Chromium often is electroplated on other metals and even plastics to produce a shiny metallic appearance. How many grams of chromium would plate out from a solution of Cr(NO₃)₃ when 10 amps of current are passed through the electrolytic cell for 5.36 hours?

Question

Quizplus · Accepted Answer

The mass of chromium can be calculated using the formula: mass = (It/nF) * M, where I is the current (10 A), t is the time in seconds (5.36 hours = 19296 seconds), n is the number of electrons transferred per atom of chromium (3 for Cr^3+), F is Faraday's constant (96485 C/mol), and M is the molar mass of chromium (51.996 g/mol). Plugging in these values gives approximately 34.7 g.

Chromium Often Is Electroplated on Other Metals and Even Plastics