REVIEW EXERCISES

General Review

Write a brief and clear answer to each question. Be sure to show your work.

Question 1

1. Balance the following chemical equations:

  1. Zn(s) + HCl(aq) → ZnCl2(aq) + H2(g)

  2. KClO3(s) → KCl(s) + O2(g)

  3. S8(s) + F2(g) → SF6(g)

  4. Fe(s) + O2(g) → Fe2O3(s)

Question 2

2. For each of the four equations in Exercise 1, name the type of reaction it represents.

Question 3

3. Using the same equations you balanced in Exercise 1, suppose that you start with 1 g of each reactant. Identify the limiting reactant and determine the mass of each product that can be made.

Question 4

4. Write a balanced chemical equation for these reactions:

  1. Calcium metal reacts with water to form calcium hydroxide and hydrogen gas.

  2. A solution of hydrochloric acid reacts with solid calcium bicarbonate to produce water, carbon dioxide, and calcium chloride.

Question 5

5. What is a neutralization reaction?

Question 6

6. Write out the complete and net ionic equations for reactions between these compounds in solution:

  1. magnesium nitrate and calcium chloride

  2. silver nitrate and potassium iodide

  3. sodium sulfate and barium chloride

Question 7

7. Does a precipitate form in any of the reactions from Exercise 6? Circle them.

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Question 8

8. Describe the steps you would follow to make a 1.0 M solution of silver nitrate.

Question 9

9. How many grams of solute are dissolved in a 500.0 mL sample of 0.50 M sodium sulfate?

Question 10

10. What is the pH of a solution with [H+] = 2.0 × 10−8? What is the [OH−] of the solution?

Question 11

11. This reaction is completed in a factory to create potassium phosphate:

____ H3PO4(aq) + ____ KOH(aq) → K3PO4(aq) + ____ H2O(l)

  1. What type of reaction is represented by the equation?

  2. Copy the equation and balance it.

  3. If you want to make 5.0 mol of potassium phosphate, how many moles of phosphoric acid, H3PO4, do you need?

  4. If 628.0 g of phosphoric acid are reacted with 1122.0 g of potassium hydroxide, what is the maximum amount of potassium phosphate that can be produced?

  5. Which is the limiting reactant in part d? How much (in moles and in grams) of the excess reactant is left over?

Question 12

12. The reaction shown here is completed by a chemical company to create phosphoric acid, H3PO4.

____ K3PO4(aq) + ____ H2SO4(aq) → ____ H3PO4(aq) + ____ K2SO3(aq)

  1. What type of reaction is represented by the equation?

  2. Copy the equation and balance it.

  3. How many moles of potassium phosphate, K3PO4, are required to produce 6 mol of phosphoric acid?

  4. How many moles of sulfuric acid, H2SO4, are required to produce 6 mol of phosphoric acid?

  5. If 750.0 g of potassium phosphate are reacted with 0.75 L of 18.4 M sulfuric acid, what is the maximum number of moles of phosphoric acid that can be produced?

  6. Which is the limiting reactant in part e? How much (in moles and in grams) of the excess reactant is left over?