Question

Here is the combustion reaction for octane (C8H18), which is a primary component of gasoline. How many moles of CO2 are emitted into the atmosphere when 11.6 g of C8H18 is burned?

Answer 1

Answer: The amount of
`CO_2` emitted into the atmosphere is 0.808 moles.

Step-by-step explanation:

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

`\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}`

For
`C_8H_(18)` :

Given mass of
`C_8H_(18)` = 11.6 g

Molar mass of
`C_8H_(18)` = 114.23 g/mol

Putting values in equation 1, we get:

`\text{Moles of }C_8H_(18)=(11.6g)/(114.23g/mol)=0.101mol`

The chemical equation for the combustion of octane follows:

`2C_8H_(18)+25O_2\rightarrow 16CO_2+18H_2O`

By stoichiometry of the reaction:

2 moles of octane produces 16 moles of carbon dioxide

So, 0.101 moles of octane will produce =
`(16)/(2)* 0.101=0.808moles` of carbon dioxide.

Hence, the amount of
`CO_2` emitted into the atmosphere is 0.808 moles.