The balanced chemical equation for the combustion of C12H26 (dodecane) is: 2 C12H26 + 37 O2 -> 24 CO2 + 26 H2O.
The chemical formulas for liquid fuels can vary depending on the specific fuel. Some common liquid fuels and their formulas include gasoline (C8H18), diesel (C12H26), and kerosene (C12H26).
The compound C12H26 emits more CO2 when burned because it contains more carbon atoms per molecule compared to C2H4. When hydrocarbons are burned, the carbon atoms combine with oxygen from the air to produce carbon dioxide (CO2). Therefore, a compound with more carbon atoms will produce more CO2 when combusted.
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Dodecane can be cracked to form ethene by the following equation: C12H26 -> 2C2H4 + C4H10. This equation shows the decomposition of dodecane into ethene (C2H4) and butane (C4H10) as the products.
6.5 grams C12H26 (1 mole C12H26/170.328 grams) = 0.038 moles of C12H26
The balanced equation for the combustion of dodecane (C12H26) in air is: C12H26 + 18.5 O2 -> 12 CO2 + 13 H2O
from C12H26 to C15H32
The compound C12H26 is a liquid at room temperature.
The balanced chemical equation for the combustion of C12H26 (dodecane) is: 2 C12H26 + 37 O2 -> 24 CO2 + 26 H2O.
The chemical formulas for liquid fuels can vary depending on the specific fuel. Some common liquid fuels and their formulas include gasoline (C8H18), diesel (C12H26), and kerosene (C12H26).
The compound C12H26 emits more CO2 when burned because it contains more carbon atoms per molecule compared to C2H4. When hydrocarbons are burned, the carbon atoms combine with oxygen from the air to produce carbon dioxide (CO2). Therefore, a compound with more carbon atoms will produce more CO2 when combusted.
First, calculate the molar mass of C12H26 (dodecane) by multiplying the molar masses of carbon and hydrogen and summing them up. Then determine the moles of C12H26 in 3.73 kg by dividing the mass by the molar mass. As the balanced equation shows a 1:12 ratio between C12H26 and CO2, multiply the moles of C12H26 by 12 to find the moles of CO2 produced. Finally, determine the mass of CO2 by multiplying the moles by its molar mass.
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The balanced chemical equation for the reaction would be: C12H26 + 37 O2 → 12 CO2 + 13 H2O
Dodecane can be cracked to form ethene by the following equation: C12H26 -> 2C2H4 + C4H10. This equation shows the decomposition of dodecane into ethene (C2H4) and butane (C4H10) as the products.
Then what? Gasoline? Then the answer is no. Gasoline is C6H12. Diesel is C12H26. Same molecular construction. Just different number of atoms.