Chemistry Exam Practice Questions

Question 1: Intermolecular Forces

1. List all types of IMFs that would occur in each of the following . First draw the lewis structures or 3D structures.

a. CH3Br                  c. CH3CH3
b. CCl4                     d. CN

2. List the dominant (strongest) type of IMF for the pure substances, then rank the strength of each compound based on IMFs within the samples.  (1 = strongest, 2 = in between, 3 = weakest)

3. State the following laws. Use both words and equations:

(a) Boyle’s Law
(b) Charles’ Law
(c) Dalton’s Law of Partial Pressures

4. A gas sample contained in a cylinder equipped with a moveable piston occupied 300.0 mL at a pressure of 2.00 atm. What would be the final pressure if the volume were increased to 500.0 mL at constant temperature?

5. Several balloons are inflated with helium to a volume of 0.75 L at 27°C. One of the balloons was found several hours later, the temperature had dropped to 22°C. What would be the volume of the balloon when found, if no helium has escaped? 

6. A given sample of gas has a volume of 4.20 L at 60.0 C and 1.00 atm pressure. Calculate its pressure if the volume is changed to 5.00 L and the temperature to 27 C. 

7. If 45 mL of water are added to 250 mL of a 0.75 M K2SO4 solution, what will the molarity of the final solution?

8. How would you prepare 250.0 mL of a 1.40 M solution CuSO4?

9. A solution is made by dissolving 25 g of sodium chloride in 240 g of water. What is the percent by mass?

10. If 45 mL of water are added to 250 mL of a 0.75 M K2SO4 solution, what will the molarity of the diluted solution be?

11. Calculate the molality, freezing point, and boiling point for each of the following water solutions of nonionizing solutes: 0.144 g of C6H12O6 dissolved in 1500 g of H2O

12. Calculate the boiling point of a solution made by dissolving 1.00 g of glycerin, C3H8O3, in 54.0 g of water

13. Calculate the boiling point of an ionic solution containing 29.7 g MgCl2 and 84.4 g water.