Isooctane, C8H18, is the component of gasoline from which the term octane rating derives.
A. Write a balanced equation for the combustion of isooctane to yield CO2 and H2O.
B. Assuming that gasoline is 100% isooctane, the isooctane burns to produce only CO2 and H2O, and that the density of isooctane is 0.792 g/mL, what mass of CO2 in kilograms is produced each year by the annual US gasoline consumption of 4.6 x 10^10 L?
C. What is the volume in L of this CO2 at STP?
D. How many moles of air are necessary for the combustion of 1 mol of isooctane, assuming that air is 21.0% O2 by volume.? What is volume in L of this air at STP?
Isooctane, C8H18, is the component of gasoline from which the term octane rating derives. A. Write a balanced equation f...
Write the balanced equation for the combustion of isooctane (C8H18) to produce carbon dioxide and water. Use the smallest possible integers to balance the equation. Also, separate the + sign with 1 space. 2C8H18 + 25O2 ? 16CO2 + 18H2O You are correct. Your receipt no. is 161-2857 Previous Tries Assuming gasoline is 90.0% isooctane, with a density of 0.692 g/mL, what is the theoretical yield (in grams) of CO2 produced by the combustion of 1.42 x 1010 gallons of...
Isooctane C8H18 is a major component of gasoline. Determine the change in enthalpy for the combustion of 228.0 g of isooctane from the following data: H2 (g) + 1/2O2 (g) ⟶ H2O (g) ΔH0 = −241.8 kJ C (s) + O2 (g) ⟶ CO2 (g) ΔH0 = −393.5 kJ 8C (s) + 9H2 (g) ⟶ C8H18 (l) ΔH0 = −224.13 kJ
the complete combustion of octane , C8H18, a component og gasoline, proceed as 2 C8H18 +25 O2 = 16 CO2 + 18H2O. a) how many moles of CO2 are produced when 1.50 mol octance reacted? b) how many grams of water produced in this reaction? c)how many moles of oxygen required to form 90.0 g water?
A major component of gasoline is octane (C8H18). When octane is burned in air, it chemically reacts with oxygen gas (O2) to produce carbon dioxide (CO2) and water (H2O). What mass of oxygen gas is consumed by the reaction of 4,41 g of octane. Round your answer to 3 significant digits
A major component of gasoline is octane C8H18. When octane is burned in air, it chemically reacts with oxygen gas O2 to produce carbon dioxide CO2 and water H2O. What mass of carbon dioxide is produced by the reaction of 6.46g of octane? Be sure your answer has the correct number of significant digits.
Here is the combustion reaction for octane (C8H18), which is a primary component of gasoline. How many moles of CO2 are emitted into the atmosphere when 17.1 g of C8H18 is burned?
According to the following combustion reaction of gasoline (Octane), how many moles of C8H18 needs to be reacted to produce 16 moles of CO2? C8H18 (l) + 25/2 O2 (g) → 8CO2 (g) + 9 H2O
The octane rating of gasoline is a relationship of the burning efficiency of the given gasoline mixture to the burning efficiency of octane (C8H18). (Figure 1)Like most hydrocarbons, octane reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is C8H18(g)+O2(g)→CO2(g)+H2O(g) part A:How many moles of water are produced in this reaction? part B:After the reaction, how much octane is left?
Consider the combustion reaction for octane (C8H18), which is a primary component of gasoline. 2C8H18+25O2⟶16CO2+18H2O How many moles of CO2 are emitted into the atmosphere when 26.6 g C8H18 is burned?
Consider the combustion reaction for octane (C8H18), which is a primary component of gasoline. 2C8H18+25O2⟶16CO2+18H2O How many moles of CO2 are emitted into the atmosphere when 25.6 g C8H18 is burned?