A sealed container holds 2 moles of an ideal gas at a temperature of 300 K and a pressure of 1 atm. If the volume of the container is doubled while keeping the temperature constant, what will be the new pressure?

Core Concept

For an ideal gas at constant temperature, Boyle's law applies: P₁V₁ = P₂V₂. If the volume is doubled (V₂ = 2V₁), then P₂ = P₁V₁/V₂ = P₁V₁/(2V₁) = P₁/2. Since the initial pressure was 1 atm, the new pressure will be 0.5 atm.