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Answered 2010-05-25 18:04:12

Yes. One of the simples examples is the pair butane and 2-methylpropane, which have not only the same empirical but the same molecular formula, C4H10.

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Benzene is an alkene, with four carbon atoms. Alkene have a general formula CnH2n, therefore the formula of benzene is C4H8. Now empirical formula is the simplest ratio of a compounds constituent atoms. In this case the ratio is 4:8, which can be simplified to 1:2. Thus the empirical formula of Benzene is CH2. In fact if you note the general formula of an alkene you can clearly see that the empirical formula for all alkenes will indeed be the same.

An empirical formula represents the lowest whole-number ratio of ions or atoms in a compound. The formulas for ionic compounds are always empirical, because the proportions of the ions are always reduced to the lowest whole-number ratio. The formulas for covalent compounds are sometimes empirical, in which case they are also the molecular formulas. For example, the formula for water, H2O, is an empirical/molecular formula because the ratio of hydrogen to oxygen atoms is 2:1, which represents the lowest whole-number ratio of atoms in a molecule of water.

the empirical formula is the simplest whole number ratio of the elements present in one molecule or formula unit of a compounds we calculate the empirical formula using the following steps: 1. note the mass of each element correctly 2. divide the atomic masses by the masses deduced in step 1 3. divide the step 2 calculation by the lowest figure

Empirical FormulaAll compounds are formed from different atoms of different elements through chemical bonding. Especially in organic chemistry, there are billions of different compounds which has made up from hydrogen and carbon.As an example let us take ethene and propene, which are two alkenes.The prior has 2 carbon atoms and 4 hydrogen atoms, and the latter has 3 carbon atoms and 6 hydrogen atoms.In both of these molecules, the simplest ratio between C:H is 1:2, hence both of these compounds have the empirical formula of CH2.Molecular FormulaThe molecular formula is given by the actual ratio of the atoms which are in the molecule. For example, ethanol and diethyl ether both have the same molecular formula of C2H6O (in the practice we write these with different notations though). Compounds with the same molecular formula are known as isomers. Constitutional isomers, Stereo-isomers and Conformational isomers are three main types of isomers.

The Chemical formula of Urea is CO(NH2)2 its empirical formula is just the same as its chemical formula. Urea has a molecular weight of 60.06gm.

The empirical formual for N2O4 is NO2

Note that di- means 2 so the empirical formula is SiO2.

C2N2H8 can be reduced to an empirical formula by dividing all the numbers by 2. So its empirical formula is CNH4. None of the others can be reduced so they are all empirical formulas.

The molecular mass is C2H7 you have 186.5 g of the substance, so calculate 2(12.01)+7(1.01)=31.09 so 186.5/31.09=6 so you can say C12H42 but when you divide 2 by 2 and 7 by 2 you obtain 1 and 3.5 because you have 3.5 you have to multiplied by 2 again, so you obtain the same formula as the empirical formula. It example is the same as water, which empirical formula es H2O as its molecular formula

No. A formula is only empirical if the elements are in their simplest whole number ratio. 4 and 6 are both divisible by 2. So the empirical formula for P4O6 would be P2O3

The emprical formula of caffeine( C8H10N4O2) is Carbon:Hydrogen:Nitrogen:Oxygen 8 : 10 : 4 : 2 4 : 5 : 2 : 1 So, its empirical formula will be wriiten as C4H5N2O

Formula: Pb(N3)2empirical: PbN6

Formula: Pb(N3)2empirical: PbN6

Formula: Pb(N3)2empirical: PbN6

Formula: Mg(O2)2Empirical: MgO4

Formula: Ba(N3)2Empirical: BaN6

It's empirical formula would be NH2. An empirical formula represents the ratio of the atoms in the compound, rather than the actual number. You can work this out by dividing by a common denominator (in this case, 2).

There are 4 step to determine molecular formula, which are given bellow Step:1:- Find empirical formula Step:2:- Find empirical formula mass Step:3:- Find n n=molecular mass/empirical formula mass Step:4:- now find molecular formula to find molecular formula molecular formula(empirical formula)n

CH3 is the empirical formula of C2H6; this molecule is an alkane commonly known as ethane.

The empirical formula would be C4H5O3 as you can divide all the subscripts by 2 to get the lowest common factor.

Yes, if we're talking about different masses of the same compound. This is because an empirical formula is the simplest whole number ratio of elements in a compound. For example water contains 2 hydrogen atoms for every one oxygen atom. If I have 18 grams of water, I have 2 mol H and 1 mol O. The empirical formula is H2O. If I have 36 grams of water, I have 4 mol H and 2 mol O. 4:2 simplifies to 2:1. The empirical formula is still H2O. If I find another compound of hydrogen and oxygen, and it has 1 mol hydrogen for every 1 mol oxygen, the empirical formula is HO, and this new compound is NOT water.

Its molecular formula will be Be(O2)2 but it can also be written in empirical formula as BeO4

No. A molecular formula can be the same as the empirical formula, such as CH4 (methane), because the two component atoms exist in a ratio that cannot be mathematically further broken down - one carbon to four hydrogens. In this case the molecular formula (the actual number of atoms per molecule), and the empirical formula (the simplest ratio of those numbers) is identical. On the other hand, ethane, C2H6 - two carbons to 6 hydrogens - has a molecular formula of C2H6 and a empirical formula of CH3, the ratio of 2 to 6 reduced to its simplest whole number form. Sooooooooooo, the molecular formula will always be equal to or greater than the empirical formula, and the empirical formula will always be equal to or less than the molecular formula. In other words (as if that wasn't enough), the molecular formula will never be less than the empirical formula and the empirical formula will never be greater than the molecular formula, but THE TWO CAN BE EQUAL. Whew!!! Ray

Empirical formula = C3H5O Molar mass of empirical formula = 3(12.01)+5(1.008)+1(16) = 57.07 Molar mass of molecular fomula = 114.15 n = Molar mass of molecular fomula/Molar mass of empirical formula = 114.15/57.07 n = 2 Molecular formula = n(empirical formula) Molecular formula = 2(C3H5O) = C6H10O2 Check: 6(12.01)+10(1.008)+2(16)= 114.14

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