Problem: Three electrolytic cells are connected in a series. The electrolytes in the cells are aqueous copper(II) sulfate, gold(III) sulfate, and silver nitrate. A current of 2.36 A is applied and after some time 1.74 g Cu is deposited. What mass of gold was deposited?

FREE Expert Solution

Step 1: Calculate moles of Cu produced (using the mole of e- from the reaction)

Step 2: Perform mole to mole comparison (1 Au: 3 Cu)
Step 3: Calculate the mass of Au produced (using the molar mass of Au)

We will perform the calculation in one equation:

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Problem Details

Three electrolytic cells are connected in a series. The electrolytes in the cells are aqueous copper(II) sulfate, gold(III) sulfate, and silver nitrate. A current of 2.36 A is applied and after some time 1.74 g Cu is deposited. What mass of gold was deposited?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Faraday's Constant concept. You can view video lessons to learn Faraday's Constant. Or if you need more Faraday's Constant practice, you can also practice Faraday's Constant practice problems.

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Based on our data, we think this problem is relevant for Professor Yang's class at UH.