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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Question
![**Problem Statement:**
How many grams of He are there in a sample of He that contains \(5.06 \times 10^{23}\) atoms?
**Solution:**
To determine the mass in grams of a helium sample containing \(5.06 \times 10^{23}\) atoms, you need to use the concept of moles and Avogadro's number.
**Explanation:**
1. **Molar Mass of Helium (He):**
- The molar mass of helium is approximately 4 grams/mole.
2. **Avogadro's Number:**
- Avogadro's number is \(6.022 \times 10^{23}\) atoms/mole.
3. **Calculate Moles of Helium:**
- First, find the number of moles of helium from the given atoms:
\[
\text{Moles of He} = \frac{5.06 \times 10^{23} \text{ atoms}}{6.022 \times 10^{23} \text{ atoms/mole}}
\]
4. **Calculate the Mass of Helium:**
- Multiply the number of moles by the molar mass of helium:
\[
\text{Mass in grams} = \text{Moles of He} \times 4 \text{ grams/mole}
\]
5. **Result:**
- Input the calculated mass in grams in the provided box.
This process allows you to convert the number of helium atoms into a mass measurement.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdfb4f807-44a0-4e53-a1ec-1c8181073ac9%2Fe25f311a-fbfa-4e7d-943f-d4409bf40283%2Fdaq3r6fy_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
How many grams of He are there in a sample of He that contains \(5.06 \times 10^{23}\) atoms?
**Solution:**
To determine the mass in grams of a helium sample containing \(5.06 \times 10^{23}\) atoms, you need to use the concept of moles and Avogadro's number.
**Explanation:**
1. **Molar Mass of Helium (He):**
- The molar mass of helium is approximately 4 grams/mole.
2. **Avogadro's Number:**
- Avogadro's number is \(6.022 \times 10^{23}\) atoms/mole.
3. **Calculate Moles of Helium:**
- First, find the number of moles of helium from the given atoms:
\[
\text{Moles of He} = \frac{5.06 \times 10^{23} \text{ atoms}}{6.022 \times 10^{23} \text{ atoms/mole}}
\]
4. **Calculate the Mass of Helium:**
- Multiply the number of moles by the molar mass of helium:
\[
\text{Mass in grams} = \text{Moles of He} \times 4 \text{ grams/mole}
\]
5. **Result:**
- Input the calculated mass in grams in the provided box.
This process allows you to convert the number of helium atoms into a mass measurement.
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