a sample of ideal gas at 1.00 atm and a volume of 1.7 L was placed in a weighted ballon and dropped into the ocean. as the sample descended, *continued below

Question

* the water pressure compressed the ballon and reduced tis volume. when the pressure had increased to 45.0 atm, what was the volume of the sample? assume the temp was held constant.

Answer 1

Constant temperature ⇒ Use Boyle's law

 

P₁V₁ = P₂V₂ ⇒

 

V₂ = (P₁/P₂)V₁ = [(1.00 atm)/(45.0 atm)] (1.7 L) ≅ 0.0378 L