Answer:
[tex]\mathbf{ CH_2NO_3}[/tex]
Step-by-step explanation:
Element %by [tex](C)[/tex] [tex](H)[/tex] [tex](N)[/tex] [tex](O)[/tex]
composition 15.56 2.16 18.26 63.16
mole ratio
[tex]\dfrac{\% \ by \ mass}{atomic \ number }[/tex] [tex]\dfrac{15.56}{12}[/tex] [tex]\dfrac{2.16}{1}[/tex] [tex]\dfrac{18.26}{14}[/tex] [tex]\dfrac{63.16}{16}[/tex]
[tex]= 1.297[/tex] [tex]2.16[/tex] [tex]1.304[/tex] [tex]3.948[/tex]
Divide by the
smallest value [tex]= \dfrac{1.297}{1.297}[/tex] [tex]= \dfrac{2.16 } {1.297}[/tex] [tex]= \dfrac{1.304} {1.297}[/tex] [tex]= \dfrac{3.948} {1.297}[/tex]
ratio [tex]1[/tex] : [tex]2[/tex] : 1 : 3
The empirical formula is = [tex]\mathbf{ CH_2NO_3}[/tex]
