A sample of an ideal gas at 1.00 atm and a volume of 1.72 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 35.0 atm, what was the volume of the sample? assume that the temperature was held constant.

Question

Arjun Jackson

Chemistry

20 December, 11:09

A sample of an ideal gas at 1.00 atm and a volume of 1.72 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 35.0 atm, what was the volume of the sample? assume that the temperature was held constant.

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Delilah Farley · Answer 1

If we analyze the situation analytically, there are situations or states. Then, we are also given with 2 values of pressure and 1 value of volume. Lastly, temperature was set as constant. Thus, this means we use the Boyle's Law.

P₁V₁ = P₂V₂

Let's find V₂.

(1 atm) (1.72 L) = (35 atm) (V₂)

Solving for V₂,

V₂ = 0.049 L