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.