is it A or ????

Question

Calculate the mass of carbon dioxide produced from 15.3 g of octane in the reaction below.

2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O

a.53.1 g carbon dioxide 

b.0.737 g carbon dioxide 

c.47.2 g carbon dioxide 

d.94 g carbon dioxide 

e.1.072 g carbon dioxide 

Answer 1

Hello, Anjela,

I note in the comments that you concluded it wasn't option A. That was good to see, but the comment was cut short, so it wasn't clear if you had picked an answer.

Note that the balanced equation says we'll obtain an amount of CO₂ equal to 8 times the amount of C₈H₁₈ from the reactant side. 15.3 grams of octance is (15.3 grams/114.1 grams/mole) = 0.134 moles of octance. 8 times that amount yields 1.073 moles of CO₂. Convert moles CO₂ into grams CO₂ by multiplying by the molar mass of CO₂ (1.073g*44g/mole) = 44.6 grams.

This isn't an option in the question, so I may have made a math error somewhere. But the logic should work.

Bob

Answer 2

Check out this video to help you answer this question.

https://youtu.be/45mKzpJ5iIg