SCH3U / Quiz – Chemical Reactions /
Chemical Reactions / Name:
Part 1 – In Class
- All the following are clues that a chemical reaction has taken place except
- a color change
- a solid forms
- the reactant is smaller
- a flame occurs
- bubbles form
- How many of the following statements are true concerning chemical equations?
- Coefficients can be fractions.
- Subscripts can be fractions.
- Coefficients represent the relative masses of the reactants and/or products.
- Changing the subscripts to balance an equation can only be done once.
- Atoms are conserved when balancing chemical equations.
- Which metal reacts with hydrochloric acid but not with water?
- Identify the solid product that forms when the following aqueous solutions are mixed: Na2CrO4(aq) + BaCl2(aq) -->
- No precipitate forms
- 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)
- 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)
- 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.
- 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]
- Which of these contaminants might be present if a precipitate formed? (1)
- Write the balanced chemical equation for the reaction that involves this contaminant. (2)
- Identify the errors in each equation, and then write the correct balanced chemical equation. [T/I]
- 2K(s) + H2O(aq) K2O(aq) + H2(g) (2)
- 2LiCl(aq) + Pb(NO3)2(aq) LiNO3(s) + PbCl2(aq)(2)
- 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)
- Describe a procedure for using a displacement reaction to produce a sample of the element copper. Explain your reasoning. [A] (3)
- 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
- Balance the following equations and classify each reaction as one of the types of reactions you have learned in class. [K/U] (13)
- C2H2 + O2 CO2 + H2O
- Mg + CuSO4 MgSO4 +Cu
- Na + O2 Na2O
- Fe(NO3)3 + MgS Fe2S3 + Mg(NO3)2
- N2O N2 + O2
- Sn(OH)4 + HBr H2O + SnBr4
- Cl2 + KI KCl + I2
- Ca + O2 CaO
- H2SO4 + NaOH Na2SO4 + H2O
- Pb(NO3)2 + K2CrO4 PbCrO4 + KNO3
- C3H6OS2 + O2 CO2 + H2O + SO2
- Mg + HCl H2 + MgCl2
- HI H2 + I2
- Complete and balance the following reactions and classify each equation. If you predict that no reaction will occur, write N.R. [T/I] 
- HNO3(aq) + Sr(OH)2(aq)
- Zn + Ni(NO3)2
- HI(aq) + K2CO3(aq)
- AlCl3(aq)+ Na2CO3(aq)
- Al(s) + O2(g)
- Cl2(g)+ LiBr(aq)
- Solid aluminum reacts with solid sulfur
- A piece of magnesium ribbon is dropped into nitric acid
- Aqueous ammonium hydroxide reacts with carbonic acid
- A solution of plumbic nitrate is added to a solution of sodium bromide
- Phosphoric acid + aqueous mercuric hydroxide
- Solid potassium chlorate is heated to produce solid potassium chloride and oxygen
- Sulfur is burned
- The product of m (above) is dissolved into water
- Aqueous solutions of lead (II) chlorate and ammonium sulfide react to form lead (II) sulfide and ammonium chlorate
- Potassium is burned
- The product of p (above) is dissolved into water
- Fluorine gas passes over solid cuprous chloride
- Solid magnesium sulfide is decomposed by heat.
- Aqueous solutions of ferric hyposulfite and cupric perchlorate are mixed.
- Calcium reacts with nitrogen gas to form a single product.
- Complete combustion of ethane (C2H6).