Question

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.

Answer 1

\[\frac{ Zn }{ 1 }\times \frac{ grams of one Zn }{ Zn atoms }\]
Without numbers, can you figure it out?

Answer 2

gramsofonezn =grams of one zinc
Znatoms= zinc atoms.

Answer 3

@Shalante can i try it out and then ask you if it's right? D:

Answer 4

Sure!
I answered your question by the way.

Answer 5

Sorry new to this and okay thanks!

Answer 6

Oh wait. I thought you were on a different board. I got confused my bad.

Answer 7

I gtg.
Be back in 90minutes
1Zn x (130.8g/6.023 x 10^23 Zn atoms.

Answer 8

okay thanks

Answer 9

\[\sf 130.8~g~Zn ~\times ~\frac{1~mol~ Zn}{65.38 ~g~Zn}~\times \frac{6.02~\times~10^{23}~Zn~atoms}{1~mol~Zn} \]\[\sf = \frac{(130.8 \cdot 6.02~\times~10^{23})}{65.38}~Zn ~atoms \] :)

Answer 10

@Jhannybean wait where did you get 65.38 from

Answer 11

Molar mass of zinc

Answer 12

ahhh im confused

Answer 13

Hmm, did I make a mistake?
I was helping 4 people at the same time.

Answer 14

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.

Answer 15

@Jhannybean
Your answer is in Zn atoms. Isnt it supposed to be the gram of one atom?

Answer 16

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.

Answer 17

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?)

Answer 18

I think my first formula is right.

Answer 19

If not, you can blame your teacher because of the bad wording.