When 84.8 g of iron(III) oxide reacts with an excess of carbon monoxide, iron is produced.
Fe2O3(s) + 3CO(g) ==> 2Fe(s) + 3CO2(g)
what is the theoretical yield of iron?
Use the balanced equation to determine the theoretical yield. Focus on the chemicals whose quantities you are given or are asked to find. CO is not important as it is excess and will make sure that all of the Fe2O3 will be changed to iron. Remember the quotients (numbers in front of formula) are the number of moles. You are given the mass of Fe2O3 in grams so you will need to convert 1 mole of Fe2O3 into grams (molar mass which, using simple atomic masses = 56x2 + 16x3 = 160g/mol but you use atomic masses that your course requires
Fe2O3(s) + 3CO(g)--> 2Fe(s) + 3CO2(g)
1 mol 2 mol
160g 112g
84.8g (112/160) x 84.8
So now you have the theoretical yield of Fe2O3 and the experimental (actual) yield = 54.3g)
Percentage Yield = (actual yield/theoretical yield) x 100
Hope this helps :)
how did u get the molar ratio of 1 to 2. I was confused and thought it was 3 to 1. (1 iron oxide(|||) and 3 carbon monoxide )
92% wc
Oh, I love a good chemical reaction! Let me do some math while keeping it light and breezy. Now, according to the balanced equation, 1 mole of Fe2O3 reacts with 3 moles of CO to produce 2 moles of Fe. To find the theoretical yield of iron, we need to convert grams of Fe2O3 to moles, and then use the mole ratio to find moles of Fe. Finally, we can convert moles of Fe to grams using its molar mass. Ready? Let's roll!
So, the molar mass of Fe2O3 is 159.69 g/mol. By dividing 84.8 g by the molar mass, we get moles of Fe2O3, which is approximately 0.531 moles.
Now, considering the mole ratio from the balanced equation, we find that 0.531 moles of Fe2O3 would produce 2 times 0.531 moles of Fe, which equals 1.062 moles of Fe.
Lastly, the molar mass of Fe is 55.85 g/mol. By multiplying the molar mass with the moles of Fe, we get the theoretical yield of iron, which is approximately 59.6 grams of Fe.
Voila! The theoretical yield of iron is approximately 59.6 grams. Keep in mind that in practice, the actual yield may differ, so don't be too hard on the iron if it doesn't match our calculations perfectly. It's trying its best!
To determine the theoretical yield of iron, we need to calculate the amount of iron that can be produced from the given amount of iron(III) oxide.
First, we need to find the molar mass of iron(III) oxide (Fe2O3). The molar mass of iron (Fe) is 55.845 g/mol, and the molar mass of oxygen (O) is 15.999 g/mol. Since there are 2 iron atoms and 3 oxygen atoms in each molecule of Fe2O3, the molar mass of Fe2O3 is:
(2 * 55.845 g/mol) + (3 * 15.999 g/mol) = 159.69 g/mol
Next, we need to calculate the number of moles of Fe2O3 in 84.8 g using the formula:
moles = mass / molar mass
moles = 84.8 g / 159.69 g/mol ≈ 0.531 moles
According to the balanced equation, 1 mole of Fe2O3 produces 2 moles of Fe. Therefore, we can calculate the number of moles of Fe that can be produced using the stoichiometry:
moles of Fe = 0.531 moles of Fe2O3 * (2 moles of Fe / 1 mole of Fe2O3) ≈ 1.062 moles
Finally, we can find the mass of iron by multiplying the number of moles of Fe by its molar mass:
mass of Fe = 1.062 moles * 55.845 g/mol ≈ 59.280 g
Therefore, the theoretical yield of iron is approximately 59.280 grams.
sdewf
Most of these problems, where only one reactant is given, is a simple stoichiometry problem. Print out these instructions and memorize them.
1. Write the equation and balance it.
2. Convert grams of iron oxide to moles. moles = grams/molar mass
3. Using the coefficients in the balanced equation, convert moles iron(III) oxide to moles Fe.
4. Now convert moles Fe to grams Fe. grams = moles x molar mass. This is the theoretical yield.