Question

What mass of carbon dioxide (co2) can be produced from 15.6 g of c6h14 and excess oxygen?

Answer 1

Answer: The mass of carbon dioxide produced is 46.7 grams.

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$      .....(1)

Given mass of hexane = 15.6

Molar mass of hexane = 88.2 g/mol

Putting values in equation 1, we get:

$\text{Moles of hexane}=\frac{15.6g}{88.2g/mol}=0.177mol$

The chemical equation for the combustion of hexane follows:

$2C_6H_{14}+19O_2\rightarrow 12CO_2+14H_2O$

As, oxygen gas is present in excess, it is considered as an excess reagent.

Thus, hexane is considered as a limiting reagent because it limits the formation of product

By Stoichiometry of the reaction:

2 moles of hexane produces 12 moles of carbon dioxide

So, 0.177 moles of hexane will produce = $\frac{12}{2}\times 0.177=1.062mol$ of carbon dioxide

Now, calculating the mass of carbon dioxide by using equation 1:

Molar mass of carbon dioxide = 44 g/mol

Moles of carbon dioxide = 1.062 moles

Putting values in equation 1, we get:

$1.062mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=(1.062mol\times 44g/mol)=46.7g$

Hence, the mass of carbon dioxide produced is 46.7 grams.

Answer 2

C6H14+9.5O2=6CO2 +7H20
Number of moles of C6H14=15.6/86=0.1814 moles
so moles of CO2 = 6(0.1814)=1.088 
As the c6h14 has 1 is to 6 ratio with co2 
so
0.1814=mass/44
mass of co2 produced = 47.9 g