promotion image of download ymail app
Promoted
Emma asked in Science & MathematicsChemistry · 2 months ago

Electrochemistry problem?

A Cr (aq) solution is electrolyzed using a current of 13.5 A. What mass of Cr(s) is plated out after 3.00 days?

1 Answer

Relevance
  • 2 months ago
    Favorite Answer

    You didn't indicate the oxidation state of the chromium solution, but I am going to assume that it is 3+. If it is different that, you will have to alter one calculation.

    Coulomb = 13.5 A X (3.00 day) X (24 hr/day) X (60 min/hr) X (60 s/min) = 3.50X10^6 Coulomb

    Moles of electrons = 3.50X10^6 C /96485 C/mole e- = 36.3 mol e-

    Moles Cr = 36.3 mol e- / 3 mol e- / mol Cr = 12.1 mol Cr X 52.00 g/mol = 629 g Cr(s)

    • Commenter avatarLogin to reply the answers
Still have questions? Get your answers by asking now.