19 4.3 Classes of Chemical Reactions: Single and Double Displacement Reactions

Practice questions

1. 1. 1. 1. What are the general characteristics that help you recognise single-replacement reactions?
            1. 1. Only cations are swapped.
               2. One element replaces another element in a compound.
               3. Only anions are swapped.
               4. Parts of two ionic compounds are exchanged, making two new compounds.
         2. What are the general characteristics that help you recognise double-replacement reactions?
            1. 1. The exchange of the cations or the anions of two ionic compounds, making two new compounds.
               2. They can occur between any given reactants.
               3. The generation of a new element and a compound.
               4. One element replaces another element in a compound.
         3. Assuming that the following single-replacement reaction occurs, predict the products of the reaction: [latex]\ce{Zn + Fe{(NO_{3})}_{2} {\rightarrow} ?}[/latex]
            1. 1. [latex]\ce{Zn + Fe + NO_{2}}[/latex]
               2. [latex]\ce{FeZn + N_{2}}[/latex]
               3. [latex]\ce{Zn + Fe{(NO_{3})}}[/latex]
               4. [latex]\ce{Zn{(NO_{3})}_{2} + Fe}[/latex]
         4. Assuming that the following single-replacement reaction occurs, predict the products of the reaction: [latex]\ce{Li + MgSO_{4} {\rightarrow} ?}[/latex]
            1. 1. [latex]\ce{LiSO_{4}}[/latex] and [latex]\ce{MgSO_{4}}[/latex]
               2. [latex]\ce{Li}[/latex] and [latex]\ce{Mg}[/latex]
               3. [latex]\ce{Li_{2}SO_{4}}[/latex] and [latex]\ce{Mg}[/latex]
               4. [latex]\ce{MgSO_{4}}[/latex] and [latex]\ce{Li}[/latex]
         5. Assuming that the following single-replacement reaction occurs, predict the products and write the balanced chemical equation: [latex]\ce{F_{2} + FeI_{3} {\rightarrow} ?}[/latex]
            1. 1. [latex]\ce{3F_{2} + 2FeI_{3} {\rightarrow} 3F_{2} + 2FeF_{3}}[/latex]
               2. [latex]\ce{3F_{2} + 2FeI_{3} {\rightarrow} 3I_{2} + 2FeF_{3}}[/latex]
               3. [latex]\ce{F_{2} + 2FeI_{3} {\rightarrow} 3I_{2} + 2FeF_{3}}[/latex]
               4. [latex]\ce{3F_{2} + 2FeI_{3} {\rightarrow} 3I_{2} + 2Fe + F_{2}}[/latex]
         6. Assuming that the following single-replacement reaction occurs, predict the products and write a balanced chemical equation: [latex]\ce{Al + NiBr_{2} {\rightarrow} ?}[/latex]
         7. Decide whether the following statement is correct regarding the single-replacement reaction between [latex]\ce{Sn}[/latex] and [latex]\ce{H_{2}SO_{4}}[/latex].  [latex]\ce{Sn}[/latex] reacts with [latex]\ce{H_{2}SO_{4}}[/latex] to produce [latex]\ce{SnSO_{4}}[/latex] and [latex]\ce{H_{2}}[/latex]. The balanced chemical equation for this reaction is [latex]\ce{Sn + H_{2}SO_{4} {\rightarrow} SnSO_{4} + H_{2}}[/latex].
         8. Use the periodic table or the activity series to predict if the following single-replacement reaction will occur and, if so, what is the balanced chemical equation? [latex]\ce{FeCl_{2} + Br_{2} {\rightarrow} ?}[/latex].
         9. Use the periodic table or the activity series to predict if the following single-replacement reaction will occur and, if so, what is the balanced chemical equation? [latex]\ce{Fe{(NO_{3})}_{3} + Al {\rightarrow} ?}[/latex]
            1. 1. [latex]\ce{3Fe{(NO_{3})}_{3} + 2Al {\rightarrow} 2Al{(NO_{3})}_{3} + 3Fe}[/latex]
               2. [latex]\ce{Fe{(NO_{3})}_{3} + Al {\rightarrow} Al{(NO_{3})}_{3} + Fe}[/latex]
               3. [latex]\ce{Fe{(NO_{3})}_{3} + Al {\rightarrow} Al + Fe}[/latex]
               4. No reaction occurs
         10. Assuming that the following double-replacement reaction occurs, predict the products and write the balanced chemical equation: [latex]\ce{Zn{(NO_{3})}_{2} + NaOH {\rightarrow} ?}[/latex]
             1. 1. [latex]\ce{Zn{(NO_{3})}_{2} + NaOH {\rightarrow} Zn{(OH_{2})} + NaNO_{3}}[/latex]
                2. [latex]\ce{Zn{(NO_{3})}_{2} + 2NaOH {\rightarrow} Zn{(OH_{2})} + 2NaNO_{3}}[/latex]
                3. [latex]\ce{Zn{(NO_{3})}_{2} + 2NaOH {\rightarrow} Zn{(OH_{2})} + 2Na}[/latex]
                4. [latex]\ce{Zn{(NO_{3})}_{2} + 2NaOH {\rightarrow} Zn +2NaNO_{3}}[/latex]
         11. Assuming that the following double-replacement reaction occurs, predict the products and write each balanced chemical equation: [latex]\ce{HCl + Na_{2}S {\rightarrow} ?}[/latex]
             1. 1. [latex]\ce{2HCl + Na_{2}S {\rightarrow} 2NaCl + H_{2}S}[/latex]
                2. [latex]\ce{2HCl + Na_{2}S {\rightarrow} 2NaCl + H_{2}}[/latex]
                3. [latex]\ce{2HCl + Na_{2}S {\rightarrow} 2NaH + Cl_{2}}[/latex]
                4. [latex]\ce{HCl + Na_{2}S {\rightarrow} 2NaCl + H_{2}S}[/latex]
         12. Assuming that each double-replacement reaction occurs, predict the products and write the balanced chemical equation: [latex]\ce{Pb{(NO_{3})}_{2} + 2KBr {\rightarrow}}[/latex] ………. [latex]\ce{+ 2}[/latex] ………. .
         13. Assuming that the following double-replacement reaction occurs, predict the products and write the balanced chemical equation: [latex]\ce{K_{2}O + MgCO_{3} {\rightarrow} ?}[/latex]
         14. Use the solubility rules to predict if the following double-replacement reaction will occur and, if so, what is the balanced chemical equation? [latex]\ce{K_{3}PO_{4} + SrCl_{2} {\rightarrow} ?}[/latex]
             1. 1. [latex]\ce{2K_{3}PO_{4} + 3SrCl_{2} {\rightarrow} Sr_{3}{(PO_{4})}_{2} {(s)} + 6KCl}[/latex]
                2. [latex]\ce{K_{3}PO_{4} + SrCl_{2} {\rightarrow} Sr_{3}{(PO_{4})}_{2} {(s)} + KCl}[/latex]
                3. No reaction occurs.
                4. [latex]\ce{2K_{3}PO_{4} + 3SrCl_{2} {\rightarrow} Sr {(s)} + 6KCl}[/latex]
         15. Use the solubility rules to predict if the following double-replacement reaction will occur and, if so, what is the balanced chemical equation? [latex]\ce{CaCO_{3} + MgCl_{2} {\rightarrow} ?}[/latex]
             1. 1. [latex]\ce{CaCO_{3} + MgCl_{2} {\rightarrow} CaCl_{2} + Mg}[/latex]
                2. [latex]\ce{CaCO_{3} + 2MgCl_{2} {\rightarrow} CaCl_{2} + 2MgCO_{3}}[/latex]
                3. [latex]\ce{CaCO_{3} + MgCl_{2} {\rightarrow} CaCl_{2} + MgCO_{3}}[/latex]
                4. No reaction occurs
         16. Decide whether the following statement is true. [latex]\ce{Na_{2}CO_{3}}[/latex] is soluble in water. Hint: use solubility rules to predict.
         17. Decide whether the following statement is true. [latex]\ce{CaCl_{2}}[/latex] is soluble in water. Hint: use solubility rules to predict.
         18. A precipitation reaction will occur when an aqueous solution of [latex]\ce{AgNO_{3}}[/latex] reacts with an aqueous solution of [latex]\ce{Na_{2}CO_{3}}[/latex].

Answers

1. 1. b
   2. a
   3. d
   4. c
   5. b
   6. [latex]\ce{2Al + 3NiBr_{2} {\rightarrow} 2AlBr_{3} + 3Ni}[/latex]
   7. True
   8. b
   9. c
   10. b
   11. a
   12. [latex]\ce{Pb{(NO_{3})}_{2} + 2KBr {\rightarrow} PbBr_{2} + 2KNO_{2}}[/latex]
   13. [latex]\ce{K_{2}O + MgCO_{3} {\rightarrow} K_{2}CO_{3} + MgO}[/latex]
   14. a
   15. d
   16. True
   17. True
   18. True