We’re being asked to calculate the mass of platinum plated on the electrode after 55s.
Pt2+(aq) + 2 e- → Pt(s)
We can now calculate the mass of Au(s) deposited.
Step 1: Calculate the total amount of current used (using current and time)
Step 2: Calculate the number of moles e- produced from the reaction (using Faraday’s constant)
Step 3: Calculate the mole of Pt(s) produced (using mol to mol comparison)
Step 4: Calculate the mass of Pt(s) produced (using molar mass)
What mass of platinum could be plated on an electrode from the electrolysis of a Pt(NO3)2 solution with a current of 0.500 A for 55.0 s?
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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 Electroplating concept. If you need more Electroplating practice, you can also practice Electroplating practice problems.