We need to get the moles of each element in the compound.

The atomic masses are 58.69 g/mol Ni and 126.9 g/mol I.

$\mathbf{1}\mathbf{.}\mathbf{245}\mathbf{}\overline{)\mathbf{g}\mathbf{}\mathbf{Ni}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\mathbf{mol}\mathbf{}\mathbf{Ni}}{\mathbf{58}\mathbf{.}\mathbf{69}\mathbf{}\overline{)\mathbf{g}\mathbf{}\mathbf{Ni}}}$ **= 0.02121 mol Ni**

$\mathbf{5}\mathbf{.}\mathbf{381}\mathbf{}\overline{)\mathbf{g}\mathbf{}\mathbf{I}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\mathbf{mol}\mathbf{}\mathbf{I}}{\mathbf{126}\mathbf{.}\mathbf{9}\mathbf{}\overline{)\mathbf{g}\mathbf{}\mathbf{I}}}$** = 0.0424 mol I**

Divide the number of moles of each by the smallest value.

A chemist decomposes samples of several compounds; the masses of their constituent elements are listed. Calculate the empirical formula for each compound.

1.245 g Ni, 5.381 g I

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