Gas Laws Section 3.2. Gas and Pressure Pressureresult of force distributed over an area.
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Transcript of Gas Laws Section 3.2. Gas and Pressure Pressureresult of force distributed over an area.
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Gas Laws
Section 3.2
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Gas and Pressure
• Pressure—result of force distributed over an area
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Gas and Pressure
• The wider the arrow, the greater the force. Which has the greatest pressure? The least pressure?
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What causes pressure?
• In a gas, it’s all about collisions– Atoms in a gas are constantly moving
• Collisions push against container and create pressure
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What affects pressure?
1) Temperature of gas2) Volume of gas3) Number of particles in gas
http://intro.chem.okstate.edu/1314F00/Laboratory/GLP.htm
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Temperature and Pressure
Overall, increasing the temperature increases the pressure
Higher temperature increases particle speed energy collisions pressure
http://intro.chem.okstate.edu/1314F00/Laboratory/GLP.htm
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Volume and Pressure
Overall, decreasing the volume increases the pressure
Less space means more collisions collisions pressure
http://intro.chem.okstate.edu/1314F00/Laboratory/GLP.htm
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Number of Particles and Pressure
Overall, increasing the number of particles increases the pressure
More particles means more collisions collisions pressure
http://intro.chem.okstate.edu/1314F00/Laboratory/GLP.htm
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The Gas Laws
Charles’s Law Boyle’s Law
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Charles’s Law
Jacques Charles Collected data on temperature
and volume
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Charles’s Law
Extended line to hit x-axis
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Charles’s Law
Temperature at which the volume is 0L is –273.15 C, or 0K.
Absolute zero Volume of gas is directly
proportional to the temperature (in Kelvin) if pressure and particle number are same
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Charles’s Law
V1 = V2
T1 T2
V1 = Initial volume T1= Initial temperature (K)
V2 = Final volume T2= Final temperature (K)
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Sample Problems
1. Steps: Identify any knowns as either V1, T1, V2, or T2
2. Make sure that all temperature values are in Kelvin
3. Plug knowns in equation4. Double-check that answer and
units make sense
http://www.chem.uiuc.edu/webFunChem/charleslaw/CLsample.htm
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A sample of gas at 101.3kPa had a volume of 1.2L at 100oC. What would its volume be at 0oC at the same pressure?
Vf = 0.88L
A balloon had a volume of 75L at 25oC. To what does the temperature need to raised in order for the balloon to have a volume of 100L at the same pressure?
Tf = 124oC
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Boyle’s Law
Robert Boyle Collected data on pressure and
volume
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Boyle’s Law
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Boyle’s Law
Volume of gas is inversely proportional to the pressure if the volume and particle number are same
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Boyle’s Law
P1V1 = P2V2
V1 = Initial volume P1= Initial pressure
V2 = Final volume R2= Final pressure
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Sample Problems
1. Steps: Identify any knowns as either V1, P1, V2, or P2
2. Plug knowns in equation3. Double-check that answer and
units make sense
http://www.chem.uiuc.edu/webFunChem/BoylesLaw/SampleProb6.htm
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The volume of the lungs is measured by the volume of air inhaled or exhaled. If the volume of the lungs is 2.400 L during exhalation and the pressure is 101.70 KPa, and the pressure during inhalation is 100.01 KPa, what is the volume of the lungs during inhalation?
2.441 L
It is hard to begin inflating a balloon. A pressure of 800.0 Kpa is required to initially inflate the balloon 225.0 mL. What is the final pressure when the balloon has reached it's capacity of 1.2 L?
150 Kpa
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Combined Gas Law
Describes the relationship between the temperature, volume, and pressure of a gas when the number of particles is constant
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Combined Gas Law
P1V1 = P2V2
T1 T2
V1 = Initial volume V2 = Final volume
T1 = Initial temperature (K) T2 = Final temperature (K)
P1 = Initial Pressure P2 = Final Pressure
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A gas takes up a volume of 17 liters, has a pressure of 2.3 atm, and a temperature of 299 K. If I raise the temperature to 350 K and lower the pressure to 1.5 atm, what is the new volume of the gas?
If I have 2.9 L of gas at a pressure of 5 atm and a temperature of 50
0C, what will be the temperature of the gas if I decrease the volume of the gas to 2.4 L and decrease the pressure to 3 atm?
If I have 17 liters of gas at a temperature of 67 0C and a pressure of 88.89 atm, what will be the pressure of the gas if I raise the temperature to 94 0C and decrease the volume to 12 liters? 136 atm
160 K
30.6 L
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