Question

A major component of gasoline is octane, C8H18. When octane is burned in air, it chemically reacts with oxygen gas (O2) to produce carbon dioxide (CO2) and water (H2O) . What mass of carbon dioxide is produced by the reaction of 3.2g of oxygen gas? Round your answer to 2 significant digits.

Answer 1

`m_(CO_2)=2.8gCO_2`

Step-by-step explanation:

Hello,

In this case, the combustion of octane is chemically expressed by:

`C_8H_(18)+(25)/(2) O_2\rightarrow 8CO_2+9H_2O`

In such a way, due to the 25/2:8 molar ratio between oxygen and carbon dioxide, we can compute the yielded grams of carbon dioxide (molar mass 44 g/mol) as shown below:

`m_(CO_2)=3.2gO_2*(1molO_2)/(32gO_2) *(8molCO_2)/((25)/(2)molO_2 ) *(44gCO_2)/(1molCO_2)\\ \\m_(CO_2)=2.8gCO_2`

Best regards.