What is the molar volume of any ideal gas at standard temperature and pressure (STP)?

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

Answer: (B)

Verified step by step guidance

1. Recall that the molar volume of an ideal gas is the volume occupied by one mole of the gas under specified conditions of temperature and pressure.
2. Identify the standard temperature and pressure (STP) conditions: temperature = 273 K (0°C) and pressure = 1 atm.
3. Use 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.
4. Set \(n = 1\) mole to find the molar volume \(V_m\), then rearrange the equation to solve for \(V\): \(V = \frac{n \times R \times T}{P}\).
5. Substitute the values for \(n = 1\) mole, \(R = 0.0821 \frac{L \cdot atm}{mol \cdot K}\), \(T = 273\) K, and \(P = 1\) atm into the equation to calculate the molar volume.