A 7.640 gram sample of iron is heated in the presence of excess iodine. A metal...

A 7.640 gram sample of iron is heated in the presence of excess iodine. A metal iodide is formed with a mass of 42.36 g. Determine the empirical formula of the metal iodide.

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Expert Solution

Answer :

mass of Iron reacted = 7.640g Fe.

There was excess of iodine. We do not know how much iodine has reacted.

7.640g of Iron would have reacted completely to form 42.36g of iron iodide.

Iron iodide is formed from iron and iodine,

So, mass of iron iodide = mass of Iron + mass if Iodine.

plug the mass of iron iodide and Iron in this, we will get the mass of iodine reacted with iron.

42.36g of Iron iodide = 7.640g of iron + mass of iodine .

mass of iodine = 42.36g - 7.640g ; (Subtracting 7.640g from both the side. )

mass of iodine = 34.72g of Iodine .

Hence, mass of iron = 7.640g and mass of iodine = 34.72g .

Our next step will be to convert this to moles.

The atomic mass of Fe and I, must be obtained from the periodic table or you may take it from any Chemistry book.

Hope this will help you in understanding the problem.

Please let me know if you have not followed any step.

Thank you. :)

queen_honey_blossom answered 1 year ago

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