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chemistry
Asked Apr 17, 2012, 10:37 PM
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1 Answer what happens to the original pressure of a sample of a gas with each of the following changes. triple the volume and half the kelvin temperature. half the volume and double the kelvin temperature |
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| School's probably out on this one, but here's practicing an answer: Assuming the sample behaves as an ideal gas, PV = nRT enables predicting what happens under the change in conditions specified. Using subsripts to describe the before (b) and after (a) conditions: Pa/Pb = TaVb/TbVa. In the first case, the pressure would be 1/6 after and four times more in the second case. | ||||
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