Anonymous
Anonymous asked in Science & MathematicsChemistry · 3 weeks ago

In the electrolysis of Ag (from Ag+)depositing on the cathode, using a current of 1.12 A for 2.40 hours, what mass of silver will form?

In the electrolysis of Ag (from Ag+)depositing on the cathode, using a current of 1.12 A for 2.40 hours, what mass of silver will form?

Answer in g. 

Need help setting up/ solving thank you

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  • 3 weeks ago

    (1.12 A) x (2.40 hours x 3600 sec/hour) = 9676.8 C

    (9676.8 C) / (96485.3399 C/mol e{-}) = 0.10029 mol e{-}

    Ag{+} + e{-} → Ag

    (0.10029 mol e{-}) x (1 mol Ag / 1 mol e{-}) x (107.8682 g Ag/mol) = 10.8 g Ag

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