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