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

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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 XXXXXXXXXXV and the Pt | H2 | H+ half-cell is the cathode. Standard reduction potentials are given on the next page. (a) Draw a diagram of the electrochemical cell, labeling all electrodes and solutions. (b) What is the pH in the Pt | H+ | H2 half-cell? (c) What is the value of the equilibrium constant for the reaction occurring in this cell?

David · Accepted Answer

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.

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 XXXXXXXXXXV and the Pt | H2 | H+ half-cell...

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