– Le Chatelier’s Principle Name _______________ Use the following equation to answer questions #1-6. [Cu(H2O)4]2+ + 2NH3 [Cu(NH3)4]2+ + 4 H2O 1. Which way will the reaction shift if NH3 is added? ____________________ 2. Which way will the reaction shift if water is added? _____________________ 3. Which way will the reaction shift if [Cu(H2O)4]2+ is removed? _____________________ 4. Which way will the reaction shift if [Cu(NH3)4]2+ is removed? ____________________ 5. What information would you need to know to determine the effect of changing temperature on the reaction? _______________________________________________________________________________________ 6. What information would you need to know to determine the effect of pressure on the system? _______________________________________________________________________________________ Use the following equation to answer questions #7-11. C (g) + Y(g) 3B(g) + heat In the reaction above C is colorless, Y is a bright yellow, and B is a bright blue. The system is initially at equilibrium and has a green color. 7. Adding a large quantity of C will result in what color at equilibrium? ______________________ 8. Cooling the system will result in what color? ______________________ 9. Adding a catalyst gives what color? _______________________ 10. Increasing the pressure will result in what color? _______________________ 11. Removing B from the system will result in what color? _______________________ 12. Suppose you’re thinking about using the following reaction to produce hydrogen from hydrogen sulfide. Keq for the equilibrium is 2.27 x 10-4 2 H2S(g) + heat 2 H2(g) + S2(g) a. Would you expect a high yield of hydrogen? ____________ b. What could you do to the volume of the reaction vessel to produce more hydrogen? ____________________ c. How could you change the temperature to increase the yield of hydrogen? ____________________________ 13. What effect would an increase in temperature have on these reactions at equilibrium? a. Heat + H2(g) + I2(g) 2HI(g) Shift LEFT or RIGHT or NO CHANGE b. CH4(g) + 2O2(g) CO(g) + 2H2O(g) + heat Shift LEFT or RIGHT or NO CHANGE c. N2(g) + 2H2(g) 2NH3(g) + heat Shift LEFT or RIGHT or NO CHANGE d. Heat + CH4(g) C(s) + 2H2(g) Shift LEFT or RIGHT or NO CHANGE 14. For each reaction, state whether increasing or decreasing the volume of the reaction vessel would yield more product at equilibrium. a. N2O4(g) 2NO2(g) INCREASE or DECREASE Volume b. 2SO3(g) 2SO2(g) + O2(g) INCREASE or DECREASE Volume c. CH4(g) + 2O2(g) CO2(g) + 2H2O(g) INCREASE or DECREASE Volume d. 2CO(g) + O2(g) 2CO2(g) INCREASE or DECREASE Volume 15. For a- f, fill in the blank with shift left, shift right, or no shift. a) Which way will the equilibrium shift if more H2 is added to this reaction at equilibrium? _____________ N2 + 3 H2 2 NH3 b) Which way will the equilibrium shift if the system temperature goes up (heat is added)? ________________ 2 SO2 + O2 2 SO3 + heat c) The container holding the following reaction (already at equilibrium) has its volume suddenly reduced by half. Which way will the equilibrium shift to compensate? __________________ PCl3 + Cl2 PCl5 d) The container holding the following reaction (already at equilibrium) has its volume suddenly increased. Which way will the equilibrium shift to compensate? __________________ H2 + Cl2 2 HCl e) The system below is already at equilibrium when some neon is added to the system. What happens to the position of the equilibrium? Does it shift right, left, or no change? __________________ H2 + Cl2 2 HCl f) The system below is already at equilibrium when a catalyst is added to the system. What happens to the position of the equilibrium? Does it shift right, left, or no change? __________________ PCl3 + Cl2 PCl5