What is the volume occupied by 1.0 mole of hydrogen gas at standard temperature and pressure (STP)?

• A. 1.0 L
• B. 0.0821 L
• C. 22.4 L
• D. 2.0 L

Answer: (C)

Verified step by step guidance

1. Recall that at standard temperature and pressure (STP), one mole of any ideal gas occupies a specific volume. STP is defined as a temperature of 0°C (273.15 K) and a pressure of 1 atm.
2. Use the molar volume of an ideal gas at STP, which is a known constant: 1 mole of an ideal gas occupies 22.4 liters under these conditions.
3. Since the problem asks for the volume occupied by 1.0 mole of hydrogen gas at STP, you can directly apply this molar volume value without further calculations.
4. If you wanted to derive this value, you could use the Ideal Gas Law: \(P \times V = n \times R \times T\), where \(P\) is pressure, \(V\) is volume, \(n\) is moles, \(R\) is the ideal gas constant, and \(T\) is temperature in Kelvin.
5. Rearranging the Ideal Gas Law to solve for volume gives: \(V = \frac{n \times R \times T}{P}\). Plugging in \(n=1.0\) mole, \(R=0.0821\) L·atm/(mol·K), \(T=273.15\) K, and \(P=1\) atm will yield the volume, which matches the molar volume of 22.4 L.