Question

How many atoms of iodine are in 12.75g of CaI2? Hint. How many Iodines are there in one CaI2 particle?

(Answer) atoms of I (4 SF)

Answer 1

`5.225x10^(22)atoms\ I`

Step-by-step explanation:

Hello!

In this case, since 12.75 g of calcium iodide has the following number of moles (molar mass = 293.89 g/mol):

`n_(CaI_2)=12.75gCaI_2*(1molCaI_2)/(293.89gCaI_2)=0.0434molCaI_2`

In such a way, since 1 mole of calcium iodide contains 2 moles of atoms of iodine, and one mole of atoms of iodine contains 6.022x10²³ atoms (Avogadro's number), we compute the resulting atoms as shown below:

`atoms\ I=0.0434molCaI_2*(2molI)/(1molCaI_2) *(6.022x10^(23)atoms\ I)/(1molI) \\\\atoms\ I = 5.225x10^(22)atoms\ I`

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