Electrochemistry Practice Problems

Electrochemistry Practice Problems - Label the parts of...

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1 Electrochemistry Practice Problems F = 96,500 coulombs • mole –1 R = 8.314 joules • mole –1 • K –1 1. Calculate E° and K for the following reactions: A) Mg (s) + Cl 2 (g) Mg 2+ + 2 Cl B) 5 MnO 2 (s) + 4 H + 3 Mn 2+ + 2 MnO 4 + 2H 2 O K RT nFE G ln 0 = = = RT nFE K 3 . 2 0 10 = = reactants products log n 0.059 E reactants products ln nF RT E E 10 0 0 cell
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2 C) I 2 (s) + 5Br 2 (aq) + 6H 2 O 2IO 3 + 10 Br + 12H + 2. Pt(s) Fe 3+ (0.1 M), Fe 2+ (0.01M) ⏐⏐ Cr 2 O 7 2- (0.01M), Cr 3+ (0.2M), H + (1.0M) Pt(s) A. Write an oxidation half reaction for the left electrode and a reduction half reaction for the right electrode. B. Write a balanced reaction for the cell reaction. C. Calculate E o for the cell. In which direction is the reaction spontaneous; left to right or right to left? D. Calculate the cell potential, taking into account the concentrations listed.
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3 3, A) Draw a diagram of the glass pH sensing electrode.
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Unformatted text preview: Label the parts of your drawing carefully. B) Write an equation which describes voltage as a function of pH for this electrode. C) Describe the cause of "alkaline error", and what effect it has on pH measurements. 4 4, A) Draw a diagram of the silver/silver chloride reference electrode. Label the parts of your drawing carefully. B) What is meant by a liquid junction potential? C) What salt shows the least tendency to cause a liquid junction potential, and why? 5 5. Using data from the table of reduction potentials, calculate the solubility product constant (K sp) for lead sulfate. 6 6. Calculate the cell potential for the following cell: Pt (s) H 2 (1 atm) acetate buffer (pH = 3.50) KCl (1.00 M) AgCl (s) Ag (s)...
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Electrochemistry Practice Problems - Label the parts of...

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