Chemistry
Elements and Compounds

# What is the empirical formula for a compound whose molecular formula is C2Cl6?

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Empirical Formula: CCl3

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## Related Questions

CCl6 doesn't exist. CCl4 and and C2Cl6 do however.

is non-polar, just by the symmetry of the molecule. The electronegativity of Cl is canceled with an electronegativity of another Cl opposite. :) I hope I have helped you

CH4 + 4Cl2 -----&gt; CCl2 + 4HCl This is the current common method of tetrachloride synthesis, under heat and pressure, although another involves further chlorinating of chlorocarbons e.g. C2Cl6 + Cl2. Earlier methods used chloroform or disulphide, reacted with chlorine.

Trimethylindium is extremely reactive towards oxygen and water. With low concentrations of oxygen (ppb to ppm to a few %), it immediately forms dimethylindium methoxide (Me2InOMe) as the first reaction product by insertion of O between In and C. With increased concentrations of oxygen (several %, atmospheric air or pure oxygen), it burns or explodes. Similar insertion reactions are expected with other elements of Group 16 (such as S, Se and Te) with highly vigorous outburst at higher concentrations of S, Se and Te. Trimethylindium reacts readily and vigorously with water to form Me2InOH and Methane (CH4) gas if the concentration of H2O is very small (upto 1000's ppm). With high concentrations of water (% level), trimethylindium can burn and often explode leaving behind In(OH)3, In2O3 as the final products. Extremely violent reactions of trimethylindium are also known with oxidizers (such as H2O2, KMnO4, HNO3, Bleach) and halogenated compounds (CCl4, CBrCl3, CBr2Cl2, CHCl3, C2Cl6 and halocarbon oils).

No: The molecular formula is never smaller than the empirical formula.

The molecular formula is the same as the empirical formula, NO2. The compound NO2 has a molar mass of 46g/mol, so the empirical and molecular formulas are the same.

A molecular formula is identical to the empirical formula, and is based on quantity of atoms of each type in the compound.The relationship between empirical and molecular formula is that the empirical formula is the simplest formula, and the molecular can be the same as the empirical, or some multiple of it. An example might be an empirical formula of C3H8. Its molecular formula may be C3H8 , C6H16, C9H24, etc. Looking at it the other way, if the molecular formula is C6H12O6, the empirical formula would be CH2O.

The empirical formula for a compound whose molecular formula is P4O10 is P2O5 = phosphor pentoxide.

Yes, the empirical formula is the most basic ratio of the elements in a compound, while the molecular formula is the ratio in a compound. For instance C5H10O could be both the empirical and the molecular formula or the molecular formula could be C10H20O2 the molecular formula depends on the molar mass.

An empirical formula may or may not be the same as a molecular formula. The empirical formula of a compound shows the smallest whole-number ratio of the atoms compound. The molecular formula tells the actual number of each kind of atom present in a molecule of the compound.

The formula of NO2 has a molecular weight of 46 g/mol. Your compound has a molecular weight of 92 g/mol. As you can see the molecular weight of the compound is twice that of the empirical formula. Therefore the molecular formula of your compound is:2 *(NO2) ---> N2O4

If you know the molar mass of the compound, you have to calculate the mass of the empirical formula and divide the molar mass of the compound by the mass of the empirical formula in order to find the ratio between the molecular formula and the empirical formula. Then multiply all the atoms by this ratio to find the molecular formula!

This is the chemical formula (empirical formula) or the formula unit of this compound.

The empirical formula tells you the simplest formula for the compound. The molecular formula will be some multiple of the empirical formula, or it can be identical to the empirical formula.

The molecular formula of this compound is N2H2. This is obvious because the empirical formula of a compound is the lowest positive integer ratio of atoms present.

What you write for an ionic compound is called the formula unit, but the formula unit is almost always the same as the empirical formula. The answer to your question could not be the molecular formula because an ionic compound is not a molecule.

C4H6. C2H3 gives a molecular mass of 27, 54/27 gives 2. Therefore the molecular formula is twice the empirical formula.

The empirical formula has the smallest whole number for their subscript whereas the molecular formula is the actual number of molecules or atoms in a compound.

The empirical formula is the lowest whole integer representation of the molecular formula. For example, the empirical formula for C6H12O6 would be CH2O.

An empirical formula is elaborated after the chemical analysis of a compound; for a structural formula more in depth studies are necessary.

A molecular formula specifies the exact number of atoms of each element in one molecule of a compound, but an empirical formula shows only enough of the atoms of the element with the smallest number of atoms in the compound to specify the proportions between or among each kind of atom in the compound. The subscript numbers after each atomic symbol in a molecular formula will therefore be an integral multiple of the subscript numbers in the empirical formula for the same compound. Since 1 is an integer, the molecular formula may be the same as the empirical formula, as it is for water, for example. A contrasting example is benzene, for which the molecular formula is C6H6, while the empirical formula is simply CH.