The compound C12H26 is a liquid at room temperature.
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.
C12H26 is the chemical formula for dodecane, which is a straight-chain alkane hydrocarbon with 12 carbon atoms and 26 hydrogen atoms. It is a component of gasoline and is used as a solvent and in the production of various chemicals.
Kerosine (sometimes spelt kerosene) is a mixture of hydrocarbons that is a fraction from the fractional distillation of petroleum extracted between 150 and 200 0C. See wikipedia -fractional distillation for a diagram of an industrial fractionating column
Most modern lighters use butane. It is liquid under pressure but vaporizes when released. Butane lighters have no wick and make a slight hissing sound when in use. Lighters with a wick use a liquid fuel that is naphtha-based.
6.5 grams C12H26 (1 mole C12H26/170.328 grams) = 0.038 moles of C12H26
The size of C12H26 (dodecane) molecule can be approximated by calculating the sum of the atomic masses of its constituent atoms. C12H26 has a molecular weight of approximately 170 g/mol.
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.
High quality of CuSo4 (Copper Sulphate)
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.