A sample of an ideal gas at 1.00 atm 1.00 atm and a volume of 1.45 L 1.45 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 70.0 atm, 70.0 atm, what was the volume of the sample? Assume that the temperature was held constant.

Question

Aaden

Chemistry

13 March, 21:16

A sample of an ideal gas at 1.00 atm 1.00 atm and a volume of 1.45 L 1.45 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 70.0 atm, 70.0 atm, what was the volume of the sample? Assume that the temperature was held constant.

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Connor Williamson · Answer 1

0.21L

Explanation:

To solve this problem, we make use of Boyle's law. It states that at constant temperature, the volume of a fixed mass of gas is inversely proportional to its pressure.

Mathematically PV = K

P1V1 = P2V2

P1 = 1 atm

V1 = 1.45L

P2 = 70 atm

v2 = ?

From the equation form, we know that

V2 = P1V1/V2

V2 = (1 * 1.45) / 70

V2 = 0.021L