What is the mass of 3.7 * 10^20 molecules of Rubidium Phosphate? (Rb_3PO_4)

1 Answer
Nam D.
May 28, 2018

Approximately 2.16*10^-1 \ "g"=0.216 \ "g"

Explanation:

We first convert to moles of Rb_3PO_4. In a mole of a substance, there'll be 6.02*10^23 units of that substance.

So, here we have:

(3.7*10^20color(red)cancelcolor(black)(Rb_3PO_4 \ "molecules"))/(6.02*10^23color(red)cancelcolor(black)(Rb_3PO_4 \ "molecules")"/mol")~~6.15*10^-4 \ "mol"

Now to find the mass, we multiply by its molar mass, which is 351.3748 \ "g/mol".

6.15*10^-4color(red)cancelcolor(black)"mol"*(351.3748 \ "g")/(color(red)cancelcolor(black)"mol")~~2.16*10^-1 \ "g"

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