Question

how can you determine the whole - number mole ratio in this substance?
your formula now is n₁o₁.₅.
although this shows the ratio of elements to each other, it is still not the empirical formula since there cannot be 1.5 atoms of oxygen in a molecule of this substance. how can you create a whole number ratio of atoms in this substance while still keeping the 1:1.5 ratio?
try to double, triple or quadruple the empirical formulas subscripts you have to get a proper empirical formula with the smallest whole number values possible.
fill in the whole number subscripts to create the empirical formula of this molecule.
n 1 mol
o 1.5 mol

Explanation:

Step1: Multiply the subscripts by 2

To convert the ratio \(1:1.5\) (or \(N_1O_{1.5}\)) to whole - number ratio, we use the property of ratios. If we have a ratio \(a:b\), we can multiply both \(a\) and \(b\) by the same non - zero number \(k\) to get an equivalent ratio \(ka:kb\). Here, \(a = 1\), \(b=1.5\), and \(k = 2\).
For \(N\): \(1\times2=2\)
For \(O\): \(1.5\times2 = 3\)

Answer:

The empirical formula with whole - number subscripts is \(N_2O_3\)