When extra NH3 is added to the system referenced above, the equilibrium point will shift in which direction of the equation (reactant or product side)?


2. When N2 is removed from the system referenced above, the equilibrium point will shift in which direction of the equation (reactant or product side)?

3. When H2 is added to the system referenced above, the equilibrium point will shift in which direction of the equation (reactant or product side)?

4. When the pressure is increased in the system referenced above, the equilibrium point will shift in which direction of the equation (reactant or product side)?


5. When the pressure is decreased in the system referenced above, the equilibrium point will shift in which direction of the equation (reactant or product side)?

Using complete sentences, respond to questions 6 -7 using the equation below. Be sure to explain your reasoning:

2 HCl (aq) + Mg(s) <--> MgCl2 (aq) + H2 (g) + heat

6. When the temperature is increased in the system referenced above, the equilibrium point will shift in which direction of the equation (reactant or product side)?

7. When the temperature is decreased in the system referenced above, the equilibrium point will shift in which direction of the equation (reactant or product side)?

Using complete sentences, respond to question 8 using the equation below. Be sure to explain your reasoning:
Fe3+ (yellow) + SCN- (colorless) <--> [FeSCN]2+ (dark red)

8. If aqueous Iron (III) chloride is added to the solution above at equilibrium, the reaction will become colorless, more yellow or darker red. Remember to explain the reasoning behind your choice.

Numbers 1-5 Reference an Equation that is not available.

1. Write your equation.
2. Review 'Le Chatelier's Principle'. I guess that if you are being asked those questions, you should have been taught this principle. Just apply it in reversible reactions whenever needed.

If you don't understand the principle, feel free to ask.