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WorksheetsYear 12 Chemistry Chapter 4
Total questions: 10
Worksheet time: 10mins
Which one of the following redox equations has not been balanced correctly?
Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq)
Fe2+(aq) + Zn(s) → Fe(s) + Zn2+(aq)
Ag+(aq) + Cu(s) → Ag(s) + Cu2+(aq)
Zn2+(aq) + Mg(s) → Zn(s) + Mg2+(aq)
Nickel metal reacts with copper (II) ions according to the following equation:
Cu2+(aq) + Ni(s) → Cu(s) + Ni2+(aq)
Which one of the following statements about this reaction is correct?
Ni(s) is oxidised and Cu2+(aq) is the oxidising agent
Ni(s) is reduced and Cu2+(aq) is the oxidising agent
Ni(s) is oxidised and Cu2+(aq) is the reducing agent
Ni(s) is reduced and Cu2+(aq) is the reducing agent
Which one of the following is not a redox reaction?
Zn(s) + Cl2(g) → ZnCl2(s)
Mg(s) + O2(g) → MgO(s)
Pb2+(aq) + 2I-(aq) → PbI2(s)
Ni(s) + Cu2+(aq) → Ni2+(aq) + Cu(s)
Which of the following directly identifies the oxidant and reductant in the corrosion process shown in the given equation?
2𝐹𝑒(𝑠)+ 𝑂2(𝑔)+𝐻2𝑂 (𝑙)→ 2𝐹𝑒2+(𝑎𝑞)+4𝑂𝐻−(𝑎𝑞)
oxidant: O2
reductant: H2O
oxidant: O2
reductant: Fe
oxidant: H2O
reductant: H2O
oxidant: H2O
reductant: Fe
Consider the following particles:
𝑀𝑛𝑂4− 𝐾2𝐶𝑟2𝑂7 𝐶𝐻4 𝑁3−
The oxidation numbers of the respective elements are:
Mn Cr C N
+8 +6 -4 -3
Mn Cr C N
+8 +12 -4 -3
Mn Cr C N
+7 +6 -4 -3
Mn Cr C N
+7 +6 +4 -3
Magnesium reacts with nickel (II) ions according to the following equation:
𝑁𝑖2+(𝑎𝑞)+𝑀𝑔(𝑠)→ 𝑁𝑖(𝑠)+ 𝑀𝑔2+(𝑎𝑞)
Which one of the following is the correct set of conjugate redox pairs for this reaction?
𝑀𝑔2+(𝑎𝑞)/𝑀𝑔(𝑠) 𝑎𝑛𝑑 𝑁𝑖2+(𝑎𝑞)/𝑁𝑖(𝑠)
𝑁𝑖(𝑠)/ 𝑀𝑔2+(𝑎𝑞) and 𝑁𝑖2+(𝑎𝑞)/𝑀𝑔(𝑠)
𝑀𝑔(𝑠)/𝑁𝑖(𝑠) and 𝑁𝑖2+(𝑎𝑞)/𝑀𝑔2+(𝑎𝑞)
𝑀𝑔(𝑠)/𝑁𝑖2+(𝑎𝑞)and 𝑁𝑖(𝑠)/𝑀𝑔2+(𝑎𝑞)
Which one of the following is not a redox reaction?
2𝐹𝑒3+(𝑎𝑞)+𝑆𝑛2+(𝑎𝑞) → 2𝐹𝑒2+(𝑎𝑞)+𝑆𝑛4+(𝑎𝑞)
𝑀𝑔(𝑠)+𝑂2 (𝑔) → 2𝑀𝑔𝑂(𝑠)
2𝑁𝑎(𝑠)+2𝐻2𝑂(𝑙) → 𝐻2(𝑔)+2𝑁𝑎𝑂𝐻(𝑎𝑞)
𝐴𝑔+(𝑎𝑞)+𝐶𝑙−(𝑎𝑞) → 𝐴𝑔𝐶𝑙(𝑠)
The equation for the redox reaction betweeen manganese dioxide and hydrochloric acid is:
𝑀𝑛𝑂2(𝑠)+ 4𝐻𝐶𝑙 (𝑎𝑞)→ 𝑀𝑛𝐶𝑙2(𝑎𝑞)+2𝐻2𝑂 (𝑙)+ 𝐶𝑙2 (𝑔)
The reduction half equation occurring is:
2𝐶𝑙−(𝑎𝑞) → 𝐶𝑙2(𝑔) + 2𝑒−
4𝐻+(𝑎𝑞) + 4𝑒− → 2𝐻2(𝑔)
𝑀𝑛𝑂2(𝑠) + 4𝐻𝐶𝑙 (𝑎𝑞) → 𝑀𝑛𝐶𝑙2(𝑎𝑞) + 2𝐻2𝑂(𝑙) + 2𝐶𝑙2(𝑔)
𝑀𝑛𝑂2(𝑠) + 4𝐻+ (𝑎𝑞) + 2𝑒− → 𝑀𝑛2+(𝑎𝑞) + 2𝐻2𝑂(𝑙)
Ethanol can be oxidised in acidic conditions to ethanoic acid. The half-equation for this reaction is:
𝐶2𝐻5𝑂(𝑎𝑞) + 𝐻2𝑂(𝑙) → 𝐶2𝐻4𝑂2(𝑎𝑞) + 3𝐻+(𝑎𝑞) + 4𝑒−
𝐶2𝐻6𝑂(𝑎𝑞) + 𝐻2𝑂(𝑙) + 4𝑒− → 𝐶2𝐻4𝑂2(𝑎𝑞) + 4𝐻+(𝑎𝑞)
𝐶2𝐻6𝑂(𝑎𝑞) + 𝐻2𝑂(𝑙) → 𝐶2𝐻4𝑂2(𝑎𝑞) + 4𝐻+(𝑎𝑞) + 4𝑒−
𝐶2𝐻6𝑂(𝑎𝑞) + OH-(aq) → 𝐶2𝐻4𝑂2(𝑎𝑞) + H2(𝑎𝑞) + 2𝑒−
Consider the following half equations sand the overall equation for the reaction between sodium metal and a solution of silver ions.
Ag+(aq) + e- → Ag(s)
Na(s) → Na+(aq) + e-
Ag+(aq) + Na(s) → Ag(s) + Na+(aq)
Which one of the following sets of statements correctly describes this redox reaction?
Na(s) is the oxidising agent, Ag+(aq) is the reducing agent, sodium metal is reduced
Na(s) is the reducing agent, Ag+(aq) is the oxidising agent, sodium metal is reduced.
Na+(aq) is the oxidising agent, Ag(s) is the reducing agent, sodium metal is oxidised
Na(s) is the reducing agent, Ag+(aq) is the oxidising agent, sodium metal is oxidised
