Electrochemical_Cells

PRELAB Electrochemical Cells NAME DATE SECTION PRELAB • 147 Standard Reduction Potential Half-Reaction E°, Volts Ca 2 + (aq) + 2 e – → Ca (s) – 2.87 Mn 2 + (aq) + 2 e – → Mn (s) – 1.18 Co 2 + (aq) + 2 e – → Co (s) – 0.28 2 H + (aq) + 2 e – → H 2 (g) – 0.00 Ag + (aq) + e – → Ag (s) + 0.80 Cl 2 (g) + 2 e – → 2Cl – (aq) + 1.36 Given the partial list of standard reduction potentials above, answer Questions 1–5. 1. Will calcium (Ca) spontaneously reduce silver ion (Ag + ) to silver (Ag)? Briefly explain your answer. If yes, what is E°?

148 • PRELAB CHEMISTRY 1225L 2. Will silver metal react spontaneously with HCl (aq) to produce H 2 (g)? Briefly explain. 3. What is the cell potential for the Mn/Mn 2 + ||Co 2 + /Co cell, based on the standard poten- tials given above? 4. Will the reaction between Ca 2 + and Cl – ions to form Ca metal and Cl 2 (g) be spontaneous? Briefly explain. 5. A student constructed a Mg/Mg 2 + ||Ag + /Ag cell and measured a cell potential of 3.17 volts. Calculate the reduction potential of the Mg/Mg 2 + half-reaction.

REPORT SHEET • 149 REPORT SHEET ElectrocSemical Cells NAME DATE SECTION Part I: Voltaic Cells A. Cell Potentials Using a Zn(s)/Zn 2 + (aq) Reference Electrode Voltage Redox Couple 1st Determination 2nd Determination Mean 1. Zn/Cu ____________ _____________ ___________ 2. Zn/Pb ____________ _____________ ___________ 3. Zn/Fe ____________ _____________ ___________ B. Cell Potentials without Using a Reference Electrode Voltage Redox Couple 1st Determination 2nd Determination Mean 1. Pb/Cu ____________ _____________ ___________ 2. Fe/Cu ____________ _____________ ___________ 3. Fe/Pb ____________ _____________ ___________