# Worksheet: Charge Transfer in Electrolysis

In this worksheet, we will practice calculating the total amount of charge transferred during electrochemical processes such as electroplating.

**Q1: **

What is the charge of a mole of electrons? The charge of a single electron is C .

- A C
- B C
- C C
- D C
- E C

**Q3: **

The reduction of lithium ions can be represented by the ionic half-equation:

How many electrons are required per lithium ion to produce lithium metal?

How many moles of electrons are required to reduce 1.00 g of lithium ions?

How much charge must be delivered to reduce 1.00 g of lithium ions? The charge of a single electron is C.

- A C
- B C
- C C
- D C
- E C

**Q14: **

In one application, a 0.010 mm
layer of chromium must be deposited on
a part with a total surface area of
3.3 m^{2} from a solution containing chromium(III) ions. How long would it take to deposit
the layer of chromium if the current was
33.46 A? The density of
chromium (metal) is
7.19 g/cm^{3}.

**Q16: **

An irregularly shaped metal part made from a particular alloy was
galvanized with zinc using a
solution. When a current of
2.399 A was used,
it took exactly 1 hour
to deposit a 0.01323 mm
layer of zinc on the part.
What was the total surface area of the part?
The density of zinc is
7.140 g/cm^{3}.
Assume the efficiency is .