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(a) Study the standard electrode potentials for the half-cells given below and answer the questions that follow. (The letters do not represent the actual symbols of the elements.)

(i) Identify the strongest oxidizing agent. Give a reason for your answer.
(ii) Which two half-cells would produce the highest potential difference when combined?
(iii) Explain whether the reaction represented below can take place.
`2N^(+)(aq)+M(s)→2N(s)+M^(2+)(aq)`
(b)100 `cm^3` of 2M sulphuric (VI) acid was electrolyzed using the set-up
represented by the diagram below.

(i) Write an equation for the reaction that produces gas L.
(ii) Describe how gas K can be identified.
(iii)Explain the difference in:
I. The volume of the gases produced at the electrodes.
II. Brightness of the bulb if 100 cm3 of 2M ethanoic acid was used in place of sulphuric (VI) acid.