At standard temperature and pressure (0.00°C and 1.00 atm), what is the volume occupied by 1 mol of an ideal gas?

• A. 22.4 L
• B. 0.0821 L
• C. 273 L
• D. 1.00 L

Answer: (A)

Verified step by step guidance

1. Identify the conditions given: standard temperature and pressure (STP), which means temperature T = 0.00°C and pressure P = 1.00 atm.
2. Recall the ideal gas law equation: \(P \times V = n \times R \times T\), where \(P\) is pressure, \(V\) is volume, \(n\) is number of moles, \(R\) is the ideal gas constant, and \(T\) is temperature in Kelvin.
3. Convert the temperature from Celsius to Kelvin using the formula: \(T(K) = T(°C) + 273.15\).
4. Use the ideal gas constant \(R = 0.0821 \frac{L \cdot atm}{mol \cdot K}\), which is appropriate for the units given.
5. Rearrange the ideal gas law to solve for volume: \(V = \frac{n \times R \times T}{P}\), then substitute \(n = 1\) mol, the converted temperature, \(P = 1.00\) atm, and \(R\) to find the volume occupied by 1 mole of an ideal gas at STP.