Write the balanced complete combustion reaction foç your fuel unknown with exces
ID: 969231 • Letter: W
Question
Write the balanced complete combustion reaction foç your fuel unknown with excess oxygen (O_2). For simplicity, ignore the presence of anÿ additives. What volume of oxygen (at STP) would be needed to completely react with 10.0 g of your fuel? How many grams of CO_2 could be produced? (Use the balanced equation from Q4 above) Imagine you were able to capture and measure the CO_2 produced by your fuel burner and you found you produced only 70% of the expected amount. Explain the likely reason for this result. How would you expect the consumption of 0_2 and production of CO_2 in the system described in question 6 to be affected by the addition of an additive? Explain.Explanation / Answer
4.
2 C8H18 + 25 O2 --> 16 CO2 + 18 H2O
5.
Mass of fuel = 10 g
MW of fuel = 114.23 g/mol
Moles of fuel = 10 / 114.23 = 0.088
Moles of O2 required = 25 / 2 * 0.088 = 1.094
Volume of O2 required at STP = n R T / P = 1.094 * 0.0821 * 273.15 / 1 = 24.54 L
Moles of CO2 produced = 16 / 2 * 0.088 = 0.7
Mass of CO2 produced = 0.7 * 44.01 = 30.82 g
6.
Likely reasons are:
a) Insufficient air supply.
b) Insufficient mixing of air and fuel.
c) Insufficient air supply to the flame.
d) The size of the hydrocarbon also has an effect in normal conditions. If the liquid is not very volatile, only those molecules on the surface can react with the oxygen. Bigger molecules have greater Van der Waals attractions which makes it more difficult for them to break away from their neighbors and turn to a gas.
7. Combustion additives enhance fuel stability and quality, ensure a more complete burnout of hydrocarbon. It also reduces unburned carbon deposits.
By addition of an additive, consumption of O2 and production of CO2 in the system will increase.
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.