C2h6
wt. of carbon= 12, and wt. of Hydrogen= 1
empirical formula wt. of CH3 = 12+1= 13
n= molecular wt./empirical formula wt.
= 30/13
=2.3
rounded off to 2.
therefore molecular formula is (CH3)n
= (CH3)2
= C2H6... which is ethane..
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 most common one would be C2H6, but there might be others.
This organic compound is ethane with the chemical formula C2H6.
The molecular formula of ethene is C2H6.
CH3 is the formula of methyl group.
C2h6.
gg
C4O2H8
The molecular mass of a compound with the formula CH2O is approx. 30, not 120.
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
2CH3O4BR
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.
C6h12o6
C26h38o4
Nh2cl
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 empirical formula and the molar mass
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.
C2h6
C4O2H8
The molecular mass of a compound with the formula CH2O is approx. 30, not 120.
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
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
The empirical formula CH2 has a formula mass of 14, and 42.0/14 = 3. Therefore, the molecular formula is C3H6.