Question

A student has 3.86 g of iron metal. How many moles of iron does the student have? Show your work.

Given your answer to (a) and the fact that rust has the formula Fe2O3, how many moles of oxygen would be required to convert all of the iron to rust? Show your work.

Answer 1

The answer to your question is:

a) 0.069 moles of Iron

b) 0.052 moles of Oxygen

Step-by-step explanation:

Data

mass Iron = 3.86 g

moles = ?

Atomic weight Fe = 56 g

Process

a) Solve it using a rule of three

56 g of Fe ---------------- 1 mol

3.86 g ---------------------- x

x = (3.86 x 1) / 56

x = 0.069 moles of Iron

b)

Balanced Equation

4Fe + 3O₂ ⇒ 2Fe₂O₃

Solve it using a rule of three

4 moles of Fe ----------------- 3 moles of O₂

0.069 moles of Fe --------- x

x = (0.069 x 3) / 4

x = 0.052 moles of Oxygen