Warm-up 1
The molar volume of an ideal gas at STP is
a. 6.02 x 1023 L
b. 11.2 L
c. 22.4 L
d. 0.0821 L
Warm-up 2
Use your knowledge of KMT to explain Boyle’s Law (pressure and volume are inversely related).
Less space (↓ V) will cause more collisions with the sides of the container (P ↑)
Warm-up 3
Use your knowledge of KMT to explain Chares’ Law (volume and temperature are directly related).
Faster particles (↑ T) at same P will require a larger container (↑ V)
Warm-up 4
1. Carlos is heating a can of soup over a campfire. It explodes and he is covered in soup. What law
does this show?
a. Boyle’s Law
b. Charles’ Law
c. Gay-Lussac’s Law
2. What should Carlos have done to prevent the can from exploding?
a. make the can smaller
b. shake the can up
c. punch a hole in the can
Warm-up 5
Provide a definition for the following three variable so you can understand them:
P: collisions with sides of the container
V: size of container
T: speed of particles (ave KE)
Warm-up 6
1. What is the ideal gas law equation?
PV=nRT
2. What is the value of “R” in
0.08206
𝐿 𝑎𝑡𝑚
𝑚𝑜𝑙 𝐾
3. What is the value of “R” in
8.314
𝐿 𝑎𝑡𝑚
𝑚𝑜𝑙 𝐾
𝑑𝑚3 𝑘𝑃𝑎
𝑚𝑜𝑙 𝐾
𝑑𝑚3 𝑘𝑃𝑎
𝑚𝑜𝑙 𝐾
Warm-up 7
How is the combined gas law different from the ideal gas law (how would you know which one to use)?
Combined gas law has old conditions and new conditions (n remains constant)
Ideal gas law has ONE set of conditions (n can change)