A 125.0-mL contains a gas at 27°C and 760 mm Hg of pressure. The gas is pumped into an empty 1.50-L flask also at a temperature of 27°C. What is the pressure (in atm) of the gas in the new flask?

Question

Quizplus · Accepted Answer

Using the ideal gas law and assuming the amount of gas and temperature are constant, the pressure-volume relationship (Boyle's Law) shows that pressure is inversely proportional to volume. The initial pressure is 760 mm Hg (1 atm), and the volume increases from 125.0 mL to 1500 mL (1.50 L). Thus, the new pressure is (125.0/1500) * 1 atm = 0.0833 atm.

A 1250-ML Contains a Gas at 27°C and 760 Mm Hg