What does Charles's law state about the relationship between volume and temperature of a gas at constant pressure?

Charles's law states that the volume of a gas is directly proportional to its absolute temperature (measured in Kelvin) when the pressure remains constant. This means that as the temperature of a gas increases, its volume also increases, provided that the gas is not experiencing any changes in pressure.

The relationship can be expressed mathematically as ( V \propto T ), highlighting that if you double the temperature (in Kelvin), the volume will also double, assuming pressure is constant. This direct proportionality is critical in understanding how gases behave under varying temperature conditions, which is essential in both chemistry and physics applications.

The other options misrepresent this relationship. The inverse proportionality suggested in the first option does not reflect how gases behave according to Charles's law. The second option mentions Fahrenheit, which is not relevant because Charles's law relies on absolute temperatures in Kelvin to maintain a direct proportionality. Lastly, the idea that volume is independent of temperature contradicts the fundamental principles of gas behavior; indeed, the volume varies with temperature changes at a constant pressure. Hence, the correct understanding lies in recognizing that volume and temperature are directly proportional when using the Kelvin scale.