Problem: A piece of aluminum foil 1.00 cm square and 0.560 mm thick is allowed to react with bromine to form aluminum bromide.How many moles of aluminum were used? (The density of aluminum is 2.699 g/cm3.)

FREE Expert Solution

We are being asked to calculate the number of moles of aluminum used.


We are given the following measurements

area aluminum foil = 1.00 cm2

thickness aluminum foil = 0.560 mm

density aluminum = 2.699 g/cm3

mol aluminum = ?


To calculate the number of moles, we will use dimensional analysis.

Recall: We use dimensional analysis as a fail proof process to convert from one unit to another.


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Problem Details

A piece of aluminum foil 1.00 cm square and 0.560 mm thick is allowed to react with bromine to form aluminum bromide.

How many moles of aluminum were used? (The density of aluminum is 2.699 g/cm3.)

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Mole Concept concept. You can view video lessons to learn Mole Concept. Or if you need more Mole Concept practice, you can also practice Mole Concept practice problems.

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Based on our data, we think this problem is relevant for Professor Leigh's class at DIXIE.