QuestionMay 12, 2025

__ 35. The mass of a 1.0 L sample of a gas is 0.716 g at STP. What is the molar mass of the gas? __ 36. What is the density at STP of NO_(2) gas (molar mass=46.01g/mol) in grams per liter?

__ 35. The mass of a 1.0 L sample of a gas is 0.716 g at STP. What is the molar mass of the gas? __ 36. What is the density at STP of NO_(2) gas (molar mass=46.01g/mol) in grams per liter?
__ 35. The mass of a 1.0 L sample of a gas is 0.716 g at
STP. What is the molar mass of the gas?
__ 36. What is the density at STP of NO_(2) gas (molar
mass=46.01g/mol) in grams per liter?

Solution
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Answer

35. Molar Mass = 16.03 g/mol ### 36. Density = 2.05 g/L Explanation 1. Calculate molar mass of the gas At STP, 1 mole of any gas occupies 22.4 L. Use the formula for molar mass: **Molar Mass = \frac{\text{mass}}{\text{volume at STP}} \times 22.4**. For the given sample, Molar Mass = \frac{0.716 \, \text{g}}{1.0 \, \text{L}} \times 22.4. 2. Calculate density of NO_2 gas Density is calculated using the formula: **Density = \frac{\text{molar mass}}{\text{volume at STP}}**. For NO_2, Density = \frac{46.01 \, \text{g/mol}}{22.4 \, \text{L/mol}}.

Explanation

1. Calculate molar mass of the gas<br /> At STP, 1 mole of any gas occupies 22.4 L. Use the formula for molar mass: **Molar Mass = \frac{\text{mass}}{\text{volume at STP}} \times 22.4**. For the given sample, Molar Mass = \frac{0.716 \, \text{g}}{1.0 \, \text{L}} \times 22.4.<br /><br />2. Calculate density of $NO_2$ gas<br /> Density is calculated using the formula: **Density = \frac{\text{molar mass}}{\text{volume at STP}}**. For $NO_2$, Density = \frac{46.01 \, \text{g/mol}}{22.4 \, \text{L/mol}}.
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