How Much CO2 is Produced in a Combustion Reaction with 93% Yield?

[EnergyField]

Hi, I'm stuck with this problem.

C8H18 ------> H20 + 8CO2

There is 15g of C8H18 and 15g of Oxygen to make combustion reaction.

If the actual yield percent of CO2 is 93%, what mass of CO2 will be produced?

I approched with Morecular weight to get mol. and...I totally get lost.

 

[chemisttree]

I would usually start here by asking you to balance your equation but you don't need to in this case. You notice that there is a particular ratio of CO2 to octane in this example? Find the number of moles of octane you have in 15 g. How many moles of CO2 will be produced if the reaction has a 100% yield? A 93% yield? From moles of CO2 you should be able to determine mass...

 

[Blueshift5]

Hello, it seems like you are trying to calculate the mass of CO2 produced in a combustion reaction. To do this, you will need to use the balanced chemical equation provided: C8H18 ------> H20 + 8CO2.

First, you will need to determine the number of moles of C8H18 and O2 that are present. You can do this by dividing the given masses (15g) by their respective molecular weights (114 g/mol for C8H18 and 32 g/mol for O2). This will give you 0.132 moles of C8H18 and 0.469 moles of O2.

Next, you need to determine the limiting reactant in this reaction. This is the reactant that will be completely consumed and will determine the amount of product that can be formed. In this case, it is the C8H18 because there is less of it compared to O2.

Using the mole ratio from the balanced equation, we can determine that for every 1 mole of C8H18, 8 moles of CO2 will be produced. Therefore, with 0.132 moles of C8H18, we can expect 8 x 0.132 = 1.056 moles of CO2 to be produced.

Finally, we can use the given actual yield percent (93%) to determine the actual mass of CO2 produced. This can be done by multiplying the expected number of moles (1.056) by the molecular weight of CO2 (44 g/mol) and then multiplying by the actual yield percent (93%). This will give you a final answer of 43.6 g of CO2 produced.

I hope this helps you with your problem. Remember to always start with a balanced equation and use the mole ratio to determine the amount of product produced. Let me know if you have any further questions.