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How many individual formaldehyde (CH20 = 30.03 g/mol) are found in a 32.0 mL sample %3D of gaseous formaldehyde? The density of formaldehyde is 0.815 g/mL. 5.23 x 1023 molecules O 7.87 x 1023 molecules 4.72 x 1026 molecules 6.42 x 1023 molecules 8.92 x 1023 molecules

How many individual formaldehyde (CH20 = 30.03 g/mol) are found in a 32.0 mL sample %3D of gaseous formaldehyde? The density of formaldehyde is 0.815 g/mL. 5.23 x 1023 molecules O 7.87 x 1023 molecules 4.72 x 1026 molecules 6.42 x 1023 molecules 8.92 x 1023 molecules

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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### Calculating the Number of Formaldehyde Molecules in a Given Sample **Problem Statement:** How many individual formaldehyde (CH₂O = 30.03 g/mol) molecules are found in a 32.0 mL sample of gaseous formaldehyde? The density of formaldehyde is 0.815 g/mL. **Options:** - 5.23 x 10²³ molecules - 7.87 x 10²³ molecules - 4.72 x 10²⁶ molecules - 6.42 x 10²³ molecules - 8.92 x 10²³ molecules **Explanation:** 1. **Determine the mass of the sample:** - Volume = 32.0 mL - Density = 0.815 g/mL - Mass = Density × Volume = 0.815 g/mL × 32.0 mL = 26.08 g 2. **Calculate the number of moles of formaldehyde:** - Molar mass of CH₂O = 30.03 g/mol - Moles (n) = Mass / Molar mass = 26.08 g / 30.03 g/mol ≈ 0.868 moles 3. **Determine the number of molecules:** - Number of molecules = (Moles) × Avogadro's number (6.022 × 10²³ molecules/mol) - Number of molecules = 0.868 moles × 6.022 × 10²³ molecules/mol ≈ 5.23 × 10²³ molecules **Answer:** - The correct option is **5.23 x 10²³ molecules**. This problem involves critical understanding of the relationships between volume, density, molar mass, and Avogadro’s number to convert from a volume of liquid to the number of molecules in that volume. It emphasizes the importance of unit conversion and proper application of formulas in chemistry.
Transcribed Image Text:### Calculating the Number of Formaldehyde Molecules in a Given Sample **Problem Statement:** How many individual formaldehyde (CH₂O = 30.03 g/mol) molecules are found in a 32.0 mL sample of gaseous formaldehyde? The density of formaldehyde is 0.815 g/mL. **Options:** - 5.23 x 10²³ molecules - 7.87 x 10²³ molecules - 4.72 x 10²⁶ molecules - 6.42 x 10²³ molecules - 8.92 x 10²³ molecules **Explanation:** 1. **Determine the mass of the sample:** - Volume = 32.0 mL - Density = 0.815 g/mL - Mass = Density × Volume = 0.815 g/mL × 32.0 mL = 26.08 g 2. **Calculate the number of moles of formaldehyde:** - Molar mass of CH₂O = 30.03 g/mol - Moles (n) = Mass / Molar mass = 26.08 g / 30.03 g/mol ≈ 0.868 moles 3. **Determine the number of molecules:** - Number of molecules = (Moles) × Avogadro's number (6.022 × 10²³ molecules/mol) - Number of molecules = 0.868 moles × 6.022 × 10²³ molecules/mol ≈ 5.23 × 10²³ molecules **Answer:** - The correct option is **5.23 x 10²³ molecules**. This problem involves critical understanding of the relationships between volume, density, molar mass, and Avogadro’s number to convert from a volume of liquid to the number of molecules in that volume. It emphasizes the importance of unit conversion and proper application of formulas in chemistry.
### Decomposition of Mercury(II) Oxide (HgO) Solid mercury(II) oxide decomposes when heated, forming liquid mercury and oxygen gas as the only products. #### Question: What mass of mercury(II) oxide must be decomposed in order to collect 0.386 L of oxygen gas under STP conditions? #### Multiple Choice Options: - **A. 14.8 g** - **B. 167 g** - **C. 7.46 g** - **D. 41.8 g** - **E. 80.5 g** In this problem, you should use the information related to the chemical equation for the decomposition of mercury(II) oxide and the properties of gases at Standard Temperature and Pressure (STP) to find the solution.
Transcribed Image Text:### Decomposition of Mercury(II) Oxide (HgO) Solid mercury(II) oxide decomposes when heated, forming liquid mercury and oxygen gas as the only products. #### Question: What mass of mercury(II) oxide must be decomposed in order to collect 0.386 L of oxygen gas under STP conditions? #### Multiple Choice Options: - **A. 14.8 g** - **B. 167 g** - **C. 7.46 g** - **D. 41.8 g** - **E. 80.5 g** In this problem, you should use the information related to the chemical equation for the decomposition of mercury(II) oxide and the properties of gases at Standard Temperature and Pressure (STP) to find the solution.
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