \]
2. **Calculate Molecules of Methanol:**
- 1 molecule of CO combines with H₂ to produce 1 molecule of CH₃OH according to the balanced equation.
- Therefore, 183 molecules of CO will produce 183 molecules of CH₃OH.
3. **Convert to Moles:**
- Use Avogadro’s number \( (6.022 \times 10^{23} \text{ molecules/mol}) \) to convert molecules to moles.
- Mole of methanol \( = \frac{183}{6.022 \times 10^{23}} \).
4. **Calculate Mass:**
- Determine the molar mass of methanol (CH₃OH):
- Carbon (C) = 12.01 g/mol
- Hydrogen (H) = 1.01 g/mol (×4)
- Oxygen (O) = 16.00 g/mol
- Total = 12.01 + 4.04 + 16.00 = 32.05 g/mol
- Multiply moles of methanol by its molar mass to find the mass in grams.
The answer will provide the mass of methanol formed from 183 molecules of CO.
Expert Solution

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H2(g)+CO(g) ->CH3OH(l)
Molecules of CO=183 molecules
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