Calcutta University (BSc II) Chemistry

Chemistry General

PART II CGT 22a

Unit II. Basic physical chemistry IV

1.      Are pure solids included in equilibrium expressions? Explain.

2.      What will happen to reaction of system if temperature is raised at equilibrium?

3.      Explain how the equilibrium shifts when energy is added or removed from a system?

4.      What is common ion? Explain how a common ion reduces the solubility of an ionic compound.

5.      How can you use the solubility product constant to calculate the solubility of a sparingly soluble ionic compound?

6.      What is common ion? Explain how a common ion reduces the solubility of an ionic compound.

7.      What is Le Chatelier’s principle? How it is applied to equilibrium systems?

8.      What is the K value for the following equation if the gaseous mixture in a 4 L container reaches equilibrium at 1000 K and contains 4.0 mol of N₂, 6.4 mol of H₂, and 0.40 mol of NH₃?                                       

               N₂(g) + 3H₂(g) ←→ 2NH₃(g)

9.      What is the Tyndall effect? Give a common example of this effect.

10.  What is the difference between a solute and solvent? Name a compound considered to be ‘universal’ solvent?

11.  Given an unknown mixture consisting of two substances, explain how a scientist could use lab techniques to determine whether the mixture is a true solution, a colloid or a suspension.

12.  Which out of milk, blood, fog and mayonnaise is not an example of colloid?

13.   Describe Brownian motion. How it is caused?

14.  Distinguish between colloids and true solutions?

15.  How does a colloid differ from a suspension?

16.  What is the difference between hydration and solvation?