The molecular formula is the same as the empirical formula, NO2. The compound NO2 has a molar mass of 46g/mol, so the empirical and molecular formulas are the same.
If you know the molar mass of the compound, you have to calculate the mass of the empirical formula and divide the molar mass of the compound by the mass of the empirical formula in order to find the ratio between the molecular formula and the empirical formula. Then multiply all the atoms by this ratio to find the molecular formula!
The molecular mass of a compound with the formula CH2O is approx. 30, not 120.
Yes, the empirical formula is the most basic ratio of the elements in a compound, while the molecular formula is the ratio in a compound. For instance C5H10O could be both the empirical and the molecular formula or the molecular formula could be C10H20O2 the molecular formula depends on the molar mass.
C4H6. C2H3 gives a molecular mass of 27, 54/27 gives 2. Therefore the molecular formula is twice the empirical formula.
the answer is: P4O10
The formula of NO2 has a molecular weight of 46 g/mol. Your compound has a molecular weight of 92 g/mol. As you can see the molecular weight of the compound is twice that of the empirical formula. Therefore the molecular formula of your compound is:2 *(NO2) ---> N2O4
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.
the molecular mass of a compound and its empirical formula
Since carbon has an atomic mass of 12 and hydrogen has an atomic mass of 1, the mass of the empirical formula is 12 + 3 = 15. 60/15 = 4; therefore, the molecular formula is C4H12.
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 molecular formula of ethene is C2H6.
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.
The empirical formula CH2 has a formula mass of 14, and 42.0/14 = 3. Therefore, the molecular formula is C3H6.
molar mass/ empirical formula mass
This molecular formula is C9H12.
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.
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.