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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
What else can I help you with?
What is the molecular formula of a compound if the weight is of a unit of the compound is 120 and the empirical formula is C3H4?
To find the molecular formula, you first need to calculate the empirical formula mass of C3H4. C3H4 has an empirical formula weight of 40 g/mol. If the molecular weight is 120 g/mol, then the molecular formula would be 3 times the empirical formula, so the molecular formula would be C9H12.
What is the empirical formula of a compound with the molecular formula C 12 H 8?
The empirical formula of a compound with the molecular formula C12H8 is CH2. This is determined by dividing the subscripts in the molecular formula by the greatest common factor (in this case, 4) to obtain the simplest whole-number ratio of atoms in the compound.
The empirical formula is CH2O. What is the molecular formula of this compound?
The molecular formula of a compound is a multiple of its empirical formula, so the molecular formula is a multiple (in this case, 6 times) of CH2O, giving C6H12O6. This molecular formula corresponds to glucose, a common sugar.
What is the molecular formula of a compound with an empirical formula of CH?
The molecular formula of a compound with an empirical formula of CH is likely to be CH, as there is only one carbon atom and one hydrogen atom in the empirical formula. In this case, the empirical formula is also the molecular formula.
Simplest empirical formula for allicin?
C6H10OS2. Molecular and empirical are the same for Allicin.
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
Can the empirical formula of a compound be triple its molecular formula?
No, the empirical formula represents the simplest whole-number ratio of atoms in a compound, while the molecular formula shows the actual number of each element present in a compound. Therefore, the empirical formula cannot be triple the molecular formula.
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 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.
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 is the empirical formula for a compound whose molecular formula is C2Cl6?
The empirical formula for a compound is the simplest whole number ratio of the elements present in the compound. In this case, the empirical formula for a compound with a molecular formula of C2Cl6 is CH3Cl.
What represent a molecular compound?
This is the chemical formula (empirical formula) or the formula unit of this compound.
A compound has a mass of 16.7g 12.7g Iodine 4g Oxygen Therefore the empirical formula is I2O5 What additional information do you need to work out the molecular formula?
To determine the molecular formula, you would need the molar mass of the compound. With the molar mass, you can calculate the empirical formula mass and then determine the ratio between the empirical formula mass and the molar mass to find the molecular formula.
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.
How do you find molecular fomula?
To find the molecular formula of a compound, you need to know its empirical formula and molar mass. Divide the molar mass of the compound by the molar mass of the empirical formula to find the "multiplication factor." Multiply the subscripts in the empirical formula by this factor to get the molecular formula.
What is the molecular formula of a compound if the weight is of a unit of the compound is 120 and the empirical formula is C3H4?
To find the molecular formula, you first need to calculate the empirical formula mass of C3H4. C3H4 has an empirical formula weight of 40 g/mol. If the molecular weight is 120 g/mol, then the molecular formula would be 3 times the empirical formula, so the molecular formula would be C9H12.
