Question

Question #54f48

Answer 1

The correct answer is "None of the above". There are `6.62 × 10^24color(white)(l) "O atoms"` oxygen atoms present.

Explanation:

Step 1. Calculate the moles of `"FeSO"_4·7"H"_2"O"`

`"Moles of FeSO"_4·7"H"_2"O" = 278 color(red)(cancel(color(black)("g FeSO"_4·7"H"_2"O"))) × ("1 mol FeSO"_4·7"H"_2"O")/(278 color(red)(cancel(color(black)("g FeSO"_4·7"H"_2"O")))) = "1.000 mol FeSO"_4·7"H"_2"O"`

Step 2. Calculate the moles of `"O"` atoms

`"Moles of O atoms" = 1.000 color(red)(cancel(color(black)("mol FeSO"_4·7"H"_2"O"))) × "11 mol O atoms"/(1 color(red)(cancel(color(black)("mol FeSO"_4·7"H"_2"O")))) = "11.00 mol O atoms"`

Step 3. Calculate the number of `"O"` atoms

`"Number of O atoms" = 11.00 color(red)(cancel(color(black)("mol O atoms"))) × (6.022 × 10^23 "O atoms")/(1 color(red)(cancel(color(black)("mol O atoms"))))`

`= 6.62 × 10^24 color(white)(l)"O atoms"`