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Q - Oxidation - Reduction

This document contains 9 questions about oxidation-reduction reactions. The questions cover identifying oxidizing and reducing agents, writing half reactions and overall redox equations, and determining oxidation states of elements in different compounds. Key concepts covered include oxidation number notation like (III), 3+, and +3 for iron, and oxidation-reduction reactions involving sulfur, iron, manganese, copper, chromium, and ethanol.

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Bisad Abu Curi
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100 views2 pages

Q - Oxidation - Reduction

This document contains 9 questions about oxidation-reduction reactions. The questions cover identifying oxidizing and reducing agents, writing half reactions and overall redox equations, and determining oxidation states of elements in different compounds. Key concepts covered include oxidation number notation like (III), 3+, and +3 for iron, and oxidation-reduction reactions involving sulfur, iron, manganese, copper, chromium, and ethanol.

Uploaded by

Bisad Abu Curi
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
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Download as PDF, TXT or read online on Scribd
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SL & HL Questions on Oxidation & reduction (1)

1. Give the oxidation state of sulfur in the reactants and products in the following reactions
and in each case state whether it has been oxidized or reduced:

i. H2S(g) + Cl2(g) → 2HCl(g) + S(s)

ii. Zn(s) + H2SO4(aq) → Zn2+(aq) + SO42–(aq) + H2(g)

iii. 2S2O32–(aq) + I2(aq) → S4O62–(aq) + 2I–(aq)

iv. 3SO32–(aq) + Cr2O72–(aq) + 8H+(aq) → 3SO42–(aq) + 2Cr3+(aq) + 4H2O(l)

2. Give the oxidation state of the transition metal in the following compounds:

i. [Fe(H2O)6]2+,

ii. [Fe(CN)6)]3–

iii. [Cu(NH3)4(H2O)2]2+

iv. [CuCl4]2–

3. Explain the difference between the use of (III), 3+ and +3 when applied to Fe.

4. State the name of the following compounds using the correct oxidation number:

i. Cu2SO4

ii. FeCl2

iii. Na2CO3

iv. Fe2O3

v. MnO2

© Dr Geoffrey Neuss, InThinking


http://www.thinkib.net/chemistry 1
5. When magnesium metal is placed in an aqueous solution of iron(II) ions, Fe2+(aq), the
magnesium dissolves and iron metal is precipitated. State the two half-equations and the
overall redox equation for the reaction taking place.

6. Bubbling sulfur dioxide gas, SO2(g) through an acidic solution of potassium


manganate(VII), KMnO4(aq), causes the colour of the solution to change from intense
purple to colourless as the manganate(VII) ion, MnO4– is reduced to manganese(II) ions,
Mn2+(aq). The two half-equations for the reactions taking place are:

MnO4–(aq) + 8H+(aq) + 5e– → Mn2+(aq) + 4H2O(l) and

SO32–(aq) + H2O(l) → SO42–(aq) + 2H+(aq) + 2e–

i. Identify the oxidizing agent present.

ii. Deduce the overall equation for the redox reaction.

7. Identify the oxidizing agent in each case and state the equation for the reaction that
occurs when:

i. chlorine gas is bubbled through an aqueous solution of potassium bromide.

ii. bromine water is added to an aqueous solution of potassium iodide.

8. Identify the oxidizing agent and the reducing reagent in the following reactions:

i. Cu(s) + 4HNO3(aq) → Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)

ii. 5H2O2(l) + 2MnO4- + 6H+(aq) → 2Mn2+(aq) + 5O2(g) + 8H2O(l)

iii. H2O2(l) + 2Fe2+(aq) + 2H+(aq) → 2Fe3+(aq) + 2H2O(l)

9. Ethanol, CH3CH2OH, can be oxidized to ethanal, CH3CHO, using an acidified solution of


dichromate(VI) ions, Cr2O72–(aq). During the process the orange solution turns green due
to the formation of chromium(III) ions, Cr3+(aq). Deduce the two half-equations and the
overall equation for the redox reaction that occurs.

© Dr Geoffrey Neuss, InThinking


http://www.thinkib.net/chemistry 2

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