pp. 302-306 13.2 the gas laws. boyle’s law robert boyle seventeenth-century irish chemist
TRANSCRIPT
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PP. 302-306
13.2 THE GAS LAWS
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Boyle’s law
Robert Boyle
Seventeenth-century Irish Chemist
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Boyles Law
States that for a fixed amount of gas at a constant temperature, the volume of a gas increases as its pressure decreases.
Likewise the volume of a gas decreases as its pressure increases.
Use PTV ruler
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13.2 Boyle’s Law
When you squeeze a fixed quantity of gas into a smaller volume the pressure goes up.
This rule is known as Boyle’s law.
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13.2 Boyle’s Law
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Solving Problems
A kit used to fix flat tires consists of an aerosol can containing compressed air and a patch to seal the hole in the tire. Suppose 5 liters of air at atmospheric pressure (1 atm) is compressed into a 0.5 liter aerosol can. What is the pressure of the compressed air in the can? Assume no change in temperature or mass.
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1. Looking for: …final pressure in atmospheres (P2)
2. Given …V1 = 5 L , P1= 1 atm, V2 = .5 L
3. Relationships: Boyle’s Law: P1V1 = P2V2
4. Solution Rearrange equation so P2 = P1V1 / V2
P2 = 1atm x 5.0 L/ 0.5 L = 10 atm.
Solving Problems
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13.2 Pressure and Temperature
The pressure of a gas is affected by temperature changes. If the mass and volume are kept constant, the pressure goes up when the temperature goes up, and down when the temperature goes down.
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13.2 Gay-Lussac’s Law
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Charles’s Law
Charles was a French physicist who studied gases and made the first ascent in a hydrogen filled balloon in 1783.
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Charles’s Law
States that for a fixed amount of gas at a constant pressure, the volume of the gas increases as its temperature increases.
Likewise, the volume of the gas decreases as its temperature decreases.
Use PTV ruler
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13.2 Charles’ Law
A hot-air balloon floats because the air inside is less dense than the air outside.
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13.2 Pressure and Temperature
Any time we apply gas laws, the temperature must be in Kelvins.
Only the Kelvin scale starts from absolute zero, when energy of particles is theoretically zero.
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13.2 Charles’ Law
According to Charles’ law, the volume of a gas increases with increasing temperature.
Volume decreases with decreasing temperature.
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Solving Problems
A balloon filled with helium has a volume of 0.50m³ at 21 C. Assuming the pressure and mass remain constant, what volume will the balloon occupy at 0 C.?.
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1. Looking for: …final volume in cubic meters (V2)
2. Given …T1= 21 C , T2 = 0 C, V = 0.50 m³
3. Relationships: Convert temps using K = C + 273 Charles’ Law: V1/T1 = V2/T2
4. Solution Rearrange equation so P2 = P1xT2 / T1
V2 = 0.50 m³ . x 273K / 294K = 0.46 m³.
Solving Problems