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chemistry unit 3
3.2 - redox reactions
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Cards (22)
What is the half equation for acidified manganate(VII) ions?
MnO4–
(aq) + 8H+(aq) +
5e–
⇌
Mn2+
(aq) + 4H2O(l)
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What colour change occurs with acidified manganate(VII) ions?
Purple to
colourless
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What is the half equation for acidified dichromate ions?
Cr2O7
2–(aq) + 14H+(aq) + 6e– ⇌ 2Cr3+(aq) + 7H2O(l)
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What colour change occurs with acidified dichromate ions?
Orange
to
green
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What is the half equation for iodine to iodide ions?
I2
(aq) + 2e– ⇌ 2I–(aq)
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What colour change occurs when iodine is reduced to iodide ions?
Brown
to
colourless
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What is the half equation for thiosulfate ions?
2S2O3
2–
(
aq
) ⇌ S4O6
2–
(
aq
) + 2e–
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What is the process involving aqueous dichromate ions and iron(II) ions?
Cr2O7 2–
(aq) oxidises
Fe2+
(aq)
Requires an indicator
Reaction: Cr2O7 2– + 14H+ + 6Fe2+ ⇌ 2Cr3+ + 7H2O + 6Fe3+
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Why is the interconversion of dichromate and chromate ions not considered redox?
Chromium does not change its
oxidation number
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What is the colour change when dichromate ions convert to chromate ions?
Orange
to
yellow
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What is the process involving aqueous thiosulfate ions and iodine?
S2O3 2– oxidised by
I2
S2O3 2– in burette, I2 in flask
Colour fades to pale-yellow, then starch added
End point: blue colour decolourised
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What is the reaction between iodide ions and copper(II) ions?
2Cu2+
(aq) +
4I–
(aq) →
2CuI(s)
+
I2(aq)
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What happens to the blue solution when iodide ions react with copper(II) ions?
It loses its colour, forming a white
precipitate
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What is the procedure for standardising potassium manganate(VII) solution?
Titrated with
iron(II) ammonium sulfate
MnO4–
in burette,
Fe2+
in flask
Excess sulfuric acid added
No indicator needed; pink colour indicates endpoint
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What is the half equation for iron(II) ions oxidising to iron(III) ions?
Fe2+
(aq) ⇌
Fe3+
(aq) + e–
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What is the overall ionic equation combining half equations for Fe2+ and MnO4–?
MnO4–
+
8H+
+
5Fe2+
⇌
Mn2+
+
4H2O
+
5Fe3+
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How do you calculate the concentration of KMnO4 solution in mol dm–3?
Use
moles of Fe2+
and
titration volume
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What is the molar mass of FeSO4.7H2O?
278.0
g/mol
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How many moles of FeSO4.7H2O are in 25.00 g?
0.08933
0.08933
0.08933
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What is the concentration of Fe2+ ions in the solution?
0.08993
mol dm
−
3
0.08993 \text{ mol dm}^{-3}
0.08993
mol dm
−
3
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How many moles of MnO4– are in 25.55 cm3?
4.496
×
1
0
−
4
4.496 \times 10^{-4}
4.496
×
1
0
−
4
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What is the concentration of the KMnO4 solution?
0.0176
mol dm
−
3
0.0176 \text{ mol dm}^{-3}
0.0176
mol dm
−
3
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