SCH3U / Quiz – Chemical Reactions /
Chemical Reactions / Name:

Part 1 – In Class

  1. All the following are clues that a chemical reaction has taken place except
  2. a color change
  3. a solid forms
  4. the reactant is smaller
  5. a flame occurs
  6. bubbles form
  1. How many of the following statements are true concerning chemical equations?

  1. Coefficients can be fractions.

  2. Subscripts can be fractions.

  3. Coefficients represent the relative masses of the reactants and/or products.
  4. Changing the subscripts to balance an equation can only be done once.
  5. Atoms are conserved when balancing chemical equations.

  1. 3
  2. 5
  3. 1
  4. 4
  5. 2

  1. Which metal reacts with hydrochloric acid but not with water?

  1. Barium
  2. Copper
  3. Sodium
  4. Silver
  5. Zinc

  1. Identify the solid product that forms when the following aqueous solutions are mixed: Na2CrO4(aq) + BaCl2(aq) -->

  1. BaCrO4
  2. Ba(CrO4)2
  3. NaCl
  4. No precipitate forms
  5. Na2Cl

  1. Determine the coefficient for O2 when the following equation is balanced in standard form (smallest whole number integers).

C4H10(g) + O2(g) --> CO2(g) + H2O(g)


  1. 4
  2. 13
  3. 20
  4. 10
  5. 8

  1. When the following equation is balanced using the smallest possible integers, what is the number in front of the underlined substance?

Mg(s) + HCl(aq) --> MgCl (aq) + H2(g)

  1. 2
  2. 4
  3. 1
  4. 3
  5. 5

  1. Complete and write the balanced molecular equation for the following: [K/U] (2)

An aqueous solution of magnesium chloride is added to an aqueous solution of silver nitrate.

  1. Several drops of sodium sulfate solution are added to a sample of water to test for contaminants. The possible contaminants in the water are sodium nitrate, calcium chloride and lead (II) acetate. [A]
  2. Which of these contaminants might be present if a precipitate formed? (1)
  1. Write the balanced chemical equation for the reaction that involves this contaminant. (2)
  1. Identify the errors in each equation, and then write the correct balanced chemical equation. [T/I]
  2. 2K(s) + H2O(aq)  K2O(aq) + H2(g) (2)
  1. 2LiCl(aq) + Pb(NO3)2(aq)  LiNO3(s) + PbCl2(aq)(2)
  1. The results of two laboratory tests are given below: [T/I]

CX + B  BX + C

A + CX  no reaction

Use these results to write an activity series for metals A, B, and C. (3)

  1. Describe a procedure for using a displacement reaction to produce a sample of the element copper. Explain your reasoning. [A] (3)
  1. Describe the process of neutralization in terms of the types of reactants used, the type of reaction that occurs, and the products that form. [C] (5)

Part 2 – Take Home

  1. Balance the following equations and classify each reaction as one of the types of reactions you have learned in class. [K/U] (13)
  1. C2H2 + O2  CO2 + H2O
  2. Mg + CuSO4  MgSO4 +Cu
  3. Na + O2  Na2O
  4. Fe(NO3)3 + MgS  Fe2S3 + Mg(NO3)2
  5. N2O  N2 + O2
  6. Sn(OH)4 + HBr  H2O + SnBr4
  7. Cl2 + KI  KCl + I2
  8. Ca + O2  CaO
  9. H2SO4 + NaOH  Na2SO4 + H2O
  10. Pb(NO3)2 + K2CrO4  PbCrO4 + KNO3
  11. C3H6OS2 + O2  CO2 + H2O + SO2
  12. Mg + HCl  H2 + MgCl2
  13. HI  H2 + I2
  1. Complete and balance the following reactions and classify each equation. If you predict that no reaction will occur, write N.R. [T/I] [22]
  1. HNO3(aq) + Sr(OH)2(aq)
  2. Zn + Ni(NO3)2 
  3. HI(aq) + K2CO3(aq) 
  4. AlCl3(aq)+ Na2CO3(aq)
  5. Al(s) + O2(g)
  6. Cl2(g)+ LiBr(aq) 
  7. Solid aluminum reacts with solid sulfur
  8. A piece of magnesium ribbon is dropped into nitric acid
  9. Aqueous ammonium hydroxide reacts with carbonic acid
  10. A solution of plumbic nitrate is added to a solution of sodium bromide
  11. Phosphoric acid + aqueous mercuric hydroxide
  12. Solid potassium chlorate is heated to produce solid potassium chloride and oxygen
  13. Sulfur is burned
  14. The product of m (above) is dissolved into water
  15. Aqueous solutions of lead (II) chlorate and ammonium sulfide react to form lead (II) sulfide and ammonium chlorate
  16. Potassium is burned
  17. The product of p (above) is dissolved into water
  18. Fluorine gas passes over solid cuprous chloride
  19. Solid magnesium sulfide is decomposed by heat.
  20. Aqueous solutions of ferric hyposulfite and cupric perchlorate are mixed.
  21. Calcium reacts with nitrogen gas to form a single product.
  22. Complete combustion of ethane (C2H6).