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Chapter 1: Q10TY (page 20)

If the mass of isolated Fe2O3were 0.300 g, what would be the average mass of iron per tablet?

Short Answer

Expert verified

The average mass of iron per tablet will be 17.5 mg

Step by step solution

01

Define average mass

An average atomic mass, also known as an atomic weight, is the weighted average mass of the atoms in a naturally occurring sample of an element.

02

Determine the average mass of iron  

Evaluate the number of moles of isolated Fe2O2corresponding to 0.300 g of Fe2O2.

The number of moles of aferric oxide is calculated as:

Fe2O2=0.300g159.69g/mol=0.0019mol

Each mol of Fe2O2has two mol of iron and so, 0.019mol of Fe2O3has 2×0.0019=0.0038mol iron.

The mass of the iron in iron (i.e., 0.300g of Fe2O3) is:

0.0038molFe=massofFeatomicmassofFemassofFe=0.0038mol×55.845gFe=0.21gFe

Therefore, the average mass of the iron per iron tablet in each of the twelve tablets is:

0.21g/12=0.0175g=17.5mg

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