Question

Consider the combustion reaction for octane (C8H18), which is a primary component of gasoline.

2C8H18+25O2⟶16CO2+18H2O

How many moles of CO2 are emitted into the atmosphere when 27.6 g C8H18 is burned?

Answer 1

`n_(CO_2)=1.93 gCO_2`

Step-by-step explanation:

Hello,

In this case, considering the given chemical reaction, we can use the molar mass of octane (114.23 g/mol) and the 2:16 molar ratio with carbon dioxide to compute the emitted moles of CO2 to the atmosphere via the following stoichiometric procedure:

`n_(CO2)=27.6gC_8H_(18)*(1molC_8H_(18))/(114.23gC_8H_(18)) *(16molCO_2)/(2molC_8H_(18)) \\\\n_(CO_2)=1.93 gCO_2`

Which also corresponds to the following mass:

`m_(CO_2)=1.93molCO_2*(44gCO_2)/(1molCO_2) \\\\m_(CO_2)=85.0gCO_2`

Best regards.