Gas Laws: Boyles Law Charless Law Avogadros Law Combined Gas Law Ideal Gas Law Constants and Conversions: Pressure Conversions 1 atm = 760mmHg 1 atm = 760 Torr 1 atm = 101.325 Pa Temperature Conversions: K = °C + 273.15 °F = (°C x 1.8) + 32 °C = Metric Conversions: 1 L = 103 mL Gas Law Constant: R = 0.08206
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?1 ?1 = ?2 ?2
?1 ?1 ?2 ?2
Combined Gas Law
?? = ???
Ideal Gas Law
Constants and Conversions:
1 atm = 760mmHg
1 atm = 760 Torr
1 atm = 101.325 Pa
K = °C + 273.15
°F = (°C x 1.8) + 32
1 L = 103 mL
Gas Law Constant:
R = 0.08206
1. Fill in the chart below for the three properties used to describe gases. For the last column,
predict whether the property would increase/decrease, if volume were to decrease.
If Volume decreases,
2. Convert the following units to their standard units:
b. 519 mmHg
c. 33 mL
3. A 125 mL sample of He (g) is kept at a pressure of 1 atm. If the pressure decreases to 519
mmHg, what is the new volume of gas?
4. Initially, a sample of gas has a temperature of 42°C and a volume of 33 mL. If the gas expands to
525 mL, what is the final temperature of the gas?
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