Can someone please solve this

Question

A sample of an ideal gas at 1.00 atm and a volume of 1.37 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 10.0 atm, what was the volume of the sample? Assume that the temperature was held constant.

𝑉= __________ L

Answer 1

In order to solve this problem, we need to use a deviation from the ideal gas law: Boyle's Law. The equation for Boyle's Law is stated below:

P₁V₁ = P₂V₂

P₁ = first pressure

P₂ = second pressure

V₁ = first volume

V₂ = second volume

We know that we need to use a deviation from the ideal gas law PV = nRT because this problem talks about gases. Additionally, we know that we need to use Boyle's Law compared to the other deviations of the gas law because this problem contains that volume and the pressure of a gas. We do not need temperature (T), constant (R), or moles (n) because in the given problem they are stated as constant (T, and by definition R is constant) or not mentioned (n).

So, in this problem:

P₁ = 1.00 atm

P₂ = 10.0 atm

V₁ = 1.37 L

V₂ = ?

Plugging the values into Boyle's Law:

P₁V₁ = P₂V₂

(1.00 atm) (1.37 L) = (10.0 atm) V₂ Solving using algebra

V₂ = 0.137 L (3 significant figures)