Could you please show me the process of solving these questions

Question

The reaction of 167 g of Fe2O3 with 85.5 g CO produces 72.3 g Fe. Calculate the following (12 points):

a. how much Fe will be formed?

b. Calculate the percent yield of Fe

Could you please show me the process of solving these problems because I have a test on this today and I don't understand? Pls and thank you

Answer 1

Whenever you are given the amounts of all the reactants, the first thing you must do, after balancing the equation, is FIND THE LIMITING REACTANT. So, first we balance the reaction between Fe₂O₃ and CO.

Fe₂O₃ + 3CO ==> 2Fe + 3CO₂ ... balanced equation

Next, find the limiting reactant. An easy way to do this is to divide the moles of each reactant by the corresponding coefficient in the balanced equation and see which value is the lowest.

For Fe₂O₃: 167 g Fe2O3 x 1 mol Fe₂O₃ / 159.7 g = 1.046 mols (÷1->1.046)

For CO: 85.5 g CO x 1 mol CO / 28.01 g = 3.052 mols (÷3->1.017)

Since 1.017 is less than 1.046, CO is LIMITING

Next step: Use the MOLES of the limiting reactant (3.052 mols) and the mole ratio in the balanced equation to find the theoretical yield of Fe....

(a). 3.052 mols CO x 2 mols Fe / 3 mols CO = 2.03 mols Fe x 55.85 g Fe/mol = 114 g Fe (3 sig. figs.)

(b). The percent yield is the actual yield divided by the theoretical yield (x100%). So we are supposed to get 114 g of Fe, but we got only 72.3 g

% yield Fe = 72.3 g / 114 g (x100%) = 63.4% yield