AQA Jun 2017 Paper 1 Q10

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21Table 4 shows some electrode half-equations and their standard electrode potentials. Table 4 Electrode half-equation Cl2(g) + 2e2Cl (aq) NO3 (aq) + 4H+(aq) + 3eNO(aq) + 2H2O(aq) Fe3+(aq) + e Fe3+(aq) Cu2+(aq) + 2eCu(s) SO4 2(aq) + 4H+(aq) + 2eSO2(g) + 2H2O(aq) 2H+(aq) + 2eH2(g) Fe2+(aq) + 2eFe(s) Deduce the oxidation state of nitrogen in NO3and in NONitrogen in NO3 Nitrogen in NO State the weakest reducing agent in Table 4. E / V +1.36 +0.96 +0.77 +0.34 +0.17 0.00 0.44 [2 marks] [1 mark] 1 0 1 0 . 1 1 0 . 2 1 0 . 3 Write the conventional representation of the cell that has an EMF of +0.43 V [2 marks] *21* Turn overIB/M/Jun17/7405/1<br /> 221 0 . 4 Use data from Table 4 to identify an acid that will oxidise copper. Explain your choice of acid. Use these data to suggest a possible equation for the reaction. Calculate the EMF of the cell that has the same overall reaction. [4 marks] *22* IB/M/Jun17/7405/1<br />

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