Question #bb58b

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Question #bb58b

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Answer 1 · 2016-05-22T21:39:38

$1.32 \times 10^{22} formula units of CaO$ $1.32\times10^{22}" formula units of CaO"$ . Note that #"CaO"-does not form discrete molecules so we talk in terms of formula units. Unfortunately the question itself misleads by using "molecules".

Explanation:

First you need the molar mass. $CaO$ $"CaO"$ has one atom of $Ca (atomic mass 40.08)$ $"Ca (atomic mass 40.08)"$ and one atom of $O (atomic mass 16.00)$ $"O (atomic mass 16.00)"$ . So we add the two atoms:

$40.08 + 16.00 = 56.08 g/mol$ $40.08+16.00=56.08" g/mol"$

Now divide the mass by the molar mass and multiply by Avogrado's Number:

$\frac{1.23 g}{\frac{56.08 g}{mol}} \times \frac{6.022 \times 10^{23} formula units}{mol}$ ${1.23" g"}/{{56.08" g"}/"mol"}\times{6.022\times10^{23}" formula units"}/"mol"$
$= 1.32 \times 10^{22} formula units$ $=1.32\times10^{22}" formula units"$

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