Which of the following is NOT true about the volume of a gas under standard conditions?

• A. The volume of a gas is directly proportional to its temperature at constant pressure.
• B. The volume of a gas is independent of the pressure applied to it.
• C. The volume of a gas can be calculated using the ideal gas law equation PV = nRT.
• D. At STP, one mole of any ideal gas occupies 22.4 L.

Answer: (B)

Verified step by step guidance

1. Step 1: Understand the relationship between volume, temperature, and pressure for gases. According to Charles's Law, the volume of a gas is directly proportional to its temperature when pressure is held constant. This means if temperature increases, volume increases, and vice versa.
2. Step 2: Recall Boyle's Law, which states that the volume of a gas is inversely proportional to its pressure at constant temperature. This means that if pressure increases, volume decreases, and if pressure decreases, volume increases.
3. Step 3: Recognize that the ideal gas law, given by the equation \(P V = n R T\), relates pressure (P), volume (V), number of moles (n), the ideal gas constant (R), and temperature (T). This equation can be used to calculate the volume of a gas under various conditions.
4. Step 4: Know the standard molar volume of an ideal gas at STP (Standard Temperature and Pressure), which is 22.4 liters per mole. This is a key reference point in gas calculations.
5. Step 5: Analyze the statement 'The volume of a gas is independent of the pressure applied to it.' Since Boyle's Law shows volume depends on pressure, this statement is NOT true. Therefore, this is the correct choice for the statement that is false about gas volume under standard conditions.