When a hydrocarbon such as octane is burned in an automobile engine most of the carbon is converted to .?

carbon dioxide but some carbon moxide is also produced. the reaction for the complete combustion of octane is: 2C8H18(g) + 25O2(g) ® 18H2O(g) + 16CO2(g)

In a particular engine it is observed that when 114.0 grams of octane is burned 334 grams of CO2(g) is produced. What is the percent yield of CO2(g)?

a) 16.0 %
b) 44.0 %
c) 94.9 %
d) 98.9 %

Answer:
For the complete combustion (i.e. no CO) the reaction would release 352 g of CO2 from 114 g of octane.
334/352 is 0.9488, so your answer should be c) 94.9%
c

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