HIGHER CHEMISTRY REVISION.

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HIGHER CHEMISTRY REVISION.
Unit 3 - Redox Reactions
1. Although they are more expensive, fuel cells
have been developed as an alternative to
petrol for motor vehicles. (a) (i) The
ion-electron equations for the processes
occurring at each electrode are H2(g) ? 2H
(aq) 2e- O2 (g) 4H(aq)
4e- ? 2H2O(l) Combine these two
equations to give the overall redox equation.
(ii) On the diagram show by means of an arrow
the path of electron flow. (b) Give one
advantage that fuel cells have over petrol for
providing energy.
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2. Sodium sulphite is a salt of sulphurous
acid, a weak acid. Identify the two
statements which can be applied to sodium
sulphite You may wish to refer to the
data booklet. A It can be prepared by a
precipitation reaction. B It can be prepared by
the reaction of sulphurous acid with sodium
carbonate. C In solution, the pH is lower than a
solution of sodium sulphate. D In redox
reactions in solution, the sulphite ion acts as
a reducing agent. E In redox reactions in
solution, the sodium ions are oxidised.
Statements in boxes A and D
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3. (a) Some carbon monoxide detectors contain
crystals of hydrated palladium(II) chloride.
These form palladium in a redox reaction if
exposed to carbon monoxide.
CO(g) PdCl2.2H2O(s) ? CO2 (g)
Pd(s) 2HCl(g) H2O(l) Write the
ion-electron equation for the reduction step in
this reaction. (b) Another type of
detector uses an electrochemical method to detect
carbon monoxide. At the positive
electrode. CO(g) H2O(l) ? CO2 (g)
2H(aq) 2e At the negative electrode O2
(g) 4H (aq) 4e ?
2H2O(l) Combine the two ion-electron equations
to give the overall redox equation.

1. Pd2 2e- ? Pd
2. 2CO O2 ? 2 CO2

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4. The glucose content of a soft drink can be
estimated by titration against a
standardised solution of Benedicts solution.
The copper(II) ions in Benedicts solution
react with glucose as shown. C6H12O6 (aq)
2Cu2(aq) 2H2O(l) ? Cu2O(s) 4H(aq)
C6H12O7(aq) (a) What change in the ratio
of atoms present indicates that the conversion of
glucose into a compound with molecular
formula (C6H12O7) is an example of
oxidation? (b) In one experiment, 25.0
cm3 volumes of a soft drink were titrated with
Benedicts solution in which the
concentration of copper(II) ions was
0.500 mol l-1. The following results were
obtained. Titration Volume of Benedicts
solution / cm3 1 18.0
2 17.1 3 17.3 Average volume of
Benedicts solution used 17.2 cm3. (i)
Why was the first titration result not used in
calculating the average volume of
Benedicts solution? (ii) Calculate the
concentration of glucose in the soft drink, in
mol l-1.
(a) The increase in the oxygen content
indicates oxidation. (b)(i) The first titration
result is a rough titration value and
is not an accurate titre. (ii) No of
moles C x V(litres)
0.5 x 0.0172 0.0086 From equation 1
mole of glucose reacts with 2 moles of copper(II)
ions. So No, of moles of glucose
0.0043. Concentration 0.0043/0.025
0.172 mol l-1.
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• 5. Vitamin C, C6H8O6, is a powerful reducing
  agent. The concentration of vitamin C in a
  solution
• can be found by titrating it with a
  standard solution of iodine, using starch as an
  indicator.
• The equation for the reaction is
• C6H8O6 (aq) I2(aq) ? C6H6O6
  (aq) 2H(aq) 2I(aq)
• Write an ion-electron equation for the reduction
  half-reaction.
• What colour change indicates that the end-point
  of the titration has been reached?
• (c) In one investigation, it was found that
  an average of 29.5 cm3 of 0.02 mol l-1 iodine
  solution was required to react completely with 25
  cm3 of vitamin C solution.
• Use this result to calculate the mass,
  in grams, of vitamin C present in the solution.

• I2 2e- ? 2I
• (b) A blue-black colour appears.
• No. of moles of iodine used C x V(litres)
• 0.02 x 29.5/1000
• 5.9 x 10-4 mol
• From equation 1 mole of vitamin C
  reacts with 1 mole of iodine
• So number of moles of vitamin C is 5.9
  x 10-4 mol.
• gfm of C6H8O6 176 g
• Mass no. of moles x gfm
• 5.9 x 10-4 x 176
• 0.104 g