Tin and purple Iodine combine to form an orange solid tin iodide compound. If the compound contains 0.00383 moles of Sn and 0.01534 moles of I, what is its' empirical formula?

Sn = 0.00383 mols

I = 0.01534.

The easy way to find the ratio is to divide the smaller number by itself (thereby assuring you will get 1.000), the divide the other number by the same small number.
Sn = 0.00383/0.00383 = 1.00
I = 0.01534/0.00383 = 4.005
Then round to whole numbers so the empirical formula is SnI4.

Well, it seems like Tin and Purple Iodine got together to create a lovely orange solid compound! To find its empirical formula, we need to determine the ratio of atoms present in the compound.

First, let's convert the amount of moles to whole numbers. We'll divide both amounts by the smallest value, which is 0.00383 moles.

0.00383 ÷ 0.00383 = 1 Sn
0.01534 ÷ 0.00383 = 4 I

So, the empirical formula of the compound is SnI₄! Looks like they really went all out with the Iodine in this one.

In order to determine the empirical formula of the tin iodide compound, we need to find the simplest, ratio of atoms present in the compound.

1. Start by determining the number of moles of each element. We are given that the compound contains 0.00383 moles of tin (Sn) and 0.01534 moles of iodine (I).

2. Next, divide the number of moles of each element by the smallest number of moles. In this case, 0.00383 moles of Sn is the smallest, so we will divide the number of moles of each element by 0.00383.

Divide 0.00383 moles of Sn by 0.00383: 0.00383/0.00383 = 1.
Divide 0.01534 moles of I by 0.00383: 0.01534/0.00383 = 4.

3. The resulting values give us the ratio of atoms in the compound. We have 1 atom of Sn and 4 atoms of I.

4. Finally, represent the empirical formula by writing the element symbols and the numbers obtained in step 3 as subscripts. The empirical formula of the tin iodide compound is SnI₄.

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