2Fe2O3 + 3C > 4Fe + 3CO2
If 6.2 mol of Fe2O3 is used, what amount of C is needed, and what amounts of Fe and Co2 are produced?
Just follow the steps is this example. Post your work if you get stuck.
http://www.jiskha.com/science/chemistry/stoichiometry.html
Thank you! Very informative.
To find the amount of C needed, we need to use the stoichiometry of the balanced equation.
The balanced equation is:
2Fe2O3 + 3C → 4Fe + 3CO2
From the equation, we can see that 2 moles of Fe2O3 react with 3 moles of C to produce 4 moles of Fe and 3 moles of CO2.
Given that 6.2 mol of Fe2O3 is used, we can set up a proportion to find the amount of C needed:
2 mol Fe2O3 / 3 mol C = 6.2 mol Fe2O3 / x mol C
Cross multiplying:
2x = 3 * 6.2
2x = 18.6
x = 18.6 / 2
x = 9.3
Therefore, 9.3 mol of C is needed.
To find the amounts of Fe and CO2 produced, we can use the stoichiometry again.
From the balanced equation, we can see that for every 2 moles of Fe2O3, 4 moles of Fe are produced and 3 moles of CO2 are produced.
Given that 6.2 mol of Fe2O3 is used, we can set up proportions to find the amounts of Fe and CO2 produced:
2 mol Fe2O3 / 4 mol Fe = 6.2 mol Fe2O3 / x mol Fe
Cross multiplying:
2x = 4 * 6.2
2x = 24.8
x = 24.8 / 2
x = 12.4
Therefore, 12.4 mol of Fe is produced.
Similarly, for CO2:
2 mol Fe2O3 / 3 mol CO2 = 6.2 mol Fe2O3 / x mol CO2
Cross multiplying:
2x = 3 * 6.2
2x = 18.6
x = 18.6 / 2
x = 9.3
Therefore, 9.3 mol of CO2 is produced.
To determine the amounts of C, Fe, and CO2 produced in the reaction, we need to use stoichiometry and the given mole ratio from the balanced chemical equation.
The balanced chemical equation is:
2Fe2O3 + 3C → 4Fe + 3CO2
From the balanced equation, we can see that 2 moles of Fe2O3 react with 3 moles of C to produce 4 moles of Fe and 3 moles of CO2.
Given: 6.2 mol Fe2O3
Let's start by finding the amount of C needed.
Using the mole ratio from the balanced equation:
2 mol Fe2O3 : 3 mol C
We can set up a proportion to find the unknown amount of C:
(3 mol C / 2 mol Fe2O3) = (x mol C / 6.2 mol Fe2O3)
Cross-multiplying, we get:
3x = 6.2 * 2
3x = 12.4
x = 12.4 / 3
x ≈ 4.13 mol
Therefore, approximately 4.13 mol of C is needed.
Now, let's find the amounts of Fe and CO2 produced.
Using the mole ratio from the balanced equation:
2 mol Fe2O3 : 4 mol Fe
2 mol Fe2O3 : 3 mol CO2
We can set up proportions to find the amounts of Fe and CO2:
(4 mol Fe / 2 mol Fe2O3) = (y mol Fe / 6.2 mol Fe2O3)
(3 mol CO2 / 2 mol Fe2O3) = (z mol CO2 / 6.2 mol Fe2O3)
Cross-multiplying, we get:
4y = 6.2 * 2
4y = 12.4
y = 12.4 / 4
y ≈ 3.1 mol
3z = 6.2 * 3
3z = 18.6
z = 18.6 / 3
z ≈ 6.2 mol
Therefore, approximately 3.1 mol of Fe and 6.2 mol of CO2 are produced.
To summarize:
- Amount of C needed ≈ 4.13 mol
- Amount of Fe produced ≈ 3.1 mol
- Amount of CO2 produced ≈ 6.2 mol