Hope this helps
In a nitrogen gas occupies has a volume of 500ml at a pressure of 0.971 atm. What volume will the gas occupies at a pressure of 1.50 atm, assuming the temperature remains constant?
V1 (initial volume) = 500 ml V2 (final volume) = unknown ?
P1 (initial pressure) = 0.971 atm P2 (final pressure) = 1.50 atm
This problem can be solve using Boyle's Law in which volume is inversely proportional to pressure when temperature and the amount of gas are constant. When Pressure increases, volume decreases.The formula of Boyle's Law is P1V1 = P2V2To Solve for the V2 (final volume) we can use V2 = P1V1 / P2
V2 = P1V1 / P2
= 0.971 atm × 500 ml / 1.50 atm (cancel the unit atm)
= 485.5 ml / 1.50
= 323.67 ml
the volume is 323.67
Hope it helps=)