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 gasoline (the estimated annual consumption of gasoline
in the U.S.)? Remember, there are 3.785 liters in 1 gallon and
assume that isooctane is the only carbon containing component of
gasoline.
Scientific notation can be entered as follows: 1.23 x
1023 = 1.23E23
g
Compare the number of moles of C8H18 to
the number of moles of CO2 from the balanced
reaction. Using this, the information given above, and the periodic table, set up an equation so the units cancel.
|
Combustion reaction is a reaction in which, a hydrocarbon reacts with oxygen to produce carbon dioxide and water.
Mass, m of a substance is related to number of moles, n as follows:
Here, M is molar mass of substance.
The balanced chemical equation of combustion of isooctane is
Volume of gasoline present (v)
Mass of gasoline (m)
Where d is the density and v is the volume of gasoline
Substitute for d and for v
Now mass of isooctane will be
Substitute for m
Number of moles of isooctane
Substitute for and 114 g for M
According to equation, 2 moles isooctane gives 18 moles carbon dioxide
Hence 0.029 mol isooctane will give mol
Hence theoretical yield of carbon dioxide in moles is mol
Theoretical yield of carbon dioxide in g
Substitute mol for and 44 g for
According to equation, 2 moles isooctane gives 18 moles carbon dioxide
Hence isooctane will give mol
Ans:
Hence, the balanced equation is:
Theoretical yield of carbon dioxide is
Write the balanced equation for the combustion of isooctane (C8H18) to produce carbon dioxide and water....
2C8H18 + 25O2 → 16CO2 + 18H2O Assuming gasoline is 91.0% isooctane, with a density of 0.692 g/mL, what is the theoretical yield (in grams) of CO2 produced by the combustion of 1.39 x 1010 gallons of gasoline (the estimated annual consumption of gasoline in the U.S.)? Remember, there are 3.785 liters in 1 gallon and assume that isooctane is the only carbon containing component of gasoline. Scientific notation can be entered as follows: 1.23 x 1023 = 1.23E23
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?
The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2C8H18(l)+25O2(g)→16CO2(g)+18H2O(g) Relevant volumetric equivalencies 1 gal = 3.785 L 1 L = 1000 mL part C Octane has a density of 0.692 g/mL at 20∘C. How many grams of O2 are required to burn 17.0 gal of C8H18? Express the mass in grams to three significant digits.
The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2C8H18(l)+25O2(g)→16CO2(g)+18H2O(g) a. How many moles of O2 are needed to burn 1.35 mol of C8H18? b. How many grams of O2 are needed to burn 13.0 g of C8H18? c. Octane has a density of 0.692 g/mL at 20 degrees C. How many grams of O2 are required to burn 1.20 gal of C8H18?
The combustion of octane, C8H18,C8H18, proceeds according to the reaction shown. 2C8H18(l)+25O2(g)⟶16CO2(g)+18H2O(l)2C8H18(l)+25O2(g)⟶16CO2(g)+18H2O(l) If 522 mol522 mol of octane combusts, what volume of carbon dioxide is produced at 38.0 ∘C38.0 ∘C and 0.995 atm?
The combustion of octane, C8H18,C8H18, proceeds according to the reaction shown. 2C8H18(l)+25O2(g)⟶16CO2(g)+18H2O(l)2C8H18(l)+25O2(g)⟶16CO2(g)+18H2O(l) If 4.10×102 mol4.10×102 mol of octane combusts, what volume of carbon dioxide is produced at 12.0 ∘C12.0 ∘C and 0.995 atm?
The combustion of octane, C8H18, proceeds according to the reaction shown. 2C8H18(l)+25O2(g)⟶16CO2(g)+18H2O(l) Calculate the volume of carbon dioxide produced when 562 moles of octane combusts at 28.0 °C and 1.00 bar.
Based on the following combustion reaction of Gasoline 2C8H18+25O2=18H2O+16CO2. A. What mass of carbon dioxide is produced ( in grams) from 5.0x10g of octane(C8H18) combusting? B. What mass of water is produced ( in grams) from 5.0x10g of octane ( C8H18) combusting? C. How much O2 was consumed ( in gams) when 5.0x10g of octane (C8H18) is combusted?
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...