Multiple Choice
Using the Ideal Gas Law, calculate the density of CO2 gas in g/L at 27°C and 0.50 atm pressure.
7. Gases
The Ideal Gas Law: Density
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What is the density of nitrogen gas (N₂) at 67.3°C and 0.288 atm, assuming ideal gas behavior?
A
0.482 g/L
B
1.250 g/L
C
0.192 g/L
D
0.750 g/L
Verified step by step guidance1
Convert the temperature from Celsius to Kelvin by adding 273.15 to the given temperature: T(K) = 67.3 + 273.15.
Use the ideal gas law equation in the form \( PV = nRT \) to find the molar volume. Rearrange it to \( V = \frac{nRT}{P} \), where P is pressure, V is volume, n is moles, R is the ideal gas constant, and T is temperature in Kelvin.
Calculate the molar volume of nitrogen gas at the given conditions using the ideal gas constant \( R = 0.0821 \text{ L atm K}^{-1} \text{ mol}^{-1} \). Substitute the values for P, R, and T into the equation.
Determine the molar mass of nitrogen gas (N₂). Since nitrogen has an atomic mass of approximately 14.01 g/mol, the molar mass of N₂ is \( 2 \times 14.01 \text{ g/mol} \).
Calculate the density using the formula \( \text{Density} = \frac{\text{Molar Mass}}{\text{Molar Volume}} \). Substitute the molar mass of N₂ and the molar volume calculated in the previous steps to find the density in g/L.
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