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molar mass over grams of element
The 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 else can I help you with?
How do you calculate Molecular formula from empirical formulaWhat could you do with that information to determine that the empirical and molecular formulas are related to one another by a factor of 6?
In order to find molecular formula from empirical formula, one needs to know the molar mass of the molecular formula. Then you simply divide the molar mass of the molecular formula by the molar mass of the empirical formula to find out how many empirical formulae are in the molecular formula. Then you multiply the subscripts in the empirical formula by that number.
How does one determine a molecule formula from the 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.
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 the molecular formula of a compound that has a molecular mass of 54 and the empirical formula C2H3?
The empirical formula C2H3 has a molecular mass of 27 (C: 12, H: 1). To determine the molecular formula with a molecular mass of 54, the molecular formula would simply be double the empirical formula, so the molecular formula would be C4H6.
What information is needed to determine molecular formula?
the empirical formula and the molar mass
Can you determine the molecular formula of a substance from its percent composition?
Not completely. The empirical formula of a substance can be determined from its percent composition, but a determination of molecular weight is needed to decide which multiple of the empirical formula represents the molecular formula.
What Process of using empirical formula and the value for experimental molar mass to determine the molecular formula?
The empirical formula is the formula in its most simplified terms. The molecular formula is how many moles there actually are (the empirical formulat multiplied by a factor).
What additional information do you need to determine the molecular formula?
To determine the molecular formula, you need the molecular weight of the compound, the empirical formula, and any information about the compound's structure or the number of atoms of each element present. Additionally, knowing the types of elements involved can also help in calculating the molecular formula accurately. If the empirical formula is known, the ratio of the empirical formula's mass to the molecular weight will help in finding the actual molecular formula.
Determine the molecular formula of a compound if its empirical formula is C2H6O and its molar mass is 138g?
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
Determine the molecular formula for the unknown if the molecular mass is 60.0 amu and the empirical formula is CH2O.?
To determine the molecular formula from the empirical formula CH2O and given molecular mass of 60.0 amu, calculate the empirical formula mass: (12.01 g/mol for C) + 2(1.01 g/mol for H) + 16.00 g/mol for O = 30.02 g/mol. Then divide the given molecular mass by the empirical formula mass to find the factor by which the empirical formula must be multiplied to get the molecular formula: 60.0 amu / 30.02 g/mol ≈ 2. Next, multiply the subscripts in the empirical formula by this factor to find the molecular formula: 2(C)2(H)2(O) = C4H4O2, giving the molecular formula as C4H4O2.
To determine the subscript of an element in a molecular formula the empirical mass must be multiplied by the actual 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)
What steps are used to convert an empirical formula into a molecular formula?
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.
