A sample of zinc with a mass of 130.8g contains 6.02 x 10^23 atoms. Calculate the mass of a single zinc atom.

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A sample of zinc with a mass of 130.8g contains 6.02 x 10^23 atoms. Calculate the mass of a single zinc atom.

Chemistry
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\[\frac{ Zn }{ 1 }\times \frac{ grams of one Zn }{ Zn atoms }\] Without numbers, can you figure it out?
gramsofonezn =grams of one zinc Znatoms= zinc atoms.
@Shalante can i try it out and then ask you if it's right? D:

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Sure! I answered your question by the way.
Sorry new to this and okay thanks!
Oh wait. I thought you were on a different board. I got confused my bad.
I gtg. Be back in 90minutes 1Zn x (130.8g/6.023 x 10^23 Zn atoms.
okay thanks
\[\sf 130.8~g~Zn ~\times ~\frac{1~mol~ Zn}{65.38 ~g~Zn}~\times \frac{6.02~\times~10^{23}~Zn~atoms}{1~mol~Zn} \]\[\sf = \frac{(130.8 \cdot 6.02~\times~10^{23})}{65.38}~Zn ~atoms \] :)
@Jhannybean wait where did you get 65.38 from
Molar mass of zinc
ahhh im confused
Hmm, did I make a mistake? I was helping 4 people at the same time.
I dont think we need molar mass since the grams would cancel out and we need to know the mass of a single Zinc atoms.
@Jhannybean Your answer is in Zn atoms. Isnt it supposed to be the gram of one atom?
Maybe it is 130.8g Zn/65.38g Zn=2.00 mol Zn \[\frac{ 2.00 mol Zn }{ 1 }\times \frac{ 6.022\times10^{23} Zn atoms }{ 1mol Zn }=1.2044\times10^{24}Zn atoms\]=1.2044 x 10^24 Zn atoms Divide 130.8 grams by that big number.
Not sure why the question tells us 130.8 g of Zn contains 6.022 x 10^23 atoms. (Is it trying to trick us or is it an exception?)
I think my first formula is right.
If not, you can blame your teacher because of the bad wording.

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