a. Write two half-equations for the reactions that take place when Fe2+(aq) is oxidised by dichromate(VI) ions.
b. Combine the two half-equations and write the equation for the oxidation of Fe2+(aq) by dichromate(VI) ions.
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c. Work out the Eθvalue of the cell made when the two half-cells in part a are connected and the reaction in part b takes place. Explain what this value predicts about the likelihood of Fe2+(aq) being oxidised by dichromate(VI) ions.
d. How many moles of Fe2+(aq) can 1 mole of dichromate(VI) oxidise?
e. In a titration, 25.0 cm3 of an solution containing Fe2+(aq) ions was completely oxidised by 15.30 cm3 of 0.00100 mol dm–3 potassium dichromate(VI) solution.
i. How many moles of potassium dichromate(VI) are there in 15.30 cm3 of 0.00 100 mol dm–3 solution?
ii. How many moles of Fe2+ were present in the 25.0 cm3 of solution?
iii. What was the concentration of the Fe2+(aq) in the flask at the start of the titration?