An organic compound contains oxygen, 26.24%, and hydrogen, 4.92%. Find its empirical formula.

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Solution

Step 1: Given data:-
Percentage composition of oxygen is 26.24%
Percentage composition of hydrogen is 4.92%
Step 2: Finding the percentage composition of carbon:-
Percentage composition of carbon
$= 100 - (26.24 + 4.92) % = 100 - 31.16 = 68.84 %$
Step 3: Calculating the empirical formula:-
Element %Composition Atomic Weight Relative Number of Atoms Simplest Ratio
Carbon(C) 68.84% 12 $\frac{68.84}{12} = 5.736$ $\frac{5.736}{1.64} \times 2 = 7$
Oxygen(O) 26.24% 16 $\frac{26.24}{16} = 1.64$ $\frac{1.64}{1.64} \times 2 = 2$
Hydrogen(H) 4.92% 1 $\frac{4.92}{1} = 4.92$ $\frac{4.92}{1.64} \times 2 = 6$
The empirical formula of the compound is $C_{7} H_{6} O_{2}$
Therefore, the required empirical formula of the compound is $C_{7} H_{6} O_{2}$

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Element	%Composition	Atomic Weight	Relative Number of Atoms	Simplest Ratio
Carbon(C)	68.84%	12	$\frac{68.84}{12} = 5.736$	$\frac{5.736}{1.64} \times 2 = 7$
Oxygen(O)	26.24%	16	$\frac{26.24}{16} = 1.64$	$\frac{1.64}{1.64} \times 2 = 2$
Hydrogen(H)	4.92%	1	$\frac{4.92}{1} = 4.92$	$\frac{4.92}{1.64} \times 2 = 6$