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Chemistry µIB
1.3b Gas Laws
10 quick questions

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10 minutes maximum!

An IB Periodic Table is required. Calculators should not be used!

 

1. Which of the following is NOT a characteristic of an ideal gas?
  • A.   There is a weak attractive force between the molecules
  • B.   Gas molecules occupy a negligible volume
  • C.   Gas molecules are in random motion
  • D.   Only elastic collisions occur between molecules
2. Which graph represents the relationship between the pressure (in Pa) and the volume (in dm3) of a fixed mass of an ideal gas at constant temperature?

P ~ V graphs for gases x 4

3. The deviation between real gas and ideal gas behavior is greatest at ...
  • A.   high temperature and low pressure
  • B.   high temperature and high pressure
  • C.   low temperature and low pressure
  • D.   low temperature and high pressure
4. What will happen to the pressure of a fixed mass of gas if the temperature (in K) and the volume are both doubled?
  • A.   It will remain the same
  • B.   It will increase by a factor of 2
  • C.   It will increase by a factor of 4
  • D.   It will decrease
5. A fixed mass of a gas occupies 40cm3 at 27°C. At what temperature, in °C, will the volume of gas be 80cm3 if the pressure remains constant?
  • A.   54
  • B.   150
  • C.   327
  • D.   600
6. The pressure and temperature (in K) of a fixed mass of gas are both halved. If the initial volume of the gas was 100cm3, what is the new volume?
  • A.   50cm3
  • B.   100cm3
  • C.   200cm3
  • D.   400cm3

7. Which graph represents the relationship between the volume (in cm3) and the temperature (in °C) of a fixed mass of an ideal gas at constant pressure?

V~T graph for a gas x 4

8. How many moles of gas are in a container of volume 2000cm3 at 100kPa pressure and a temperature of 400K?
(R = 8.31 J K-1 mol-1)
 
  • A. 
$${100 \times 2000} \over{8.31 \times 400}$$
  • B. 
$${100 \times 2} \over{8.31 \times 400}$$
  • C. 
$${100 \times 2000} \over{8.31 \times 127}$$
  • D. 
$${100 000 \times 2000} \over{8.31 \times 400}$$
9. A fixed mass of gas is at a pressure of 4kPa.

The volume of the gas is halved and the temperature (in K) of the gas is doubled.
What is the new gas pressure after these changes?

  • A.   1kPa
  • B.   4kPa
  • C.   8kPa
  • D.   16kPa
10. What is the molecular mass of gas Z if 2.00g of the gas occupies a volume of 500cm3 at 25°C and 1.01 x 105 Pa?
(R = 8.31 J K-1 mol-1)
 
  • A. 
$${2.00 \times 8.31 \times 25} \over{1.01 \times 10^5 \times 0.5}$$
  • B. 
$${1.01 \times 10^5 \times 0.5} \over{2.00 \times 8.31 \times 298}$$
  • C. 
$${2.00 \times 8.31 \times 298} \over{1.01 \times 10^5 \times 5 \times 10^{-4}}$$
  • D. 
$${1.01 \times 10^5 \times 5 \times 10^{-4}} \over{2.00 \times 8.31 \times 298}$$