What happens to the pressure of a given mass of gas if its volume is halved while keeping the temperature constant, according to Boyle's law?

💡 Solution & Explanation

Boyle's law states that at constant temperature, the absolute pressure exerted by a given mass of an ideal gas is inversely proportional to the volume it occupies. Therefore, halving the volume causes the pressure to double proportionally. Incorrect choices suggest direct proportionality or no change, violating the isothermal pressure volume relationship. Real gases closely approximate this ideal behavior at moderate pressures and higher temperatures.