A balloon filled with helium gas at 8.25 atm occupies 56.0 L.. What volume would the balloon occupy in the upper atmosphere, at a pressure of 4.25 atm and a constant temperature? Be sure your answer has the correct number of significant figures.
To solve this problem, we can use the ideal gas law:
P₁V₁ = P₂V₂
where:
P₁ = initial pressure = 8.25 atm
V₁ = initial volume = 56.0 L
P₂ = final pressure = 4.25 atm
V₂ = final volume (what we need to solve for)
Substitute the values into the equation:
(8.25 atm)(56.0 L) = (4.25 atm)(V₂)
462 = 4.25V₂
Divide both sides by 4.25 to solve for V₂:
V₂ = 462 / 4.25
V₂ = 108.706 L
Therefore, the balloon would occupy 108.7 L in the upper atmosphere.