Question

how many moles of carbon dioxide (CO2) are produced when reacting 6.00 moles of butane (C4H10) in excess oxygen (O2)?

Answer 1

Balance the equation first:

1C4H10 + 13O2 ----> 8CO2 + 10H2O

As we know oxygen is in excess, butane is the limiting reactant.
the ratio between butane and CO2 is 1-8
Therfore
1:8
6:x
x=48
48 moles of CO2 will be produced

Answer 2

Answer: 24 moles

Explanation:

Combustion is a type of chemical reaction in which hydrocarbon is oxidized to carbon dioxide and water.

The balanced chemical reaction for combustion of butane is :

$2C_4H_{10}+13O_2\rightarrow 8CO_2+10H_2O$

According to stoichiometry,

Given: Oxygen is the excess reagent. Thus butane is the limiting reagent as it limits the formation of product.

2 moles of butane gives 8 moles of carbon dioxide.

Thus 6 moles of butane will give=$\frac{8}{2}\times 6=24moles$ of carbon dioxide.