A 2 L container will hold about 4 g of which of the following gases at 0°C and 1 atm?

• A. CO2
• B. O2
• C. N2
• D. He

Answer: (D)

Verified step by step guidance

1. Identify the problem: We need to determine which gas among CO\_2, O\_2, N\_2, and He will have a mass of about 4 g when contained in a 2 L container at 0°C and 1 atm.
2. Recall the Ideal Gas Law: \(P V = n R T\), where \(P\) is pressure, \(V\) is volume, \(n\) is moles, \(R\) is the ideal gas constant, and \(T\) is temperature in Kelvin.
3. Calculate the number of moles of gas in the container using the Ideal Gas Law. Convert temperature to Kelvin: \(T = 0 + 273.15 = 273.15\) K. Use \(P = 1\) atm, \(V = 2\) L, and \(R = 0.0821\) L·atm/(mol·K). Then, \(n = \frac{P V}{R T}\).
4. Determine the molar mass of each gas: CO\_2 (44 g/mol), O\_2 (32 g/mol), N\_2 (28 g/mol), He (4 g/mol).
5. Calculate the mass of each gas in the container by multiplying the number of moles \(n\) by the molar mass of each gas. The gas whose calculated mass is closest to 4 g is the correct answer.