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yes it is
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Is the empirical formula molar mass less than or equal to the actual molar mass for all compound?
The empirical formula molar mass is the mass of the simplest whole-number ratio of the elements in a compound, while the actual molar mass corresponds to the molar mass of the compound's molecular formula. The empirical formula molar mass is always less than or equal to the actual molar mass because the empirical formula represents the smallest ratio of atoms, which can be multiplied to obtain the molecular formula. Therefore, for compounds with a molecular formula that is a multiple of the empirical formula, the empirical molar mass will be less than the actual molar mass.
How does one determine a molecular formula from the empirical form?
molar mass of unknown/molar mass of empirial = # of empirical units in the molecular formula. Example: empirical formula is CH2O with a molar mass of 30. If the molar mass of the unknown is 180, then 180/30 = 6 and molecular formula will be C6H12O6
What is relationship between the formula weight of a substance and its molar mass?
Molar mass is the mass of particles in one mole of a substance. Molar mass is equal to atomic/ molecular/ formula mass in amu. Formula mass is in atomic mass unit while molar mass is in grams .
How does on determine a molecular formula from the empirical formula?
molar mass over grams of elementThe above answer is somewhat correct. In order to find the molecular formula when given the empirical formula, you must first find the molar mass of the empirical formula.MOLAR MASS# atoms element A x Atomic Mass element A (Periodic Table) = mass A# atoms element B x atomic mass element B (periodic table) = mass B... etc.Add up all of the mass values found above and you have the molar mass.Then, after you have found the empirical formula's molar mass, you divide the molar mass of the molecular formula by the empirical formula's molar mass (solving for n).MOLECULAR FORMULA EQUATION: N (Empirical formula) (read as N times empirical formula) where:N = Molar mass substance---- Molar Mass emp. form.
How many times heavier is the molar mass than the empirical formula mass?
The molar mass of a compound is typically a multiple of its empirical formula mass, depending on the molecular formula. To determine how many times heavier the molar mass is than the empirical formula mass, you can divide the molar mass by the empirical formula mass. This ratio will yield a whole number that represents how many times the empirical formula fits into the molecular formula. For example, if the molar mass is 60 g/mol and the empirical formula mass is 15 g/mol, then the molar mass is 4 times heavier than the empirical formula mass.
How does one determine a molecular formula from empirical formula?
molar mass over grams of elementThe above answer is somewhat correct. In order to find the molecular formula when given the empirical formula, you must first find the molar mass of the empirical formula.MOLAR MASS# atoms element A x Atomic Mass element A (Periodic Table) = mass A# atoms element B x atomic mass element B (periodic table) = mass B... etc.Add up all of the mass values found above and you have the molar mass.Then, after you have found the empirical formula's molar mass, you divide the molar mass of the molecular formula by the empirical formula's molar mass (solving for n).MOLECULAR FORMULA EQUATION: N (Empirical formula) (read as N times empirical formula) where:N = Molar mass substance---- Molar Mass emp. form.
What is the molecular formula of a compound with the empirical formula NH2Cl and molar mass of 51.5g mol?
The empirical formula NH2Cl has a molar mass of 51.5 g/mol, so the molecular formula can be determined by finding the ratio of the molar mass of the molecular formula to the molar mass of the empirical formula. The molecular formula of the compound is therefore NH2Cl2.
What is the molecular formula of NH2Cl molar 51.5g?
The molar mass of NH2Cl is 51.5 g/mol, which means one mole of NH2Cl weighs 51.5 grams. The molecular formula of NH2Cl remains the same, NH2Cl, regardless of its molar mass.
What is the molecular formula of a compound given the molar mass of the compound is 186.5g and the empirical formula is C2H7?
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
Styrene has the empirical formula CH. It has a molar mass of 104 g. What is the multiplier to get the molecular formula?
The molar mass of styrene (C8H8) is 104 g/mol. The empirical formula is CH, which has a molar mass of 13 g/mol. To find the multiplier to get the molecular formula from the empirical formula, divide the molar mass of the molecular formula by the molar mass of the empirical formula: 104 g/mol / 13 g/mol = 8. This means the multiplier is 8, and the molecular formula of styrene is C8H8.
What is the molecular formula of the compound ch2 with molar mass equals 168 gmol?
c12h24
Do glucose and fructose have the same molar mass?
Yes, glucose and fructose have the same molar mass, which is approximately 180.18 g/mol. Both are monosaccharides with the molecular formula C6H12O6, differing only in their structural arrangement. This structural difference is why they are classified as isomers, but their molar mass remains identical.
