Step 1: Carbon is burned in a limited supply of oxygen to form carbon monoxide. Step 2: The carbon monoxide formed in Step 1 is used to reduce iron(III) oxide to metallic iron and carbon dioxide.
Calculate the mass (in kg) of O2 needed to produce 100 kg of Fe.
Can someone please help me with this and could you please write the equation out for me. Thanks to anyone who helps
I would like to apologize as I now know the first 3 gentlemen were correct. I offer my most sincere apologies for any potential damage caused.
To calculate the mass of O2 needed to produce 100 kg of Fe, we need to consider the stoichiometry of the reaction and use the molar masses of the substances involved.
First, let's write out the balanced equation for the reaction:
Step 1: C + O2 -> CO
Step 2: 3CO + Fe2O3 -> 2Fe + 3CO2
From the balanced equation, we can see that it takes three moles of carbon monoxide (CO) to reduce one mole of iron(III) oxide (Fe2O3) to form two moles of iron (Fe). This means that the ratio of CO to Fe is 3:2.
Now, let's calculate the molar masses of Fe and O2:
- Molar mass of Fe = 55.85 g/mol
- Molar mass of O2 = 32 g/mol
To find the mass of O2 needed to produce 100 kg (100,000 g) of Fe, we can use the ratio of CO to Fe as follows:
1) Calculate the moles of Fe:
Moles of Fe = Mass of Fe / Molar mass of Fe
Moles of Fe = 100,000 g / 55.85 g/mol
2) Calculate the moles of CO:
Moles of CO = (3/2) * Moles of Fe
3) Calculate the moles of O2:
Moles of O2 = Moles of CO
4) Calculate the mass of O2:
Mass of O2 = Moles of O2 * Molar mass of O2
Now, let's plug in the values and calculate the mass of O2 needed:
Moles of Fe = 100,000 g / 55.85 g/mol
Moles of CO = (3/2) * Moles of Fe
Moles of O2 = Moles of CO
Mass of O2 = Moles of O2 * Molar mass of O2
Note: It is important to carry out all calculations keeping the appropriate number of significant figures.
By following these steps, you should be able to calculate the mass of O2 needed to produce 100 kg of Fe.
Thank you DrBob. I got the answer correct and I understand it now.
Nuts to you three guys. Your answer(s) has/have nothing to do with the post by Jack. I would delete those three posts if I could. Here is the solution to Jack's problem.
2C + O2 ==> 2CO
Fe2O3 + 3CO ==> 2Fe(s) + 3CO2
So 1 mol O2 in eqn 1 = 2 mols CO
In eqn two, 2 mol Fe = 3 mols CO
Multiply eqn 1 by 3 and eqn 2 by 2 to obtain
eqn 1 x 3 is 3 mols O2 = 6 mols CO and
eqn 2 x 2 is 4 mols Fe = 6 mols CO; therefore,
3 mols O2 = 4 mols Fe.
Now, you want 100 kg Fe which is 100,000/55.85 = 1790 mols.
That will require 1790 mols Fe x (3 mols O2/4 mols Fe) = 1790 x 3/4 = ?
Convert that to grams by multiplying by molar mass of O2 (that's 32) = ?
Then convert grams to kg and you have it. Post your work if you have any trouble. As for the three funny guys (hahaha), just forget them.