Under standard temperature and pressure (STP), what volume does one mole of an ideal gas occupy?

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

Answer: (C)

Verified step by step guidance

1. Recall the definition of standard temperature and pressure (STP), which is 0°C (273 K) and 1 atm pressure.
2. Understand that under STP conditions, one mole of an ideal gas occupies a specific volume known as the molar volume.
3. Use the ideal gas law formula: \(P \times V = n \times R \times T\), where \(P\) is pressure, \(V\) is volume, \(n\) is number of moles, \(R\) is the ideal gas constant, and \(T\) is temperature in Kelvin.
4. Substitute the known values for STP: \(P = 1\) atm, \(n = 1\) mole, \(R = 0.0821\) L·atm/(mol·K), and \(T = 273\) K into the ideal gas law to solve for \(V\).
5. Calculate \(V\) by rearranging the ideal gas law to \(V = \frac{n \times R \times T}{P}\) and plugging in the values to find the volume occupied by one mole of an ideal gas at STP.