Chemistry · States of Matter - Gases, Liquids and Solids

Option B is correct. When the pressure of an ideal gas is reduced to half at a constant temperature, the volume of the gas will double. This relationship is described by Boyle's Law, which states that for a given mass of an ideal gas at constant temperature, the product of pressure (P) and volume (V) is constant (PV = constant). Hence, if the pressure is halved, to maintain the constant product, the volume must double. Therefore, if the initial volume is x, the new volume will be 2x.

Option A is incorrect because it suggests the volume reduces to half, which is not in accordance with the principle of gas behavior. Option C is incorrect as it implies that the volume quadruples, which is not true under these conditions. Option D is also incorrect as it indicates a significant reduction in volume, which contradicts the expected increase in volume when pressure decreases.

This option suggests that the volume reduces to half when the pressure is halved, which is incorrect according to Boyle's Law. When pressure decreases, volume increases.

This is correct. According to Boyle's Law, if the pressure of an ideal gas is halved while keeping the temperature constant, the volume will double, resulting in a volume of 2x.

This option incorrectly suggests that the volume quadruples when the pressure is halved. According to Boyle's Law, volume is directly proportional to the inverse of pressure, resulting in a doubling, not quadrupling, of volume.

This option indicates a drastic reduction in volume, which contradicts the principle that volume increases as pressure decreases. Therefore, it is incorrect.