A compound containing #"36.5%"# of sulfur and #"63.5%"# of iron reacts with a compound containing #"27.6%"# oxygen and #"724%"# of iron. What is the balanced equation and the theoretical yield of iron oxide?
The theoretical yield of the iron oxide will be 880 g.
The first step is to use the known percent composition of sulfur in the compound to find the formula for iron sulfide. Assuming that the formula for iron sulfide looks like this
In this formula, the percentage of sulfur would be
This indicates that you've
This is how the chemical equation appears.
Proceed similarly with the iron oxide now.
You'll get this
This implies that the form of your balanced chemical equation will be as follows.
Because there is too much oxygen present, every mole of iron sulfide will participate in the reaction. To find out how many moles of the compound are in your 1.0-kg sample, use its molar mass.
This indicates that the response will result in
Thus, the reaction's theoretical yield will be
The answer, rounded to two sig figs, will be the number of sig figs you provided for the mass of iron sulfide.
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The balanced equation is
The theoretical yield of
A) EQUAL PERCENTAGE
We need to find the formulas for iron sulfide and iron oxide because iron can form multiple ions, and we need to do this in order to write a balanced chemical equation for this reaction.
Find the iron oxide and iron sulfide formulas.
Sulfur Dioxide
Fe=63.5% S=36.5%
By dividing the mass of each element by its molar mass (atomic mass on the periodic table in grams), we can convert the masses to moles. Since 36.5% is 35/100, we can assume a 100-g sample of iron sulfide and state that there are 36.5 g S and 63.5 g Fe.
Sulfur
Iron
Sulfur and iron are found in a 1:1 ratio.
Oxide of Iron
Once more, we can assume a 100-g sample of iron oxide because 27.6% is 27.6/100. Based on this, we can say that there are 27.6 g of oxygen and 72.4 g of Fe. Once more, we can convert the masses to moles by dividing each element's mass in grams by its molar mass, or atomic mass on the periodic table.
Air
Iron
Mole proportions of Fe and O
Calculate the smallest number of moles by dividing the moles of each element.
Equilibrated Chemical Formula
B) IRON OXIDE THEORICAL YIELD
Molar mass of #"Fe"_3"O"_4=(3xx55.945 "g/mol")+(4xx15.999 "g/mol")=231.531 "g/mol"#
The mole ratio between iron sulfide and oxide is:
Determine the Theoretical Iron Oxide Yield
To calculate moles of iron oxide, multiply moles of FeS by the mole ratio of iron oxide to iron sulfide, or 1 kg FeS to 1000 g FeS. Next, use the molar mass of FeS to convert its mass to moles. Finally, multiply the moles of iron oxide by their molar mass.
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The balanced equation for the reaction between sulfur-iron compound and oxygen-iron compound is:
4FeS + 7O2 → 2Fe2O3 + 4SO2
To find the theoretical yield of iron oxide (Fe2O3), we need to calculate the moles of each reactant, determine the limiting reactant, and then use stoichiometry to find the moles of Fe2O3 produced. Finally, we convert moles of Fe2O3 to grams.
Given the percentages:
- The molar mass of FeS is approximately 87.91 g/mol.
- The molar mass of Fe2O3 is approximately 159.69 g/mol.
Now, we can calculate the moles of each reactant:
- Moles of FeS = (36.5 g / 100 g/mol) / 87.91 g/mol
- Moles of O2 = (27.6 g / 100 g/mol) / 32 g/mol
- Moles of FeS = (724 g / 100 g/mol) / 159.69 g/mol
Next, we determine the limiting reactant, which is the one that produces the least amount of product. After finding the limiting reactant, we use stoichiometry to find the moles of Fe2O3 produced.
Finally, we convert moles of Fe2O3 to grams using its molar mass.
This process will give us the theoretical yield of iron oxide.
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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.
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.
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.
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.
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