The sample 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 85.0 atm, what was the volume of the sample? Assume that the temperature was held constant?
Please explain the atmospheric pressure? Thank you!
Please explain the atmospheric pressure? Thank you!
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The combined gas law is expressed in the formula PV = NRT where
P is pressure
V is volume
N is quantity of gas
R is a constant determined by the units you want to use
T is the absolute temperature
If temperature does not change then PV = K and that is the condition of this question. So you have P1V1 = P2V2 or 1.00 x 1.03 = 85 x V2
V2 = 1.03/85 = .0121 liter
P is pressure
V is volume
N is quantity of gas
R is a constant determined by the units you want to use
T is the absolute temperature
If temperature does not change then PV = K and that is the condition of this question. So you have P1V1 = P2V2 or 1.00 x 1.03 = 85 x V2
V2 = 1.03/85 = .0121 liter