1.
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When combining E° values, why don't we multiply by a factor as we do in Hess's law?
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2.
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Use standard reduction potentials to determine Keq for the process below. HNO2 (aq) + H+(aq) + e- ---> NO (g) + H2O(l) E = 0.983
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3.
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Use electrochemical potentials to determine which of the following solutions can dissolve silver metal.
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4.
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Determine Ecell at 50°C for the cell that is diagrammed below. Cu(s)|Cu2+(aq,0.18 M) || BrO-(aq,0.25 M), pH = 10.00|Br2(l)|Pt(s)
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5.
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Electrochemical cells are used to determine the pH of a solution. What is the pH at the anode in the cell that is diagrammed below? The cell potential is 0.122 V, and the temperature is 25°C. Pt(s)|H2(g, 0.95 atm), pH = ?|| H+ (aq,1.0 M), H2(g, 0.95 atm)|Pt(s)
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6.
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Use appropriate electrochemical data to determine the Ksp of AgI at 25°C.
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7.
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What current is required to plate out 0.500 g of chromium from a solution containing chromium(III) ion in 1.00 hour?
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8.
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Two copper electrodes are placed in 150.0 mL of a 0.100 M CuSO4(aq) solution. The solution is electrolyzed by a 0.100 A current for 75.0 min. What is the change in the Cu2+ concentration?
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9.
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1.25 L of a 0.925 M solution of CrCl3(aq) is electrolyzed with a current of 31.2 amperes for 25.0 minutes, and chromium plates out on the cathode. (a) What mass in grams of chlorine gas is produced? (b) What is the final concentration of CrCl3(aq) in moles/liter?
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10.
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Calculate the Ksp of lead iodide from the following standard electrode potentials at 25°. 2 e- + PbI2(s) <==> Pb(s) + 2 I-(aq), E° = -0.365 volts 2 e- + Pb2+(aq) <==> Pb(s), E° = -0.126 volts.
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