Simultaneous Redox Reactions
15 Questions · 38 Total Marks · Oxidation & Reduction Occurring Together
What does the term 'redox' stand for?
In a redox reaction, what happens to a substance that is oxidised in terms of electrons?
In a redox reaction, what happens to the oxidation number of a substance that is reduced?
Define the term 'oxidising agent'.
Define the term 'reducing agent'.
Explain the term 'redox reaction'.
Explain, in terms of electrons, why the following reaction is a redox reaction: Mg + CuSO₄ → MgSO₄ + Cu
Explain why it is impossible to have oxidation without reduction occurring at the same time.
Define oxidation and reduction in terms of oxidation numbers.
State what is meant by a 'displacement reaction' and explain why all displacement reactions are also redox reactions.
ZnO + C → Zn + CO Identify (i) the substance oxidised and (ii) the substance reduced. Explain your reasoning in terms of electrons or oxidation numbers.
Fe₂O₃ + 3CO → 2Fe + 3CO₂ This reaction occurs in a blast furnace. Identify (i) the oxidising agent and (ii) the reducing agent.
Cl₂ + 2KBr → 2KCl + Br₂ (a) Identify the substance oxidised and the substance reduced. (b) State the oxidation number change for each.
2Mg + O₂ → 2MgO (a) Write the ionic half-equation for the oxidation of magnesium. (b) Write the ionic half-equation for the reduction of oxygen. (c) What is the oxidising agent?
The following is a disproportionation reaction — a special type of redox where the SAME element is both oxidised and reduced: Cl₂ + 2NaOH → NaCl + NaClO + H₂O (a) What is the oxidation number of chlorine in: Cl₂, NaCl, and NaClO? (b) Explain why this is a simultaneous redox reaction.
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