Respuesta :
Explanation:
The given data is as follows.
Mass of antimony = 19.75 g
Molar mass of Sb = 121.76 g/mol
Therefore, calculate number of moles of Sb as follows.
Moles of Sb = [tex]\frac{mass}{\text{molar mass}}[/tex]
= [tex]\frac{19.75 g}{121.76 g/mol}[/tex]
= 0.162 mol
Mass of oxygen given is 6.5 g and molar mass of oxygen is 16 g/mol. Hence, moles of oxygen will be calculated as follows.
Moles of oxygen = [tex]\frac{mass}{\text{molar mass}}[/tex]
= [tex]\frac{6.5 g}{16 g/mol}[/tex]
= 0.406 mol
Hence, ratio of moles of Sb and O will be as follows
Sb : O
[tex]\frac{0.162}{0.162} : \frac{0.406}{0.162}[/tex]
1 : 2.5
We multiply both the ratio by 2 in order to get a whole number. Therefore, the ratio will be 2 : 5.
Thus, we can conclude that the empirical formula of the given oxide is [tex]Sb_{2}O_{5}[/tex].
