if 100 g of iron were reacted with 100 g of oxygen according to the reaction below, the maximum yield in grams of Fe2O3 would be:
chemistry urgent - bobpursley, Tuesday, November 30, 2010 at 4:20pm
Balance the equation. Note the coefficents on Fe and O2, that is the mole ratio.
calcuate how many moles of Fe, and O2 you have.
Which is the limiting reactant.
For instance, if the coefficents were 45Fe+ 34O2, the mole ratio of O2 to Fe is 34/45
If you had 2.3 moles of Fe, and 3.2 moles of O2, your mole ratio of O2 to Fe would be 3.2/2.3, significantly greater than the coefficents of needed moles. Well, if you have more, that means you have too much O2, so you limiting reageant would be Fe.
Finally, figure out how much product you get with your limiting reageant.
Dear Bobberley,
I'm still don't get it yet. Please help
4 Fe + 3 O2 -> 2 Fe2O3
a. 143
b. 260
c. 333.7
d. 200
e. none of these
You need to learn to do these so I don't intend to do this for you. However, if you follow the steps in the link I gave you (or if you follow Bob Pursley's instructions) you should get where you want to go.
Post any steps you don't understand with your work. We can help you through but only after we know what you don't understand WITH THE WORK.
To find the maximum yield in grams of Fe2O3, we need to determine the limiting reactant and then calculate the amount of product obtained from that reactant.
1. Start by balancing the chemical equation:
4 Fe + 3 O2 -> 2 Fe2O3
2. Now, we need to calculate the number of moles of Fe and O2 we have. To do this, we use the molar mass of each element:
- Molar mass of Fe: 55.85 g/mol
- Molar mass of O2: 32 g/mol
Number of moles of Fe = mass of Fe / molar mass of Fe
Number of moles of O2 = mass of O2 / molar mass of O2
Based on the question, we have 100g of iron and 100g of oxygen. So:
Number of moles of Fe = 100g / 55.85 g/mol
Number of moles of O2 = 100g / 32 g/mol
3. Now we need to determine the limiting reactant. The limiting reactant is the one that is completely consumed first, limiting the amount of product that can be formed. To find the limiting reactant, we compare the mole ratios of the reactants.
Looking at the balanced equation:
4 Fe + 3 O2 -> 2 Fe2O3
The mole ratio of O2 to Fe is 3/4.
Using the number of moles of Fe and O2 calculated earlier, we can determine the mole ratio:
Mole ratio of O2 to Fe = (moles of O2) / (moles of Fe)
4. Finally, we compare this mole ratio to the stoichiometric ratio (coefficients in front of the reaction) to determine the limiting reactant. If the mole ratio is larger than the stoichiometric ratio, it means we have an excess of that reactant. The reactant with the smaller mole ratio is the limiting reactant.
5. Once we have determined the limiting reactant, we can calculate the amount of product obtained from that reactant.
Looking at the balanced equation:
4 Fe + 3 O2 -> 2 Fe2O3
The ratio of Fe2O3 to O2 is 2/3.
Using the mole ratio of Fe2O3 to O2 and the number of moles of the limiting reactant, we can calculate the moles of Fe2O3 produced.
Moles of Fe2O3 = (moles of limiting reactant) * (ratio of Fe2O3 to limiting reactant)
Finally, we convert the moles of Fe2O3 to grams using the molar mass of Fe2O3:
Mass of Fe2O3 = Moles of Fe2O3 * Molar mass of Fe2O3
The answer to the question is the mass of Fe2O3 calculated above.