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A galvanic cell uses the following solutions:5 M Cr 2 (SO 4 ) 3 in 0.8 L of water and 0.8 M Au(NO 3 ) 3 in 1.2 L of water.

10.2. A galvanic cell uses the following solutions: 1.5 M Cr2(SO4)3 in 0.8 L of water and 0.8 M Au(NO3)3 in 1.2 L of water. Write the balanced chemical equations of the dissolution of Cr2(SO4)3and Au(NO3)3 into ions in water.

10.3. The galvanic cell includes solid bars of gold (Au) and chromium (Cr). Using your answer in Problem 10.2 and the table of standard reduction potentials write the following:

Oxidation half-reaction:

Reduction half reaction: 

Overall balanced reaction:

Voltage of the galvanic cell:

10.4. Recall that at the cathode, positive ions in solution are reduced into the solid form. The galvanic cell will stop working when all of the ions in solution are reduced to the solid form. For the galvanic cell in 10.2, identify the ion that is being reduced at the cathode and calculate the total number of moles of the ion in solution at the beginning of the reaction.


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