Which of the following is the correct pressure, in kPa, exerted by 1.00 mol of oxygen gas (O_2) in a 22.4 L container at 0°C? (Assume ideal gas behavior.)

• A. 273 kPa
• B. 0.0821 kPa
• C. 22.4 kPa
• D. 101.3 kPa

Answer: (D)

Verified step by step guidance

1. Identify the known variables from the problem: number of moles \(n = 1.00\) mol, volume \(V = 22.4\) L, temperature \(T = 0^\circ C = 273\) K, and the gas constant \(R = 0.0821\) L·atm/(mol·K) or \$8.314$ J/(mol·K) depending on units used.
2. Recall the Ideal Gas Law equation: \(P \times V = n \times R \times T\), where \(P\) is pressure, \(V\) is volume, \(n\) is moles, \(R\) is the ideal gas constant, and \(T\) is temperature in Kelvin.
3. Since the problem asks for pressure in kPa, use the gas constant \(R = 8.314\) L·kPa/(mol·K) to keep units consistent.
4. Rearrange the Ideal Gas Law to solve for pressure \(P\): \(P = \frac{n \times R \times T}{V}\).
5. Substitute the known values into the equation: \(P = \frac{1.00 \times 8.314 \times 273}{22.4}\), then calculate to find the pressure in kPa.