The molecular formula mass of this compound is 240 amu. The subscripts in the actual molecular formula 8,16,8.
The molecular formula mass of this compound is 60.0 amu. The subscripts in the actual molecular formula are 2,4,2.
The molecular formula mass of this compound is 210 amu. The subscripts in the actual molecular formula Enter the subscripts for C H and O is 7,14.7.
Mana M Al mansour the answer is 5,10,5
The simplest form for a compound, called the empirical formula, gives the simplest whole-number ratio of the elements in the compound, and may differ from the actual molecular formula. For example, the molecular formula for glucose is C6H12O6. The empirical formula would be CH2O, which can be found by dividing the molecular subscripts by 6.
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 information about the actual molar mass is superfluous. Given any molecular formula, the corresponding empirical may be obtained by dividing all the subscripts in the molecular by the largest integer that yield an integer quotient for each subscript. In the given formula, the empirical formula is CH2.
The requirements for an empirical formula are that it give the correct ratios between all pairs of atoms in the actual molecule and have subscripts (including the value 1 implied by lack of an explicit subscript) with the lowest possible values to achieve all the correct ratios. To meet the latter condition, either one subscript must be one or the two smallest subscripts must be distinct prime number. The formula of the compound given has only one prime number subscript, 5. If all subscripts in the molecular formula are divided by the same number to yield an integral quotient, the resulting formula will still be empirically correct. In the given molecular formula, all the subscripts are integrally divisible by 5. Therefore, the empirical formula is CH3O2.
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.
Because Na2SO4 is an ionic compound and so does not have actual molecules.
The empirical formula of a compound shows the lowest whole number ratio of the elements in that compound; AKA simplest formula. The molecular formula describes the number of atoms of each element that make up the molecule or formula unit; AKA actual formula
Molecular formula. I think..
In an empirical formula, at least one of the element symbols must have a subscript (possibly including the implicit subscript "1" that is presumed when there is no explicit subscript) that is a prime number. The subscripts in a chemical formula must correspond to the actual number of atoms of each element present in a molecule or formula unit of the compound and therefore may be any integral multiple of the subscripts in the empirical unit. For example, the empirical formula of both acetylene (also called "ethyne") and benzene is CH, but the chemical formulas are C2H2 for acetylene and C6H6 for benzene. The empirical formula uses as subscripts the lowest whole number ratio of atoms combined in the substance. Many ionic substances do not have a molecular formula because they form a crystal lattice and not individual molecules. Molecular compounds may have both. The molecular formula shows the actual number of combined atoms in a single molecule.
An empirical formula contains the constituent elements in the lowest possible mathematical whole-number ratio. In some cases, this is the legitimate formula for the compound, particularly if the substance you're dealing with is an ionic compound. Sometimes, however, the actual formula, known as the molecular formula, is a whole-number multiple of the empirical formula. The molecular formula for glucose is C6H12O6. However, an empirically-derived formula for glucose would be CH2O, which is the lowest possible ratio of carbon, hydrogen, and oxygen in that compound.
the actual number of atoms in a molecule
The molecular formula specifies the actual number of atoms of each element in a molecule.
The empirical formula should have the lowest subscript numbers possible, consistent with the actual proportions of atoms present. In the formula given, all the subscripts are divisible by 4; therefore, the empirical formula should be C4H8O2N.
empirical formula shows the simplest ratio between atoms present in molecule. For example, the empirical formula of glucose is CH2o [c6h12o6]. it shows simple ratio between carbon, hydrogen and oxygen. molecular formula shows the actual number of combining atom in a compound. for example molecular formula of benzene is c6h6
The actual mass must be divided by the empirical mass. This was derived from the following equation: (subscript)(empirical formula) = (molecular formula) subscript = (molecular formula)/(empirical formula)
Molecular formula is the actual representation of the constitution of the substancewhile Empirical formula is the simplest representation of the molecular formula.Molecular formula= Empirical formula*n(where n= Molecular weight/Empirical formula weight)Example :-EtheneMolecular formula =C2H4Empirical formula=CH2here CH2 is the simplest representation of molecular formula of Ethene.
The empirical formula for cyclohexane is CH2. The molecular formula of cyclohexane is C6H12. Since an empirical formula gives only the proportions of elements present in a compound but not the actual numbers or arrangement of atoms the formula is CH2.
the empirical formula only gives the amount of each element as a ratiothe molecular formula gives the actual number of atoms of each element in a molecule of the compoundFor example these compounds all have the same empirical formula (CH2) but different molecular formulas: ethylene C2H4butene C4H8cyclohexane C6H12cyclooctane C8H16cyclodecane C10H20etc.
It is called phosphorus pentoxide, however the actual molecular formula is P4O10.It could also be called anhydrous phosphoric acid.
Empirical formulas show the simplest whole number ratio of these atoms. Molecular formulas show the actual ratio of atoms in the compound. For example: Glucose is the a simple sugar whose molecular formula is C6H12O6 Its empirical formula would be CH2O which would be its molecular formula divided by the smallest whole number. Chemical Name Hydrogen peroxide Empirical Formula HO Molecular Formula H2O2 chemical name Benzene empirical formula CH molecular formula C6H6 remember that several compounds can have the same empirical formula
First, find the atomic masses of the elements and add them together:C - 12.0H - 1.00_____13.0 gUse this formula to find the actual molecular formula:x(added atomic mass) = molar mass of compoundx(13.0) = 78.0 gDivide the added atomic mass to get x = #:x = 6Take your x value and multiply the number of atoms in the empirical formula by it:C1H1 * 6 = C6H6The final result is the actual molecular formula.