You fill a balloon with helium gas to a volume of 2.96 L at 23 °C and 758 mmHg. Now you release the balloon. What would be the volume of the helium if its pressure changes to 636 mmHg but the temperature is unchanged?
2007-10-15 08:21:08 · 3 answers · asked by Bernie 1 in Science & Mathematics ➔ Chemistry
Temperature is constant.
you will use Boyle's Law:
P1V1 = P2V2
V1 = 2.96 L
P1 = 758 mm Hg
P2 = 636 mm Hg
V2 = ?
V2 = P1V2/P2 = (758 mm Hg) (2.96L)/(636 mm Hg)
= 3.53 L
ref: http://en.wikipedia.org/wiki/Boyle's_Law
2007-10-15 08:28:35 · answer #1 · answered by Dr Dave P 7 · 0⤊ 0⤋
P1V1=P2V2
If the temperature and the amount of gas are constant, you can always use this relationship.
2007-10-15 15:26:38 · answer #2 · answered by hcbiochem 7 · 0⤊ 0⤋
PiVi=PfVf
make sure your units match up :)
2007-10-15 15:26:24 · answer #3 · answered by nacsez 6 · 0⤊ 0⤋