A 1.50-liter sample of dry air in a cylinder exerts a pressure of 3.00 atmospheres at a temperature of 25^circ C Without change in temperature, a piston is moved in the cylinder until the pressure in the cylinder is reduced to 1.00 atmosphere. The volume of the gas is: V=((1.50)(1.00))/((3.00)(298))=0.0016TL V=((1.50)(1.00))/(3.00)=0.50L V=((1.50)(25)(3.00))/((1.00))=113L V=((1.50)(3.00))/((1.00))=4.50L

To find the new volume of the gas when the pressure is reduced to 1.00 atmosphere, we can use Boyle's Law. Boyle's Law states that for a given amount of gas at constant temperature, the pressure and volume are inversely proportional. Mathematically, it is expressed as: Where:- is the initial pressure (3.00 atm),- is the initial volume (1.50 L),- is the final pressure (1.00 atm),- is the final volume.We need to solve for : Substitute the known values into the equation: Therefore, the volume of the gas when the pressure is reduced to 1.00 atmosphere is 4.50 liters. The correct answer is: