Chemistry 11 Practice Quiz for Gas Laws
Solutions

 

1)      In your own words describe what you observed in Lab #8 on Charles’ Law.  (Hint: you put the plastic bag filled with air into ice water…).  In particular, describe how the volume of gas changed as the temperature changed.

2)      A mixture of gases at 2.4 atm total pressure is made up of equal parts of helium, oxygen and nitrogen.  What is the partial pressure of each gas?  Bonus: If you doubled the amount of helium gas and kept the total pressure the same, what would the partial pressure of each gas be?

3)      A sample of helium gas of volume 1.5 L is at STP (I will expect you to know what this means for the test).   How many moles of helium are there? 

4)      A rigid box contains gas at 20ºC and a pressure of 1.6 atm.  What will the pressure be at 100ºC?

5)      Do the following conversions:

a)      650 Torr to Pa

b)      2.26 × 10²⁴units to moles

c)      95 mL to m³

 

Conversions

1000 L =  1m³

T_K = T_C + 273

6.02 × 10²³units = 1 mole

760 Torr = 1.0 atm = 1.01× 10⁵ Pa

Prefixes: milli = m = 10^-3