Iron(III) oxide is formed when iron combines with oxygen in the air. How many grams of Fe2O3 are formed when 16.7 g of Fe reacts completely with oxygen?

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You've got to be kidding. Just follow the instructions.

To determine the number of grams of Fe2O3 formed when 16.7 g of Fe reacts completely with oxygen, we need to use the stoichiometry of the chemical equation.

The balanced chemical equation for the reaction between iron and oxygen is:

4Fe + 3O2 → 2Fe2O3

From the balanced equation, we can see that 4 moles of Fe react with 3 moles of O2 to produce 2 moles of Fe2O3.

To find the number of moles of Fe, we can use the molar mass of Fe (55.85 g/mol) and the given mass:

moles of Fe = mass of Fe / molar mass of Fe
moles of Fe = 16.7 g / 55.85 g/mol

moles of Fe ≈ 0.299 mol (rounded to 3 decimal places)

According to the stoichiometry of the balanced equation, we see that 4 moles of Fe produce 2 moles of Fe2O3. Therefore, 0.299 mol of Fe will produce:

moles of Fe2O3 = (moles of Fe / 4) × 2
moles of Fe2O3 ≈ (0.299 mol / 4) × 2

moles of Fe2O3 ≈ 0.299 mol (rounded to 3 decimal places)

Now, to find the mass of Fe2O3 formed, we need to multiply the number of moles by the molar mass of Fe2O3 (159.69 g/mol):

mass of Fe2O3 = moles of Fe2O3 × molar mass of Fe2O3
mass of Fe2O3 ≈ 0.299 mol × 159.69 g/mol

mass of Fe2O3 ≈ 47.7 g (rounded to 3 decimal places)

Therefore, approximately 47.7 grams of Fe2O3 are formed when 16.7 g of Fe reacts completely with oxygen.

1. Write and balance the equation.

4Fe + 3O2 ==> 2Fe2O3

2. Convert what you have (in this case 16.7 g Fe) to moles. moles = grams/molar mass.

3. Using the coefficients in the balanced equation, convert moles of what you have (Fe) to moles of what you want (in this case Fe2O3).

4. Now convert moles of Fe2O3 to grams.
g = moles Fe2O3 x molar mass Fe2O3.

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