Question

A chemistry student was asked to calculate the number of moles of iron required to react with 1.20 mol of oxygen to produce iron(III) oxide. His calculation is shown below: 1.20

Answer 1

To calculate the number of moles of iron required to react with 1.20 mol of oxygen to produce iron(III) oxide, you need to determine the stoichiometric mole ratio from the balanced chemical equation. The ratio is 1 mole of iron to 1.5 moles of oxygen, which can be multiplied by 2 to get the balanced equation.

Step-by-step explanation:

To calculate the number of moles of iron required to react with 1.20 mol of oxygen to produce iron(III) oxide, you need to determine the stoichiometric mole ratio from the balanced chemical equation. Based on the equation, the ratio is 1 mole of iron to 1.5 moles of oxygen. Since the ratio is not a whole number, you need to multiply it by 2 to get the smallest possible whole number subscripts while maintaining the correct iron-to-oxygen ratio. Therefore, the balanced equation is: 2 Fe + 1.5 O₂ → Fe₂O₃.

Answer 2

1.6 moles of iron

Step-by-step explanation:

-Metals reacts with oxygen to form oxides.

-The chemical reaction between oxygen and iron is written as below:

`4Fe_((s))+3O_2_((g))->2Fe_2O_3_((s))`

-pu notice from the balanced chemiocal equation above that the mole ration of iron to oxygen is 4:3

-We equate and cross multiply to find moles of iron in the reaction;

`Fe:O_2=4:3\\\\\\(Fe)/(O_2)=(4)/(3)\\\\(Fe)/(1.2)=(4)/(3)\\\\Fe=(4* 1.2)/(3)\\\\=1.6\ moles`

Hence, 1.6 moles of iron reacts with 1.2 moles of oxygen in the above reaction.