Respuesta :

teamath333
First we will calculate the number of moles of Iron:
[tex]n = \frac{m}{M} [/tex], where n is the number of moles, m is the mass of iron in the reaction and M is the Atomic weight.
[tex]n= \frac{84.9}{55.845} = 1,52[/tex] moles of Iron.
The same number of moles of Oxygen will take part in the reaction.
So [tex]1,52= \frac{mOxygen}{32} [/tex] where 32 is the Atomical Weight of Oxygen (16 x 2).
=>[tex]mOxygen=32*1,52=48,64[/tex]g

Answer:

36.385 grams of oxygen reacts when 84.9 grams of iron.

Explanation:

[tex]4Fe+3O_2\rightarrow 2Fe_2O_3[/tex]

Moles of iron = [tex]\frac{84.9 g}{56 g/mol}=1.5160 mol[/tex]

According to reaction, 4 moles of iron reacts with 3 moles of oxygen gas.

Then 1.5160 moles of iron will react with:

[tex]\frac{3}{4}\times 1.5160 mol=1.1370 mol[/tex] of oxygen gas

Mass of 1.1370 moles of oxygen gas:

[tex]1.1370 mol\times 32 g/mol=36.385 g[/tex]

36.385 grams of oxygen reacts when 84.9 grams of iron.

Otras preguntas