1. Calculate the final molarity if 75.0 mL of a 5.0 M NaOH solution were diluted to a final volume of 650.0 mL. M 1 V 1 = M 2 V 2 0.58 M NaOH

2. Jared believes that equilibrium means the concentration of reactants is equal to the concentration of products. Do you agree or disagree? Explain your answer. Disagree because concentrations do not have to be equal at equilibrium

3. Explain the difference between activation energy and activated complex? Activation energy is the minimum amount of energy needed to react Activated complex is the intermediate between reactants and products

4. Explain the following P.E. diagram using correctly the terms endothermic and exothermic processes and reactions. Exothermic reaction Endothermic process Exothermic process

5. Which way would a system at equilibrium shift if products were removed? Towards the right (products)

6. Joe believes that a reaction stops when it reaches equilibrium. Do you agree or disagree? Explain your answer. Disagree because equilibrium is mainly about forward and reverse rates canceling each other out

7. Which way would a system at equilibrium shift if heat were added to an exothermic reaction? Towards the left (reactants) because heat is like a product in exothermic reactions (heat released)

8. Calculate the initial molarity of a Pb(NO 3 ) 2 solution if 40.0 mL were diluted to make 2.10 L of a 0.50 M Pb(NO 3 ) 2 solution. M 1 V 1 = M 2 V 2 26 M Pb(NO 3 ) 2

9. Which is the more diluted solution? Explain.

10. Explain how using reactants with a smaller surface area would affect the reaction rate in terms of the collision of particles. Smaller surface area would decrease reaction rate because less particles are exposed for collisions to occur

11. Which part of the P.E. diagram represents change in enthalpy?

12. What is the molar mass of Li 2 S? Please include units. 45.95 g/mol Li 2 S

13. Calculate the volume of a 6.0 M KOH solution needed to make 850.0 mL of a 1.20 M solution? M 1 V 1 = M 2 V 2 170 mL of 6.0 M KOH

14. Which way would a system at equilibrium shift if products were added? Towards the left (reactants)

15. Which is the more concentrated solution? Explain.

16. Which way would a system at equilibrium shift if reactants were added? Towards the right (products)

17. How many grams of MgSO 4 are required to prepare 350.0 mL of a 1.50 M solution? M = mol/L 63.2 g MgSO 4

18. Explain how decreasing the concentration of reactants would affect the reaction rate in terms of the collision of particles. Decreasing concentration would decrease reaction rate because less particles would be available to collide

19. What is the molar mass of KOH? Please include units. 56.11 g/mol KOH

20. Will this reaction be hot or cold to the touch? Explain. Hot because energy from the reaction is released to your hand

21. Which is the solvent in this solution?

22. Which way would a system at equilibrium shift if heat were removed from an endothermic reaction? Towards the left (reactants) because heat is like a reactant in endothermic reactions (heat absorbed)

23. Which way would a system at equilibrium shift if heat were added to an endothermic reaction? Towards the right (products) because heat acts like a reactant in endothermic reactions (absorbed)

24. Calculate the final volume in milliliters of a NH 4 Cl solution if 125.0 mL of a 7.0 M solution were diluted to 0.15 M. M 1 V 1 = M 2 V 2 5800 mL NH 4 Cl

25. Is the reaction endothermic or exothermic? Explain. Exothermic because energy of products is less than energy of reactants

26. What is the molar mass of HC 2 H 3 O 2 ? Please include units. 60.06 g/mol HC 2 H 3 O 2

27. Which way would a system at equilibrium shift if heat were removed from an exothermic reaction? Towards the right (products) because heat is like a product in exothermic reactions (heat released)

28. Which is the solute in this solution?

29. Which way would a system at equilibrium shift if reactants were removed? Towards the left (reactants)

30. What is the molarity of a solution containing 28.0 g of magnesium chloride in enough water to make 1.50 L of solution? M = mol/L 0.196 M MgCl 2

31. Calculate the final molarity if 15.0 mL of a 3.0 M NaOH solution were diluted to a final volume of 450.0 mL. M 1 V 1 = M 2 V 2 0.10 M NaOH

32. Calculate the initial molarity of a Pb(NO 3 ) 2 solution if 200.0 mL were diluted to make 1.00 L of a 0.30 M Pb(NO 3 ) 2 solution. M 1 V 1 = M 2 V 2 1.5 M Pb(NO 3 ) 2

33. What is the molar mass of sodium hydroxide? Please include units. 40.00 g/mol NaOH

34. Calculate the volume of a 2.0 M KOH solution needed to make 150.0 mL of a 0.50 M solution? M 1 V 1 = M 2 V 2 38 mL of 2.0 M KOH

35. How many grams of sodium chloride are required to prepare 150.0 mL of a 2.50 M solution? M = mol/L 21.9 g NaCl

36. What is the molar mass of HCl? Please include units. 36.46 g/mol HCl

37. Calculate the final volume in milliliters of a CaCl 2 solution if 25.0 mL of a 6.0 M solution were diluted to 0.10 M. M 1 V 1 = M 2 V 2 1500 mL CaCl 2

38. What is the molar mass of C 6 H 12 O 6 ? Please include units. 180.18 g/mol C 6 H 12 O 6

39. Explain the difference between activation energy and activated complex? Activation energy is the minimum amount of energy needed to react Activated complex is the intermediate between reactants and products

40. Explain the following P.E. diagram using correctly the terms endothermic and exothermic processes and reactions. Endothermic reaction Endothermic process Exothermic process

41. Which part of the P.E. diagram represents change in enthalpy?

42. Is the reaction endothermic or exothermic? Explain. Endothermic because energy of products is greater than energy of reactants

43. Will this reaction be hot or cold to the touch? Explain. Cold because energy from your hand is absorbed in the reaction