A student wants to reclaim the iron from an 18.0-gram sample of iron(III) oxide, which
occurs according to the reaction shown below:
2Fe2O3(s) — 4Fe(s) + 30,(g)
How many grams of iron can be reclaimed?

12.6g of Fe.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is given below:

2Fe2O3(s) —> 4Fe(s) + 3O2(g)

Next, we shall determine the mass of Fe2O3 that decomposed and the mass of Fe that is produced from the balanced equation.

This is illustrated below:

Mola mass of Fe2O3 = (56 x 2) + (16x3) = 160g/mol

Mass of Fe2O3 from the balanced equation = 2 x 160= 320g

Molar mass of Fe = 56g/mol

Mass of Fe from the balanced equation = 4 x 56 = 224g

From the balanced equation above,

320g of Fe2O3 decomposes to produce 224g of Fe.

Finall, we can obtain the mass of the Fe produced from the decomposition of 18g of Fe2O3 as follow:

From the balanced equation above,

320g of Fe2O3 decomposes to produce 224g of Fe.

Therefore 18g of Fe2O3 will decompose to produce = (18x224)/320 = 12.6g of Fe.

Therefore, 12.6g of Fe is obtained from 18g of Fe2O3.

1. they vary with a higher number because boiling is way hotter than melting