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DP IB Chemistry: SL

Topic Questions

Home / IB / Chemistry: SL / DP / Topic Questions / 9. Redox Processes / 9.1 Redox Processes / Structured Questions: Paper 2


9.1 Redox Processes

Question 1a

Marks: 3
a)
Chlorine reacts with water to form chlorine water via the following equation.

Cl2 + H2O → HOCl + HCl

   State the oxidation number of chlorine in the following species

   Cl2 …………………..

   HOCl ………………….

   HCl …………………..

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    Question 1b

    Marks: 1
    b)
    Chlorine is an oxidising agent.
    Define oxidising agent in terms of electrons. 

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      Question 1c

      Marks: 2
      c)
      Nitrogen monoxide, NO, is formed when silver metal reduces nitrate ions, NO3- , ions in an acidic solution. State the oxidation numbers of nitrogen in NO and NO3-

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        Question 1d

        Marks: 1
        d)
        State the half equation for the formation of silver ions, Ag+ (aq), from silver metal.

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          Key Concepts
          Half equations

          Question 2a

          Marks: 6
          a)
          Deduce the oxidation numbers of of the elements in the following species.
          S2- …………………
          Sn2+ …………………
          V3+ …………………
          Si …………………
          Sb3+ …………………
          H- …………………
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            Question 2b

            Marks: 3
            b)
            Oxidation states are sometimes visible in the names of chemicals. Deduce the oxidation numbers of the stated elements in the following species.

            Copper in copper(I) oxide ………………..
            Iron in iron(III) oxide ………………..
            Phosphorus(V) oxide …………………
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              Question 2c

              Marks: 2
              c)

              The dichromate(VI) ion, Cr2O72- (aq) , reacts with sulfite ions, SO32- (aq), as follows.


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

              i)
              State whether the sulfite ions, SO32- (aq), are acting as an oxidising or reducing agent.
              ii)
              Justify your answer to part (i).
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                Question 2d

                Marks: 3
                d)
                Redox reactions can be identified by either reduction and oxidation occurring or the presence of a reducing agent and an oxidising agent.
                i)
                Deduce if the reaction between hydrochloric acid and sodium hydroxide is a redox reaction.

                HCl + NaOH → NaCl + H2O
                ii)
                Justify your answer.
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                  Question 3a

                  Marks: 1
                  a)
                  An iron tablet, weighing 1.35 g was dissolved in dilute sulfuric acid. The sample was dissolved in sulfuric acid to oxidise all of the iron to Fe2+ ions.

                  The solution is then titrated with 0.02 mol dm-3 potassium dichromate, K2Cr2O7, producing Fe3+ and Cr3+ ions in acidic solution. The titration requires 31.00 cm3 of K2Cr2O7 for 1.35 g of the sample.

                  Balance the following half equations:

                  Fe2+ (aq) → Fe3+ (aq) + ………

                  Cr2O72-(aq) + 14H(aq) + ……… → …….Cr3+ (aq) + …...H2O (l)
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                    Key Concepts
                    Half equations

                    Question 3b

                    Marks: 2
                    b)
                    The overall equation for the reaction in part (a) is as follows.

                    6Fe2+ (aq) + Cr2O72- (aq) + 14H+ (aq) → 6Fe3+ (aq) + 2Cr3+ (aq) + 7H2O (l)

                    i)
                    Using the information in part (a), calulate the number of moles of potassium dichromate, K2Cr2O7 used.
                    ii)
                    Use your answer to part (b) (i) to determine the number of moles of Fe2+ in the sample.
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                      Key Concepts
                      Redox Titrations

                      Question 3c

                      Marks: 2
                      c)
                      Using the information in part (a) calculate the mass, in grams, of iron in the original sample.
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                        Key Concepts
                        Redox Titrations

                        Question 3d

                        Marks: 1
                        d)
                        Using the information in part (a) and your answer to part (c) calculate the percentage of iron in the original 1.35 g iron tablet.
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                          Key Concepts
                          Redox Titrations

                          Question 4a

                          Marks: 2
                          a)
                          Zinc metal will react with copper sulfate solution. State the equation for this reaction.

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                            Key Concepts
                            The activity series

                            Question 4b

                            Marks: 1
                            b)
                            Predict the products, if any, of the reaction between lead(IV) oxide and zinc.

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                              Question 4c

                              Marks: 5
                              c)
                              A voltaic cell is made from a half-cell containing a zinc electrode in a solution of zinc nitrate and a half-cell containing a silver electrode in a solution of silver nitrate. Using section 25 in the data booklet, label the following diagram.


                              9-1-ib-sl-sq-easy-voltaic-cell-q4c

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                                Key Concepts
                                Voltaic cells

                                Question 4d

                                Marks: 3
                                d)
                                State three differences between a voltaic cell and an electrolytic cells. 

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                                  Question 5a

                                  Marks: 1
                                  a)
                                  A 500 cm3 sample of lake water was analysed using the Winkler Method. 0.0600 mol dm-3 sodium thiosulfate solution, Na2S2O(aq), was titrated against liberated iodine. It was determined that the average titre of Na2S2Owas 19.30 cm3.
                                  Calculate the amount, in moles, of sodium thiosulfate used in the titration. 

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                                    Question 5b

                                    Marks: 1
                                    b)
                                    In the Winkler method 1 mol of O2 is equivalent to 4 mol of Na2S2O3 Deduce the amount, in moles, of oxygen that has reacted.

                                    [1]

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                                      Question 5c

                                      Marks: 2
                                      c)
                                      Use your answer to part (b) and section 6 in your data booklet to calculate the following

                                      • The concentration, in mol dm-3, of oxygen in the water ………………..
                                      • The concentration, in g dm-3, of oxygen in the water …………………

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                                        Question 5d

                                        Marks: 3
                                        d)
                                        Define the biological oxygen demand (BOD).

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                                          Key Concepts
                                          The Winkler Method