V
(State the unit that is associated with V as well)
Volume
L (liters)
100
What is the Ideal Gas Law?
PV = nRT
100
How many moles of gas does it take to occupy 120. liters at a pressure of 2.30 atmospheres and a temperature of 340. K?
9.89 moles
100
Convert 2000. Torrs to atm.
2.632 atm
200
n
Number of moles
200
What is the universal constant?
The combined proportionality (.08206 L atm/K per mol)
200
If I have a 50.0 liter container that holds 45.0 moles of gas at a temperature of 200° C, what is the pressure inside the container? (Solve in atm)
34.9 atm
200
Convert 3.4 x 10-4atm to torrs.
0.26 torrs
300
T
(State the unit that is associated with T as well)
Temperature (Kelvins)
300
What are the units expressed for P, V,n, and T according to the Universal Gas Constant?
Atm, Liters, moles and Kelvins
300
How many moles of gas are in a 30.00 liter scuba canister if the temperature of the canister is 300.0 K and the pressure is 200.0 atmospheres?
243.7 moles
300
Convert 3.4 x 10-4atm to Pa.
35 Pa
400
R
Universal Gas Constant
400
What is the Ideal Gas Law Equation solved for n?
n=PV⁄RT
400
I have a balloon that can hold 100.0 liters of air. If I blow up this balloon with 3.000 moles of oxygen gas at a pressure of 1.000 atmosphere, what is the temperature of the balloon?
406.2 K
400
Convert 3.48 kPa to atm.
0.0343 atm
500
P
Name three of the units associated with P as well.
Pressure
atm, Psi, Pa, Torr
500
What are the 5 steps to GUESS (15 seconds)
Given, Unknown, Equation, Substitute, Solve
500
A sample of helium was compressed at 35 °C from a volume of 0.50 L to 0.25 L where the pressure is 450 mmHg. What was the original pressure?
Use Boyle’s Law for a constant temperature case of the ideal gas law:
PiVi = PfVf