A balloon filled with helium gas at 1.00 atm occupies 12.9 L. What volume would the balloon occupy in the upper atmosphere, at a pressure of 0.19 atm and a constant temperature? Enter your answer in the box provided.

67,9 L

Explanation:

Boyle's Law indicates that the pressure of a fixed amount of gas at a constant temperature is inversely proportional to the volume of a gas, for a constant amount of gas we can write:

P1V1=P2V2

For the problem:

P1 = 1 atm, V1 = 12,9 L

P2=0,19 atm, V2=?

Therefore:

V2=P1V1/P2 ... V2=1 atm*12,9L/0,19 atm = 67,9 L

The balloon would occupy a volume of 67,9 L in the upper atmosphere.