15.17 g gold is produced when 16.9 A of current is passed through a gold solution for 22.0 min
Current passed = 16.9 A
Time = 22.0 mil
Mass of gold produced = ?
Write the ionic equation of the above-mentioned reaction.
Au³⁺ + 3e⁻ → Au
Convert time from minutes to seconds
Time in seconds = time in minutes × 60
Time in seconds = 22.0 × 60
Time in seconds = 1320 sec
Calculate the amount of charge
amount of charge = 16.9 coulomb/s x 1320 s
amount of charge = 22308 coulomb
amount of charge = 22308 / 96500
amount of charge = 0.231 faradays
Calculate the number of moles
number of moles = 0.231 / 3
number of moles = 0.077 mol Au
mass of Au = 0.077 mol × 196.967 g/mol
mass of Au = 15.17 g
You can also learn about ionic equations from the following question:
https://brainly.com/question/15467502
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