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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.

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Q: What is the molecular formula of a compound given that molar mass of the compound is 30.04 gram and the empirical formula is NH?

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Calculate the empirical formula weight. Find the ratio of the molecular weight to the empirical formula weight. (n= molecular weight/ empirical formular weight). Multiply each subscript of the empirical formula by n.

The chemical formula in which the subscripts are given in the smallest ratio.

The formula given for butane is a molecular formula. The empirical formula for any molecular is obtained by dividing all the element subscript numbers by the highest common factor of all the subscripts; in this particular instance leading to C2H5 as he empirical formula.

The density or some other information must be given that allow you to find the molar mass. Calculate the empirical formula mass. Divide molar mass by empirical formula mass. This answer is multiplied by all subscripts of the empirical formula to get the molecular formula.

In order to find a substance's molecular formula, proceed with the following steps. An element's molecular formula is either going to be equal to the empirical formula or is a multiple of the empirical formula (n).1. Find the empirical formula's molar mass. Calculate the molar mass of the empirical formula.# atoms element A x atomic mass element A = mass A# atoms element B x atomic mass element B = mass B... etc.Add up all of the mass values found above for the empirical formula's molar mass (MM).2. Solve this equation (below).n = MM compound (given) = Empirical Formula Units---- MM emp. form.3. After solving for n, multiply the empirical formula.Molecular Formula = N (Empirical Formula)Ex. What is the molecular formula of a compound which has an empirical formula of CH2 and a molar mass of 126.2g?1. Find the empirical formula's molar mass.1 atom carbon (C) x 12.01g = 12.01g2 atoms hydrogen (H) = 2.016gEmpirical Molar Mass = 14.032. Solve this equation (below).n = 126.2g substance = 9 Empirical Formula Units (n)--------- 14.03g CH23. After solving for n, multiply the empirical formula.Molecular Formula = 9 (CH2) --> C9H18

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You have to find its empirical formula using the percentage composition. When you have done that, work out the relative molecular mass (Mr) of the empirical formula. This should be a multiple of the compound's Mr, so you multiply the amount of each atom in the empirical formula by this number, which gives you the final molecular formula.

Calculate the empirical formula weight. Find the ratio of the molecular weight to the empirical formula weight. (n= molecular weight/ empirical formular weight). Multiply each subscript of the empirical formula by n.

If you mean to find its molecular formula: 1. First you must obtain the empirical formula. Find the molar mass of the empirical formula. 2. The molar mass of the entire molecule must be given or its molecular formula cannot be find. 3. Put the molar mass given over the molar mass of the empirical formula. 4. Use this number (kind of like a scaler) to multiply by the entire empirical formula. This is the molecular formula.

Because an empirical formula is the simplest form of a compound, we know that the molecular formula contains more atoms than it does. Since we are given the molar mass, we can use this formula. x ( MM of empirical formula ) = MM of molecular formula MM of empirical formula = 12(2) + 1(6) + 16 = 46 MM of molecular formula = 138 46x = 138 x= 138 / 46 x=3 Therefore, the molecular formula is 3(C2H6O) that is C6H18O3

Because unlike the empirical formula, the molecular formula does not have to be the simplest ratio.If by chance you are given the percent composition of the elements in a substance, you could calculate the empirical formula and then the empirical formula's mass. However, the molecular formula equation is molecular formula= (empirical formula)n, where n is the mass of the molecular formula divided by the mass of the empirical formula. You would, therefore, need to know the mass belonging to the molecular formula, which you are not given.

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 empirical formula of SN has a formula unit mass of the sum of the gram atomic masses of nitrogen and sulfur, i.e., about 46.0667. The gram molecular mass given in the problem divided by this formula unit mass is about 4. Therefore, the molecular formula is S4N4.

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

The empirical formula is representative for the chemical composition of a compound; the structural formula is representative for the spatial structure of the compound.

The gram formula unit mass of the empirical formula C2H3 is twice the gram atomic mass of carbon plus three times the gram atomic mass of hydrogen, or about 27. The nearest integer to 162.27/27 is 6. Therefore, the molecular formula for the compound is C12H18.

The chemical formula in which the subscripts are given in the smallest ratio.

The formula given for butane is a molecular formula. The empirical formula for any molecular is obtained by dividing all the element subscript numbers by the highest common factor of all the subscripts; in this particular instance leading to C2H5 as he empirical formula.

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