Electrolysis and Faraday's law

You might need: Periodic table

In an electroplating process,

26.0 g

of chromium metal is deposited from a solution of

Cr^{3 +} (a q)

ions.

How many coulombs of charge are transferred during this process?

The AP Chemistry exam includes a section of equations and constants that you can reference during the exam. One of the equations included in this section is the equation relating current and charge, which is shown below.

Electrolysis equation:

I = \frac{Q}{t}

Electrolysis variables and constants:

\begin{aligned} I & = current (amperes) \\ Q & = charge (coulombs) \\ t & = time (seconds) \end{aligned}

\begin{aligned} Faraday’s constant, F & = 96,485 coulombs per mole \\ of electrons \end{aligned}

AP®︎/College Chemistry

Course: AP®︎/College Chemistry > Unit 9

Problem