The number of atoms making up the compound is
Na = 1, N = 1, C = 5, H = 8 and O = 4
The empirical formula is the smallest comparison of atoms of compound forming elements.
A molecular formula is a formula that shows the number of atomic elements that make up a compound.
(empirical formula) n = molecular formula
The principle of determining empirical formula and molecular formula
Determine the mass ratio of the constituent elements of the compound.
Determine the mole ratio by dividing the elemental mass with the relative atomic mass obtained by the empirical formula
Determine molecular formulas by looking for values of n
Percentage of elements A and B in AxBy compounds:
% A in AₓBy = (x x Ar A / Mr AₓBy) x% AₓBy
% B in AₓBy = (y x Ar B / Mr AₓBy) x% AₓBy
It is known about the% mass of each element
To find the empirical formula, we look for its mole ratio (% mass/ its relative atomic mass)
Na = 13.6 / 23 = 0.5913
N = 8.29 / 14 = 0.5921
C = 35.51 / 12 = 2.9592
H = 4.77 / 1 = 4.77
O = 37.85 / 16 = 2.3656
To simplify the comparison as an integer, we divide by the mole ratio of the smallest element
Na = 0.5913 / 0.5913 = 1
N = 0.5921 / 0.5913 = 1
C = 2.9592 / 0.5913 = 5
H = 4.77 / 0.5913 = 8
O = 2,3656 / 0,5913 = 4
So the empirical formula:
NaNC5H8O4
We look for the molecular formula to get the number of atoms making up the compound
(NaNC5H8O4) n = Mr compound
(1.23 + 14.1 + 5.12 + 8.1 + 4.16) n = 169
(169) n = 169
n = 1
So that the empirical formula and molecular formula are the same so that the number of atoms making up the compound is
Na = 1, N = 1, C = 5, H = 8 and O = 4
the molar mass of a substance
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Determine the empirical and molecular formulas
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Determine the molecular formula of the compound
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Keywords: empirical formula, molecular formula, mass, mole