Chapter 8 – Review
8.1 Writing and Balancing Chemical Equations
- What does it mean to say an equation is balanced? Why is it important for an equation to be balanced? Check Answer: [1]
- Balance the following equations: Check Answer: [2]
- [latex]\text{PCl}_5(s) + \text{H}_2 \text{O}(l) \longrightarrow \text{POCl}_3(l) + \text{HCl}(aq)[/latex]
- [latex]\text{Cu}(s) + \text{HNO}_3(aq) \longrightarrow \text{Cu(NO}_3)_2(aq) + \text{H}_2 \text{O}(l) + \text{NO}(g)[/latex]
- [latex]\text{H}_2(g) + \text{I}_2(s) \longrightarrow \text{HI}(s)[/latex]
- [latex]\text{Fe}(s) + \text{O}_2(g) \longrightarrow \text{Fe}_2 \text{O}_3(s)[/latex]
- [latex]\text{Na}(s) + \text{H}_2 \text{O}(l) \longrightarrow \text{NaOH}(aq) + \text{H}_2(g)[/latex]
- [latex]\text{(NH}_4)_2 \text{Cr}_2\text{O}_7(s) \longrightarrow \text{Cr}_2\text{O}_3(s) + \text{N}_2(g) + \text{H}_2 \text{O}(g)[/latex]
- [latex]\text{P}_4(s) + \text{Cl}_2(g) \longrightarrow \text{PCl}_3(l)[/latex]
- [latex]\text{PtCl}_4(s) \longrightarrow \text{Pt}(s) + \text{Cl}_2(g)[/latex]
- Balance the following equations:
- [latex]\text{Ag}(s) + \text{H}_2 \text{S}(g) + \text{O}_2(g) \longrightarrow \text{Ag}_2 \text{S}(s) + \text{H}_2 \text{O}(l)[/latex]
- [latex]\text{P}_4(s) + \text{O}_2(g) \longrightarrow \text{P}_4 \text{O}_{10}(s)[/latex]
- [latex]\text{Pb}(s) + \text{H}_2 \text{O}(l) + \text{O}_2(g) \longrightarrow \text{Pb(OH)}_2(s)[/latex]
- [latex]\text{Fe}(s) + \text{H}_2 \text{O}(l) \longrightarrow \text{Fe}_3 \text{O}_4(s) + \text{H}_2(g)[/latex]
- [latex]\text{Sc}_2 \text{O}_3(s) + \text{SO}_3(l) \longrightarrow \text{Sc}_2 \text{(SO}_4)_3(s)[/latex]
- [latex]\text{Ca}_3 \text{(PO}_4)_2(aq) + \text{H}_3 \text{PO}_4(aq) \longrightarrow \text{Ca(H}_2 \text{PO}_4)_2(aq)[/latex]
- [latex]\text{Al}(s) + \text{H}_2 \text{SO}_4(aq) \longrightarrow \text{Al}_2 \text{(SO}_4)_3(s) + \text{H}_2(g)[/latex]
- [latex]\text{TiCl}_4(s) + \text{H}_2 \text{O}(g) \longrightarrow \text{TiO}_2(s) + \text{HCl}(g)[/latex]
- Write a balanced molecular equation describing each of the following chemical reactions. Check Answer: [3]
- Solid calcium carbonate is heated and decomposes to solid calcium oxide and carbon dioxide gas.
- Gaseous butane, C4H10, reacts with diatomic oxygen gas to yield gaseous carbon dioxide and water vapour.
- Aqueous solutions of magnesium chloride and sodium hydroxide react to produce solid magnesium hydroxide and aqueous sodium chloride.
- Water vapour reacts with sodium metal to produce solid sodium hydroxide and hydrogen gas.
- Write a balanced equation describing each of the following chemical reactions.
- Solid potassium chlorate, KClO3, decomposes to form solid potassium chloride and diatomic oxygen gas.
- Solid aluminum metal reacts with solid diatomic iodine to form solid Al2I6.
- When solid sodium chloride is added to aqueous sulfuric acid, hydrogen chloride gas and aqueous sodium sulfate are produced.
- Aqueous solutions of phosphoric acid and potassium hydroxide react to produce aque