The empirical formula of metal iodide : CoI₃(Cobalt(III) Iodide)
<h3>Further explanation</h3>
13.02 g sample of Cobalt , then mol Co(MW=58.933 g/mol) :
![\tt mol=\dfrac{mass}{Ar}=\\\\mol=\dfrac{13.02~g}{58.933}\\\\mol=0.221](https://tex.z-dn.net/?f=%5Ctt%20mol%3D%5Cdfrac%7Bmass%7D%7BAr%7D%3D%5C%5C%5C%5Cmol%3D%5Cdfrac%7B13.02~g%7D%7B58.933%7D%5C%5C%5C%5Cmol%3D0.221)
Mass of metal iodide formed : 97.12 g, so mass of Iodine :
![\tt =mass~metal~iodide-mass~Cobalt\\\\=97.12-13.02\\\\=84.1~g](https://tex.z-dn.net/?f=%5Ctt%20%3Dmass~metal~iodide-mass~Cobalt%5C%5C%5C%5C%3D97.12-13.02%5C%5C%5C%5C%3D84.1~g)
Then mol iodine (MW=126.9045 g/mol) :
![\tt \dfrac{84.1}{126.9045}=0.663](https://tex.z-dn.net/?f=%5Ctt%20%5Cdfrac%7B84.1%7D%7B126.9045%7D%3D0.663)
mol ratio of Cobalt and Iodine in the compound :
Answer:
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Explanation: