Question

For the reaction, calculate how many moles of the product form when 0.048 mol of O2 completely reacts. Assume that there is more than enough of the other reactant. 4Fe(s)+3O2(g)→2Fe2O3(s)

Answer 1

 0.032 moles of Iron(III) Oxide is produced.

Answer 2

Answer : The number of mole of product $Fe_2O_3$ form are 0.032 moles.

Explanation : Given,

Moles of $O_2$ = 0.048 mole

The balanced chemical reaction is,

$4Fe(s)+3O_2(g)\rightarrow 2Fe_2O_3(s)$

From the balanced chemical reaction we conclude that,

As, 3 moles of $O_2$ react to give 2 moles of $Fe_2O_3$

So, 0.048 moles of $O_2$ react to give $\frac{2}{3}\times 0.048=0.032$ moles of $Fe_2O_3$

Therefore, the number of mole of product $Fe_2O_3$ form are 0.032 moles.