the definition of 'empirical mass' is the simplest ratio of the molecular mass.
for example: glucose.
the molecular mass of glucose is C6 H12 O6 = 180
but the empirical mass of glucose is C H2 O = 30
hope this helps. it's all about ratios.
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)
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.
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
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.
To determine the molecular formula from the empirical formula and gram formula mass, first calculate the empirical formula mass of C4H9 (4 carbons + 9 hydrogens). Then, divide the gram formula mass by the empirical formula mass to find the ratio. Finally, multiply the subscripts in the empirical formula by this ratio to get the molecular formula, which in this case is C8H18.
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.
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)
To calculate the empirical formula mass, first determine the molar mass of each element in the empirical formula by using the periodic table. Multiply the atomic mass of each element by the number of times it appears in the formula. Finally, sum these values to obtain the total empirical formula mass. This value represents the mass of one empirical formula unit of the compound.
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.
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.
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
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.
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.
The correct answer is a) empirical formula mass. The molar mass of a compound is often a whole number multiple of its empirical formula mass, as the empirical formula represents the simplest whole-number ratio of the elements in the compound, while the molar mass reflects the total mass of a mole of its molecules or formula units.
By determining the molecular mass, then dividing the molecular mass by the formula mass of the empirical formula to determine by what integer the subscripts in the empirical formula must be multiplied to produce the molecular formula with the experimentally determined molecular mass.
To determine the molecular formula from the empirical formula and gram formula mass, first calculate the empirical formula mass of C4H9 (4 carbons + 9 hydrogens). Then, divide the gram formula mass by the empirical formula mass to find the ratio. Finally, multiply the subscripts in the empirical formula by this ratio to get the molecular formula, which in this case is C8H18.
To determine the molecular formula from the empirical formula and the vapor density, we first need to calculate the empirical formula mass. The empirical formula mass of CH2O is 12g (carbon) + 2g (hydrogen) + 16g (oxygen) = 30g/mol. Next, we compare the vapor density with the empirical formula mass to find the factor by which the empirical formula mass is multiplied to get the molecular mass. The factor is 1.5 (45 / 30 = 1.5). Finally, we multiply the subscripts in the empirical formula by this factor to get the molecular formula, which is C3H6O3.