Problem: What mass of aluminum can be plated onto an object in 755 minutes at 5.80 A of current? Please do step by step and as clearly as possible.

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We’re being asked to calculate the mass of aluminum that can be plated onto an object in 755 minutes at 5.80 A of current. Aluminum is electroplated from a solution containing Al3+ ion.

Let’s first determine what happens to Ag+:

• Al(s) must be formed from Al3+(aq)
• Al3+ needs to gain 3 e- in order to become Al(s)

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What mass of aluminum can be plated onto an object in 755 minutes at 5.80 A of current? Please do step by step and as clearly as possible.

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