Can Someone please solve this for me???

Question

Combining 0.255 mol Fe2O3 with excess carbon produced 14.8 g Fe.

Fe2O3+3C⟶2Fe+3CO

What is the actual yield of iron in moles?

actual yield:

What is the theoretical yield of iron in moles?

theoretical yield:

What is the percent yield?

percent yield:

Answer 1

The actual yield is the 14.8 grams of Fe that was made from this experiment, so you need to convert from grams to moles using the equation n = g / MM

n = 14.8 / 55.85 = 0.259 moles Fe

To find the theoretical yield first you need to write down the reaction and balance it.

Fe2O3 + 3C —> 2Fe + 3CO

The theoretical yield is the amount of yield you would get if all of the reactants reacted to make products.

You find the theoretical yield by taking what you are given which is 0.255 moles of Fe2O3 and using the balanced reaction to convert to moles product (which can be either Fe or CO - for this example we will use moles of Fe).

( 0.255 moles Fe2O3 ) * ( 2 moles Fe / 1 mole Fe2O3 ) = 0.51 moles Fe

For the last part of the question to find the theoretical yield you need to divide the actual by the theoretical then multiply by 100.

0.259 / 0.51 * 100 = 50.7%