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A sample of CH2F2 with a mass of 19 contains atoms of F. O 2.2 x 1023 O 9.5 9 3.3 x 1024 4.4 x 1023 O 38

A sample of CH2F2 with a mass of 19 contains atoms of F. O 2.2 x 1023 O 9.5 9 3.3 x 1024 4.4 x 1023 O 38

Chemistry
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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A sample of CH2F2 with a mass of 19g contains how many atoms of F?
**Question:** A sample of CH₂F₂ with a mass of 19 g contains _______ atoms of F. **Answer Choices:** - ○ \(2.2 \times 10^{23}\) - ○ 9.5 - ○ \(3.3 \times 10^{24}\) - ○ \(4.4 \times 10^{23}\) - ○ 38 **Explanation:** To solve this, we need to calculate the number of fluorine atoms in the given mass of CH₂F₂ (difluoromethane). 1. **Find Molar Mass of CH₂F₂:** - Carbon (C): \(12.01 \, \text{g/mol}\) - Hydrogen (H): \(1.01 \, \text{g/mol}\), for two H atoms: \(2 \times 1.01 = 2.02 \, \text{g/mol}\) - Fluorine (F): \(19.00 \, \text{g/mol}\), for two F atoms: \(2 \times 19.00 = 38.00 \, \text{g/mol}\) - Total molar mass: \(12.01 + 2.02 + 38.00 = 52.03 \, \text{g/mol}\) 2. **Calculate Moles of CH₂F₂:** - Moles \(= \frac{\text{mass}}{\text{molar mass}} = \frac{19}{52.03} \approx 0.365 \, \text{mol}\) 3. **Calculate Number of Fluorine Atoms:** - Each molecule of CH₂F₂ contains 2 fluorine atoms. - Moles of F from CH₂F₂ = \(0.365 \times 2 = 0.73 \, \text{mol of F atoms}\) - Number of fluorine atoms = \(0.73 \, \text{mol} \times 6.022 \times 10^{23} \, \text{atoms/mol} \approx 4.4 \times 10^{23} \, \text{atoms}\) Thus, the correct choice is \(4.4 \times 10^{23}\).
Transcribed Image Text:**Question:** A sample of CH₂F₂ with a mass of 19 g contains _______ atoms of F. **Answer Choices:** - ○ \(2.2 \times 10^{23}\) - ○ 9.5 - ○ \(3.3 \times 10^{24}\) - ○ \(4.4 \times 10^{23}\) - ○ 38 **Explanation:** To solve this, we need to calculate the number of fluorine atoms in the given mass of CH₂F₂ (difluoromethane). 1. **Find Molar Mass of CH₂F₂:** - Carbon (C): \(12.01 \, \text{g/mol}\) - Hydrogen (H): \(1.01 \, \text{g/mol}\), for two H atoms: \(2 \times 1.01 = 2.02 \, \text{g/mol}\) - Fluorine (F): \(19.00 \, \text{g/mol}\), for two F atoms: \(2 \times 19.00 = 38.00 \, \text{g/mol}\) - Total molar mass: \(12.01 + 2.02 + 38.00 = 52.03 \, \text{g/mol}\) 2. **Calculate Moles of CH₂F₂:** - Moles \(= \frac{\text{mass}}{\text{molar mass}} = \frac{19}{52.03} \approx 0.365 \, \text{mol}\) 3. **Calculate Number of Fluorine Atoms:** - Each molecule of CH₂F₂ contains 2 fluorine atoms. - Moles of F from CH₂F₂ = \(0.365 \times 2 = 0.73 \, \text{mol of F atoms}\) - Number of fluorine atoms = \(0.73 \, \text{mol} \times 6.022 \times 10^{23} \, \text{atoms/mol} \approx 4.4 \times 10^{23} \, \text{atoms}\) Thus, the correct choice is \(4.4 \times 10^{23}\).
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