If there are $8.800 x 10^25$ atoms of tin, how many moles is this, and what would be the mass?

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Answer 1 · 2016-09-02T06:30:12

$"1 mole"$ of tin has a mass of $118.71*g$ ; there are $6.022140857(74)xx10^23$ individual atoms of tin in $1$ $mol$

And thus,

$"Moles of tin"$ $=$ $(8.800xx10^25" tin atoms")/(6.022xx10^23" tin atoms mol"^-1)$

$~=$ $146*mol$

And thus $"mass of tin atoms"$ $=$ $118.71*g*mol^-1xx146*mol$ $=$ $"over "17*kg$ of tin metal.

If there are 8.800 x 10^258.800 x 10^25 atoms of tin, how many moles is this, and what would be the mass?