Problem page liquid octane ch3ch26ch3 will react with gaseous oxygen o2 to produce gaseous carbon dioxide co2 and gaseous water h2o . suppose 6.9 g of octane is mixed with 10.1 g of oxygen. calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. round your answer to 3 significant digits.

- 8.89 g of carbon dioxide can be produced.

Solution:- The balanced equation for the combustion of octane in presence of oxygen to give carbon dioxide and water is:

From given info, we have 6.9 g octane and 10.1 g oxygen and asked to calculate the maximum mass of carbon dioxide formed.

It is a stoichiometry problem. Let's first figure out the limiting reactant. For this we could either calculate grams of octane required to react completely with given grams of oxygen or vice versa.

From balanced equation, there is 25:2 mol ratio between oxygen and octane.

Let's say we calculate grams of oxygen for given grams of octane as:

= 24.1 g oxygen

From calculations, 24.1 g of oxygen are required to react completely with 6.9 g of octane but in actual only 10.1 g of oxygen are available. So, oxygen is limiting reactant and so the product yield depends on it and calculated as:

= 8.89 g carbon dioxide

So, from given masses of octane and oxygen, maximum 8.89 g of carbon dioxide can be produced.

thats how its supposed to be

i just calculated it all out, and not including weekends, and all the different days off. as of this school year (2018-2019) students are spending 2198 hours in school this year