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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please help and kindly explain this to me
![**Question:**
Determine how many molecules of H₂CO are present in 33.0 mL of a 4.500 M solution of H₂CO in water.
**Solution:**
To solve this problem, we will use the following steps:
1. **Calculate the number of moles of H₂CO in the solution.**
- **Molarity (M)** is defined as moles of solute per liter of solution. Therefore, to find the number of moles, we use the formula:
\[
\text{Moles of H}_2\text{CO} = \text{Molarity} \times \text{Volume (L)}
\]
- Given the molarity is 4.500 M and the volume is 33.0 mL, convert the volume to liters:
\[
33.0 \, \text{mL} \times \frac{1 \, \text{L}}{1000 \, \text{mL}} = 0.0330 \, \text{L}
\]
- Calculate the moles:
\[
\text{Moles of H}_2\text{CO} = 4.500 \, \text{mol/L} \times 0.0330 \, \text{L} = 0.1485 \, \text{mol}
\]
2. **Calculate the number of molecules of H₂CO.**
- Use Avogadro's number: \(6.022 \times 10^{23}\) molecules/mol.
- Multiply the moles of H₂CO by Avogadro's number to find the number of molecules:
\[
0.1485 \, \text{mol} \times 6.022 \times 10^{23} \, \text{molecules/mol} = 8.945 \times 10^{22} \, \text{molecules}
\]
**Conclusion:**
There are approximately \(8.945 \times 10^{22}\) molecules of H₂CO in 33.0 mL of the solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe8d6915e-d90b-434d-a514-7e312490ff06%2Ffd776475-aa95-4106-9826-9b41d2825ffc%2Fn2eeuwq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question:**
Determine how many molecules of H₂CO are present in 33.0 mL of a 4.500 M solution of H₂CO in water.
**Solution:**
To solve this problem, we will use the following steps:
1. **Calculate the number of moles of H₂CO in the solution.**
- **Molarity (M)** is defined as moles of solute per liter of solution. Therefore, to find the number of moles, we use the formula:
\[
\text{Moles of H}_2\text{CO} = \text{Molarity} \times \text{Volume (L)}
\]
- Given the molarity is 4.500 M and the volume is 33.0 mL, convert the volume to liters:
\[
33.0 \, \text{mL} \times \frac{1 \, \text{L}}{1000 \, \text{mL}} = 0.0330 \, \text{L}
\]
- Calculate the moles:
\[
\text{Moles of H}_2\text{CO} = 4.500 \, \text{mol/L} \times 0.0330 \, \text{L} = 0.1485 \, \text{mol}
\]
2. **Calculate the number of molecules of H₂CO.**
- Use Avogadro's number: \(6.022 \times 10^{23}\) molecules/mol.
- Multiply the moles of H₂CO by Avogadro's number to find the number of molecules:
\[
0.1485 \, \text{mol} \times 6.022 \times 10^{23} \, \text{molecules/mol} = 8.945 \times 10^{22} \, \text{molecules}
\]
**Conclusion:**
There are approximately \(8.945 \times 10^{22}\) molecules of H₂CO in 33.0 mL of the solution.
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