# Gases (Ch 5) 1. ? Describe Boyle’s Law, Charles’ Law and

## Transcription

Gases (Ch 5) 1. ? Describe Boyle’s Law, Charles’ Law and
```Gases (Ch 5)
1. Describe Boyle’s Law, Charles’ Law and
Avogadro’s Law. If you combine them, what
do you get ?
Gases (Ch 5)
2. A tank of nitrous oxide (N2O) has a volume of
160. L and contains 34.5 kg of the gas. At
25 °C, what is the pressure of the nitrous in
the tank?
Gases (Ch 5)
3. A balloon is filled with 1.00 L of helium at
27.0 °C and 1.00 atm. The balloon rises to a
point in the atmosphere where the temperature
is -35.0 °C and the pressure is 250. torr. What
is the change in volume the balloon
underwent?
Gases (Ch 5)
4. Consider the flasks diagrammed below. What is
the total pressure (in atm) after the stopcock
between the two flasks is opened? (Assume the
final volume is 3.00 L)
Gases (Ch 5)
5. An unknown diatomic gas has a density of
3.164 g/L at STP. What is the identity of the
gas?
Gases (Ch 5)
6. A mixture of 1.00 g of hydrogen and 1.00 g of
helium exerts a pressure of 0.480 atm.
What is the partial pressure of each gas?
Gases (Ch 5)
7. A gas mixture of Ne and Ar has a total
pressure of 4.00 atm and contains 16.0 mol of
gas. If the partial pressure of Ne is 2.75 atm,
how many moles of Ar are in the mixture?
Gases (Ch 5)
8. The hydrogen gas formed in a chemical
reaction is collected over water at 30.0 °C at
an atmospheric pressure of 732 torr. If the
volume of gas collected is 722 mL, calculate
the mass of hydrogen produced by the
reaction. (The vapor pressure of water at 30.0
°C is 31.86 torr)
Gases (Ch 5)
9. According to Kinetic Molecular Theory, what
are the assumptions for an ideal gas?
Gases (Ch 5)
10. Indicate if and how each of the following changes
will affect these properties:
Increasing the Increasing the Increasing
volume
mass of gas
temperature
particle
Average
kinetic energy
Root mean
square
velocity
Frequency of
collisions
Increasing
moles of gas
Gases (Ch 5)
11. It took 10.0 minutes for a sample of hydrogen
gas to effuse through a porous barrier. How
long will it take for the same amount of
chlorine gas to effuse under identical
conditions?
Gases (Ch 5)
12. Answer the following, given the velocity curves below:
a. If the plots represent 1.0 L H2 versus 1.0 L N2 at STP, which
corresponds to each gas?
b. If the plots represent 1.0 L H2 at 273 K versus 1.0 L H2 at 1000
K, which corresponds to each temperature?
Gases (Ch 5)
13. Consider 784 mol of nitrous gas (N2O) in a
160 L tank at 25.0 °C . Calculate the pressure
using:
a. the ideal gas law
b. the van der Waals equation
(a= 3.83 atm L2/mol2, b = 0.044 L / mol)
Gases (Ch 5)
Bonus Q:
What happens to a person who inhales SF6 gas
(a gas more dense than air)? …
….see for yourself:
```

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