The equation for the reaction is
A_"r":color(white)(mmmll)14.01color(white)(mml)16.00Ar:mmmll14.01mml16.00
color(white)(mmmmmll)x"N"_2color(white)(m) + color(white)(ll) y"O"_2 → 2"N"_x"O"_y"mmmmmllxN2m+llyO2→2NxOy
"Mass/µg":color(white)(m)24.5color(white)(mmm)70.0"color(white)(mml)94.5
First, we must calculate the masses of "N" and "O" from the mass of the oxide.
"Mass of N in oxide = 24.5 µg"
"Mass of O in oxide" = "mass of oxide - mass of N" = "(94.5 - 24.5) µg" = "70.0 µg"
Now, we must convert these masses to moles and find their ratios.
From here on, I like to summarize the calculations in a table.
ul(bb("Element"color(white)(X) "Mass/µg"color(white)(X) "Amt/µmol"color(white)(m) "Ratio"color(white)(ml)×2color(white)(mm)"Integers"))
color(white)(mm)"N"color(white)(mmmml)24.5color(white)(mmmmll)1.748color(white)(Xmm)1color(white)(mmml)2color(white)(Xmmml)2
color(white)(mm)"O" color(white)(XXXml)70.0 color(white)(mmmmll)4.375 color(white)(mmm)2.502 color(white)(ml)5.004color(white)(Xml)5
The empirical formula is "N"_2"O"_5.
