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Vahlhalla Applying Boyles Law Practices

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Znevrcynbg

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Vahlhalla

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Identify the variables in each problem to determine which of the gas laws you will use and make sure to show your work and to show the formula you are using for each problem.

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Make sure to show the formula you are using for each problem and the substitutions. 1. A gas occuples 10 Lat 760 mmHg of pressure. What will the new gas pressure be if the volume increases to 20 L? 2. A gas occupies a volume of 3.0 Lat 1 atm. If the pressure is decreased to 0.5 atm, what will the new volume be? 3. A balloon is inflated to a volume of 2.0 L. If the temperature of air inside the balloon is warmed from -73°C to 27°C what will be the final volume? (be careful of the temp units!) 4. 100 mL of hydrogen gas is collected at a temperature of 250 K. If the temperature falls to 50 K, what will be the final gas volume? 5. A gas sample at is standard temperature and pressure and is brought to 0.5 atm of pressure. What is the new temperature? (look up the values for STP in your notes if you don't remember them!) 6. A sample of gas at 300 K and 600 mmHg is cooled to 200 K. What is the resulting pressure? 7. A balloon contains 3.4 moles of helium gas. An additional 0.6 moles of gas are added to the balloon giving it a volume of 8 L. What was the original volume of the balloon? (be careful with your substitution!) 8. 5.0 moles of H;gas in a balloon have a volume of 20 L. Some of the gas effuses out. How much gas remains if the volume is now 16 L?
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Explanation & Answer

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1. Applying boyles law
PV = constant
P1v1 = p2v2
P2 = p1v1/v2
= 10 x 760 / 20
= 380 mmHg.
2. Applying boyles law
PV = constant
P1v1 = p2v2
V2 = p1v1/p2
= 3 x 1/0.5
=6L
3. Applying charles law
V/T = constant
v1/T1 = v2/T2
T1= 273 + (-73) = 200 K
T2= 273 + (27) = 300 K
V2 = V1T2/T1
= 2 x 300 / 200
=3L
4. Applying charles law
V/T = constant
v1/T1 = v2/T2
T1= 250 ...

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