Gas Laws 1
Ideal Gas Law
Gas Laws 2
KMT
100

If I start with 30 mL at 200 K and heat it to 400 K, what would be the new volume. (Pressure is constant)

60 mL

100

If I have 0.7 moles of gas at 131.7 kPa and 43 L, what would the T be?

973 K

100

What is the pressure at STP?

1 atm = 760 mmHg

100

What does it mean when we say a gas is ideal?

It means that there is no attraction between the gas molecules/atoms

200

If I start with 0.9 atm at 10 Celsius and cool it to 3 Celsius, what would be the new pressure. (Volume is constant)

0.88 atm

200

If I have 3.7 moles of gas at 5 L and 210 K, what would the Pressure be?

1297 kPa

200
How many liters are in 50 grams of Cl2 at STP?
15.8 L
200
What does the kinetic energy of gas particles depend upon?
Temperature
300

If an aerosol can is heated up, and the volume remains constant because the container is rigid, which quantity must change?

Pressure

300

If I have 22 L of gas at 334.3 kPa and 280 K, how many moles do I have?

3.16 moles

300
Of the 3 laws, which 2 have a direct relationship (one goes up, so does the other) and which has an indirect relationship (one increases while the other decreases)?
Charles and Gay-Lussac = direct
Boyles = indirect
300

Using KMT, describe what is happening when the pressure inside a container increases

The number of collisions between the gas particles and the walls of the container is increasing.

400

Daily Double - Name the individual gas law (the answer is NOT 'combined gas law') that this video illustrates.

Charles' Law

400

If a container of O2 at 300K has a pressure of 202.6 kPa, and occupies a volume of 5 L, how many grams of O2 are there?

13 grams

400
A mixture of gases with a pressure of 600.0 mmHg contains nitrogen with a partial pressure of 420 mmHg and oxygen. What is the partial pressure of oxygen in this mixture?
180 mmHg
400

Using KMT, explain the relationship between temperature and volume (keeping pressure constant).

As the volume of the gas gets larger, in order for the pressure to remain the same (# of collisions with the walls stays the same), the temperature of the gas must also get larger.

500

(Intro Hint: When solving a Combined Gas Law Problem, what is the ONLY variable that must have its units converted?) If I start with 44 mL at 10 Celsius and 152 mmHg, and heat it to 41 Celsius while increasing the pressure to 2432 mmHg, what would be the new volume.

3.05 mL

500

What is the value for R, and what are its units?

0.0821 L*atm/mol*K

8.31 L*kPa/mol*K

500

If you have collected an unknown gas in an inverted graduated cylinder via the water displacement method at a barometric pressure of 752 mmHg, and the water temperature is 18.5 C, what is the partial pressure of the unknown gas? (P H2O  at 18.5 C is 16 mmHg)

736 mmHg

500

Why can't we apply the laws of KMT to liquids

The atoms/molecules do not behave ideally (they attract each other, which is why it is a liquid in the first place!)

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