1)The half-cell, Tl | Tl+(1 mol L?1), is connected to a Pt | H+ | H2(1 atm) half

Question

1)The half-cell, Tl | Tl+(1 mol L?1), is connected to a Pt | H+ | H2(1 atm) half-cell in which the concentration of H+ is unknown. The measured cell voltage is 0.0841 V and the Pt | H2 | H+ half-cell is the cathode. Standard reduction potentials are given on the next page. (1A) Draw a diagram of the electrochemical cell, labeling all electrodes and solutions. (1B) What is the pH in the Pt | H+ | H2 half-cell? (1C) (3 marks) What is the value of the equilibrium constant for the reaction occurring in this cell?

Explanation / Answer

E=0.0841-(RT/nF)*ln(K),,,,,,,,,,K=equilibrium constant=17.1

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