Question

How many grams CO2 is produced by burning 1 gallon of ethanol (C2H6O), the amount of ethanol in 10 gallons of E10 gasoline. Remember the steps. Get to grams, grams to moles, moles to moles, moles to grams. 3.8 L in a gallon. The density of ethanol is 789 g/L.

Answer 1

Volume of Ethanol = 1 gallons = 1*3.8 = 3.8 L

Calculate the mass of Ethanol as follows:

Mass = vol*density = 789*3.8 = 2998.2 grams.

Molar mass of Ethanol = 46 g/mol

Calculate the moles of Ethanol as follows:

Moles = mass/molar mass = 2998.2/46

Moles = 65.17826 moles

Balanced reaction for combustion of ethanol is as follows:

C2H6O + 3O2 ---> 2CO2 + 3H2O

1 Mole of Ethanol will give 2 moles of CO2.

Calculate the moles of CO2 produced as follows:

Moles of CO2 = 2*moles of Ethanol = 2*65.17826

Moles of CO2 = 130.35652 moles.

Molar mass of CO2 = 44 grams/mole

Calculate the mass of CO2 as follows:

Mass of CO2 = mole*molar mass= 130.35652*44

Mass of CO2 = 5735.688 grams.

Therefore, answer is 5735.688 grams.

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