Which general statement concerning ideal gases is true?

The statement regarding ideal gases that is true is that volume is inversely proportional to pressure. This relationship is captured in Boyle's Law, which states that for a given amount of gas at a constant temperature, the volume of the gas will decrease as the pressure increases, and vice versa. Mathematically, this can be expressed as ( P \cdot V = k ), where ( P ) is pressure, ( V ) is volume, and ( k ) is a constant. This fundamental principle underscores how changes in pressure and volume interact within an ideal gas.

The other statements do not hold true for ideal gases. Volume is not directly proportional to temperature; rather, it is directly proportional to temperature when pressure is held constant, as described by Charles's Law. Pressure is not independent of volume; any changes in one of these variables will lead to changes in the other, as illustrated by the inverse relationship established in Boyle's Law. Additionally, temperature is not independent of pressure; in a closed system where the amount of gas remains constant, changes in pressure can influence temperature and vice versa. The behavior of ideal gases follows specific relationships that link these variables closely together in predictable ways.