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
What is the pressure at STP?
1 atm = 760 mmHg
What does it mean when we say a gas is ideal?
It means that there is no attraction between the gas molecules/atoms
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
If I have 3.7 moles of gas at 5 L and 210 K, what would the Pressure be?
12.8 atm
If an aerosol can is heated up, and the volume remains constant because the container is rigid, which quantity must change?
Pressure
If I have 22 L of gas at 3.3 atm and 280 K, how many moles do I have?
3.16 moles
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.
Daily Double - Name the individual gas law (the answer is NOT 'combined gas law') that this video illustrates.
Charles' Law
If I have 0.7 moles of gas at 1.3 atm and 43 L, what would the T be?
973 K
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.
(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
If a container of O2 at 300K has a pressure of 2 atm, and occupies a volume of 5 L, how many grams of O2 are there?
13 grams
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!)