Initially, a 55.0 liter compressible container, holding 2.4 moles of a gas, exerts a pressure of 760 millimeters of mercury at a temperature of 280 Kelvin. What is the pressure when the container is compressed to 43.0 liters, the moles of gas reduces to 1.8 moles, and the temperature changes to 36 degrees Celsius?

93.7 mm Hg

492 mm Hg

740 mm Hg

805 mm Hg

Question

Chemistry

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15 January, 04:38

Initially, a 55.0 liter compressible container, holding 2.4 moles of a gas, exerts a pressure of 760 millimeters of mercury at a temperature of 280 Kelvin. What is the pressure when the container is compressed to 43.0 liters, the moles of gas reduces to 1.8 moles, and the temperature changes to 36 degrees Celsius?

93.7 mm Hg

492 mm Hg

740 mm Hg

805 mm Hg

+5

Answers (1)

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Laila Garza · Answer 1

You would have to use the ideal gas law for this:

PV=nRT

Pressure, Volume, n=moles, R gas constant, Temperature in Kelvin

P=nRT/V

(1.8mol) (62.36) (309K) / 43.0L = 805mm Hg