10.0 grams of a gas occupies 12.5 liters at a pressure of 42.0 mm Hg. What is the volume when the pressure has increased to 75.0 mm Hg? 0.143 L 6.72 L 7.00 L 22.3 L

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Chemistry

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30 April, 10:22

10.0 grams of a gas occupies 12.5 liters at a pressure of 42.0 mm Hg. What is the volume when the pressure has increased to 75.0 mm Hg? 0.143 L 6.72 L 7.00 L 22.3 L

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Amari Simon · Answer 1

To solve this we assume that the gas is an ideal gas. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant temperature and number of moles of the gas the product of PV is equal to some constant. At another set of condition of temperature, the constant is still the same. Calculations are as follows:

P1V1 = P2V2

V2 = P1 x V1 / P2

V2 = 42.0 x 12.5 / 75.0

V2 = 7.0 L