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
![**Question:**
What is the mass in grams of \(5.00 \times 10^{12}\) H\(_2\)O molecules?
**Explanation:**
This question is asking for the mass, in grams, of a specific number of water (H\(_2\)O) molecules.
*Note for students:*
To solve this, you will need to use the concept of the molar mass of water and Avogadro's number.
1. **Molar Mass of Water (H\(_2\)O):**
- Hydrogen (H) has a molar mass of approximately 1 g/mol.
- Oxygen (O) has a molar mass of approximately 16 g/mol.
- Therefore, the molar mass of H\(_2\)O is \(2 \times 1 + 16 = 18\) g/mol.
2. **Avogadro's Number:**
- Avogadro's number is \(6.022 \times 10^{23}\) molecules per mole.
- This number represents the quantity of molecules in one mole of any substance.
3. **Steps to Calculate the Mass:**
- First, calculate the number of moles of water molecules:
\[
\text{Number of moles} = \frac{\text{Number of molecules}}{\text{Avogadro's number}} = \frac{5.00 \times 10^{12}}{6.022 \times 10^{23}}
\]
- Then, find the mass:
\[
\text{Mass in grams} = \text{Number of moles} \times \text{Molar mass of H\(_2\)O}
\]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F19c732c8-efee-414f-84d3-ed7ea6f7d2e9%2F62da08c6-2a69-44c1-86f0-d72f7c0d91ba%2Fuqmbf4_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question:**
What is the mass in grams of \(5.00 \times 10^{12}\) H\(_2\)O molecules?
**Explanation:**
This question is asking for the mass, in grams, of a specific number of water (H\(_2\)O) molecules.
*Note for students:*
To solve this, you will need to use the concept of the molar mass of water and Avogadro's number.
1. **Molar Mass of Water (H\(_2\)O):**
- Hydrogen (H) has a molar mass of approximately 1 g/mol.
- Oxygen (O) has a molar mass of approximately 16 g/mol.
- Therefore, the molar mass of H\(_2\)O is \(2 \times 1 + 16 = 18\) g/mol.
2. **Avogadro's Number:**
- Avogadro's number is \(6.022 \times 10^{23}\) molecules per mole.
- This number represents the quantity of molecules in one mole of any substance.
3. **Steps to Calculate the Mass:**
- First, calculate the number of moles of water molecules:
\[
\text{Number of moles} = \frac{\text{Number of molecules}}{\text{Avogadro's number}} = \frac{5.00 \times 10^{12}}{6.022 \times 10^{23}}
\]
- Then, find the mass:
\[
\text{Mass in grams} = \text{Number of moles} \times \text{Molar mass of H\(_2\)O}
\]
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