A given quantity of a gas occupies a volume of 228 cm3 at a pressure of 750mm Hg. What will be its volume at atmospheric pressure?

We can use the combined gas law to solve this problem, which states that the product of pressure and volume is directly proportional to the product of the number of moles of gas and the absolute temperature. Since the number of moles of gas and the temperature are constant, we can use the following equation: P1V1 = P2V2 where P1 is the initial pressure, V1 is the initial volume, P2 is the final pressure (atmospheric pressure), and V2 is the final volume (what we want to find). Substituting the values given in the problem, we get: (750 mm Hg)(228 cm^3) = (760 mm Hg)(V2) Solving for V2, we get: V2 = (750 mm Hg)(228 cm^3) / (760 mm Hg) V2 = 225 cm^3 Therefore, the volume of the gas at atmospheric pressure would be 225 cm^3. The answer is option (B).