QuestionJuly 24, 2025

Suppose you want to calculate the volume of 32.9 g of nitrogen gas at 298 .15 K and 1 atm. What information do you need to calculate the volume of nitrogen? mass of nitrogen gas molar mass of nitrogen gas gas constant pressure of nitrogen gas

Suppose you want to calculate the volume of 32.9 g of nitrogen gas at 298 .15 K and 1 atm. What information do you need to calculate the volume of nitrogen? mass of nitrogen gas molar mass of nitrogen gas gas constant pressure of nitrogen gas
Suppose you want to calculate the volume of 32.9 g of nitrogen gas at 298 .15 K and 1 atm. What
information do you need to calculate the volume of nitrogen?
mass of nitrogen gas
molar mass of nitrogen gas
gas constant
pressure of nitrogen gas

Solution
4.2(199 votes)

Answer

The volume of nitrogen gas is approximately 27.6 L. Explanation 1. Identify Required Information To calculate the volume of nitrogen gas, you need the mass of nitrogen gas, molar mass of nitrogen gas, gas constant, temperature, and pressure. 2. Calculate Moles of Nitrogen Gas Use the formula n = \frac{\text{mass}}{\text{molar mass}}. For nitrogen (N_2), the molar mass is approximately 28.02 g/mol. So, n = \frac{32.9 \, \text{g}}{28.02 \, \text{g/mol}}. 3. Apply Ideal Gas Law Use **PV = nRT** to find the volume. Rearrange to V = \frac{nRT}{P}. Given R = 0.0821 \, \text{L atm/mol K}, T = 298.15 \, \text{K}, and P = 1 \, \text{atm}.

Explanation

1. Identify Required Information<br /> To calculate the volume of nitrogen gas, you need the mass of nitrogen gas, molar mass of nitrogen gas, gas constant, temperature, and pressure.<br /><br />2. Calculate Moles of Nitrogen Gas<br /> Use the formula $n = \frac{\text{mass}}{\text{molar mass}}$. For nitrogen ($N_2$), the molar mass is approximately 28.02 g/mol. So, $n = \frac{32.9 \, \text{g}}{28.02 \, \text{g/mol}}$.<br /><br />3. Apply Ideal Gas Law<br /> Use **PV = nRT** to find the volume. Rearrange to $V = \frac{nRT}{P}$. Given $R = 0.0821 \, \text{L atm/mol K}$, $T = 298.15 \, \text{K}$, and $P = 1 \, \text{atm}$.
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