Calculate the mass in grams of 3.19 x 1024 molecules of propylamine. The chemical formula for propylamine is C,H,N. x1023 mass: 313.046 x10 Incorrect
Calculate the mass in grams of 3.19 x 1024 molecules of propylamine. The chemical formula for propylamine is C,H,N. x1023 mass: 313.046 x10 Incorrect
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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![**Problem Statement:**
Calculate the mass in grams of \(3.19 \times 10^{24}\) molecules of propylamine. The chemical formula for propylamine is \(C_3H_9N\).
**Student's Answer:**
- **Mass:** \( 313.046 \times 10^{23} \) g
- Status: Incorrect
**Explanation:**
This question asks the student to calculate the mass of a given number of molecules of propylamine, \(C_3H_9N\). The student provided an answer of \(313.046 \times 10^{23}\) grams, which is indicated to be incorrect.
**Steps to solve the problem correctly:**
1. **Determine the Molar Mass of Propylamine (\(C_3H_9N\)):**
- For Carbon (C): \(3 \times 12.01 = 36.03\)
- For Hydrogen (H): \(9 \times 1.008 = 9.072\)
- For Nitrogen (N): \(14.01\)
- Total molar mass = \(36.03 + 9.072 + 14.01 = 59.112 \, \text{g/mol}\)
2. **Use Avogadro's Number:**
- Avogadro's Number \(\approx 6.022 \times 10^{23} \, \text{molecules/mol}\)
3. **Convert the given number of molecules to moles:**
\[
3.19 \times 10^{24} \, \text{molecules} \times \frac{1 \, \text{mol}}{6.022 \times 10^{23} \, \text{molecules}} \approx 5.299 \, \text{moles}
\]
4. **Calculate the mass of the moles:**
\[
\text{Mass} = 5.299 \, \text{moles} \times 59.112 \, \text{g/mol} \approx 312.95 \, \text{g}
\]
Thus, the correct answer should be approximately 312.95 grams.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2b52cd77-b3d2-4b5d-8903-b23362bef087%2F50568897-36e6-47d5-8531-9a9b64731d00%2F58zv6gh_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
Calculate the mass in grams of \(3.19 \times 10^{24}\) molecules of propylamine. The chemical formula for propylamine is \(C_3H_9N\).
**Student's Answer:**
- **Mass:** \( 313.046 \times 10^{23} \) g
- Status: Incorrect
**Explanation:**
This question asks the student to calculate the mass of a given number of molecules of propylamine, \(C_3H_9N\). The student provided an answer of \(313.046 \times 10^{23}\) grams, which is indicated to be incorrect.
**Steps to solve the problem correctly:**
1. **Determine the Molar Mass of Propylamine (\(C_3H_9N\)):**
- For Carbon (C): \(3 \times 12.01 = 36.03\)
- For Hydrogen (H): \(9 \times 1.008 = 9.072\)
- For Nitrogen (N): \(14.01\)
- Total molar mass = \(36.03 + 9.072 + 14.01 = 59.112 \, \text{g/mol}\)
2. **Use Avogadro's Number:**
- Avogadro's Number \(\approx 6.022 \times 10^{23} \, \text{molecules/mol}\)
3. **Convert the given number of molecules to moles:**
\[
3.19 \times 10^{24} \, \text{molecules} \times \frac{1 \, \text{mol}}{6.022 \times 10^{23} \, \text{molecules}} \approx 5.299 \, \text{moles}
\]
4. **Calculate the mass of the moles:**
\[
\text{Mass} = 5.299 \, \text{moles} \times 59.112 \, \text{g/mol} \approx 312.95 \, \text{g}
\]
Thus, the correct answer should be approximately 312.95 grams.
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