Under which conditions will 1.00 mole of an ideal gas occupy 22.41 L?

• A. At 0°C and 2 atm pressure
• B. At 0°C and 1 atm pressure
• C. At 100°C and 1 atm pressure
• D. At 25°C and 1 atm pressure

Answer: (B)

Verified step by step guidance

1. 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.
2. Identify the standard molar volume of an ideal gas, which is the volume occupied by 1 mole of gas at standard temperature and pressure (STP). STP is defined as 0°C (273.15 K) and 1 atm pressure, and the molar volume is approximately 22.41 L under these conditions.
3. Convert the given temperatures to Kelvin by adding 273.15 to the Celsius temperature, since the Ideal Gas Law requires temperature in Kelvin.
4. Use the Ideal Gas Law to check if the volume of 22.41 L corresponds to 1 mole of gas at the given temperature and pressure conditions by substituting \(n=1\) mole, \(V=22.41\) L, and the respective \(P\) and \(T\) values into the equation.
5. Compare the calculated volumes or conditions to determine under which condition 1 mole of an ideal gas occupies exactly 22.41 L, confirming that it matches the standard condition of 0°C and 1 atm pressure.