Question

Liquid octane will react with gaseous oxygen to produce gaseous carbon dioxide and gaseous water . Suppose 66. g of octane is mixed with 123. g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Be sure your answer has the correct number of significant digits.

Answer 1

`m_(CO_2)=108gCO_2`

Step-by-step explanation:

Hello,

In this case, the undergoing chemical reaction is:

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

In such a way, the limiting reagent is determined by the comparison between the available moles of octane and the moles of octane consumed by 123 g of oxygen as shown below:

`n_{C_8H_(18)}^(available)=66.0gC_8H_(18)*(1molC_8H_(18))/(114gC_8H_(18))=0.579molC_8H_(18)\\n_{C_8H_(18)}^(Consumed \ by \ O_2 )=123.0gO_2*(1molO_2)/(32gO_2)*(1molC_8H_(18))/((25)/(2)molO_2) =0.308molC_8H_(18)`

In such a way, since there are less grams consumed by the oxygen, octane is in excess whereas oxygen is the limiting reagent, therefore, the minimum amount of produced carbon dioxide by the reaction is:

`m_(CO_2)=0.308molC_8H_(18)*(8molCO_2)/(1molC_8H_(18)) *(44gCO_2)/(1molCO_2) \\m_(CO_2)=108gCO_2`

In this case, three significant figures should be used based on the initial data.

Best regards.