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The Gas Laws

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David Madorin

on 5 May 2016

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Transcript of The Gas Laws

The Gas Laws
Boyle's Law
For a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure
Charles's Law
the volume of a fixed gas is directly proportional to its Kelvin temperature if the pressure is constant
Gay-Lussac's Law
the pressure of a gas is directly proportional to the Kelvin temperature if the volume remains constant
A balloon contains 30.0 L of He
(g) at 103 kPa. What is the volume of the He when the ballon rises to an altitude where the pressure is only 25 kPa?
124 L
A balloon inflated in a room at 24 degrees Centigrade has a volume of 4.00L. The balloon is then heated to a temperature of 58 degrees Centigrade. What is the new volume of the balloon?
The gas in a used aerosol can is at a pressure of 103 kPa at 25 degress Centigrade. If the can is thrown in a fire, what will the pressure be when the temperature reaches 928 degrees Centigrade?
415 kPa
The Combined Gas Law
describes the relationship among the pressure, temperature, and volume of an enclosed gas
The volume of a gas filled balloon is 30.0 L at 313 Kelvin and 153 kPa pressure. What would the volume be at standard temperature and pressure (STP)?
The Ideal Gas Law
Used to calculate the number of moles of a contained gas
PV = nRT
P = Pressure V = Volume n = number of moles R = Ideal Gas Constant T = Temperature
A deep underground cavern contains 2,240,000 L of methane gas at a pressure of 1,500 kPa and a temperature of 315 K. How many kilograms of methane does the cavern contain?
20591.77 kg Methane
Dalton's Law
In a mixture, the total pressure is the sum of the partial pressures of the gases
Air contains oxygen, nitrogen, carbon dioxide, and trace amounts of other gases. What is the partial pressure of oxygen at 101.30 kPa of total pressure if the partial pressures of nitrogen, carbon dioxide, and other gases are 79.10 kPa, 0.040 kPa, and 0.94 kPa respectively?
21.22 kPa
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