5 need help with this please

Question

A gas‑filled weather balloon has a volume of 57.0 L at ground level, where the pressure is 755 mmHg and the temperature is 23.2 ∘C. After being released, the balloon rises to an altitude where the temperature is −2.84 ∘C and the pressure is 0.0569 atm. What is the weather balloon's volume at the higher altitude?

Answer 1

Hi Andrea!

This question is similar to the ones earlier using Charles' Law and Boyle's Law - only this time we're going to combine them (along with Gay Lussac's Law) to form the Combined Gas Law. Just a couple rules -- like before, all temperatures must be in Kelvin. As for volume and pressure, the units don't matter, as long as they are matching on both sides of the equation. For this problem, we're going to have to convert our pressures to make them match -- remember, 1 atm = 760 mmHg = 760 Torr.

So first, let's get our mmHg into atmospheres...755 mmHg * (1 atm / 760 mmHg) = 0.9934 atm

The Combined Gas Law is.... P₁V₁/T₁ = P₂V₂/T₂

So plugging in the numbers, we get (.9934atm * 57.0L)/(296.2K) = (0.0569atm * V2)/(270.16K)

And solving for V₂, we get 907.7L. Woof, that's huge!

Hope that helps!

-Niral