The chemical formula for rust is #Fe_2O_3#. How many moles of #Fe# are present in 1.0 kg of the compound?

Answer 1

#"1.0 kg Fe"_2"O"_3"# contains #"13 mol Fe ions"#.

#"1 mol Fe"_2"O"_3"# contains #"2 mol Fe ions and 3 mol O ions"#

#"1.0 kg=1000 g"#

#"Molar mass Fe"_2"O"_3="159.6882 g/mol"# http://pubchem.ncbi.nlm.nih.gov/compound/14833#section=Top

Determine the moles of #"Fe"_2"O"_3"# by dividing the given mass by its molar mass, then multiply times the mol ratio between #"Fe"# ions and #"Fe"_2"O"_3"# to get the moles of #"Fe"# ions in #"1000 g Fe"_2"O"_3"#.

#1000cancel("g Fe"_2"O"_3)xx(1cancel("mol Fe"_2"O"_3))/(159.6882cancel("g Fe"_2"O"_3))xx(2"mol Fe")/(1cancel("mol Fe"_2"O"_3")##="13 mol Fe ions"# (rounded to two significant figures)

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Answer 2

Cooper Adams

To determine the number of moles of Fe in 1.0 kg of Fe₂O₃, we first need to calculate the molar mass of Fe₂O₃:

Molar mass of Fe = 55.845 g/mol Molar mass of O = 15.999 g/mol

Molar mass of Fe₂O₃ = (2 * molar mass of Fe) + (3 * molar mass of O)

Now, convert 1.0 kg to grams: 1.0 kg = 1000 g

Now, use the molar mass to find the number of moles of Fe in 1.0 kg of Fe₂O₃:

Number of moles = mass / molar mass

Now, substitute the values and calculate the number of moles of Fe.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.