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
Step 1
Given -
H2(g)+CO(g) ->CH3OH(l)
Molecules of CO=183 molecules
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