# Which of the following samples contains the largest number of atoms?

Which of the following samples contains the largest number of atoms?

a.    2.0 moles of $\ce{H3PO4}$
b.    3.0 moles of $\ce{H2SO3}$
c.    4.0 moles of $\ce{HNO3}$
d.    6.0 moles of $\ce{HClO}$
e.    8.0 moles of $\ce{HBr}$

My logic would tell me that every mole has $6.022\times10^{23}$ atoms in it. Then you divide the amount of grams of each compound by the number of moles?

so for A I'd  use the following:

(Avg # *2) / 98 grams/per mole of $\ce{H3PO4}$  = $1.22\times10^{22}$ atoms

and so on, but I don't get the right answer :/

$(2\times(6.022\times10^{23})$ = number of atoms = $1.20\times10^{23}$ $\ce{H3PO4}$ = 98 grams/mole

The answer is C btw, I just don't know to set up the equation right to get to this answer.

$\ce{K2SO4}$ has 2 moles of potassium, 1 mole of S and 4 moles of O per mole of $\ce{K2SO4}$. So that is 7 moles of atoms per mole $\ce{K2SO4}$.