Question

What is the mass, in grams, of a sample of 6.98 × 1024 atoms of magnesium (Mg)? Show your work or explain the steps that you used to determine your answer.

Answer 1

Hello!

* First Step: to know Avogrado's Law

We know that by the Law of Avogrado, for each mole of substance we have 6.02*10²³ atoms, if:

** Second Step: to know the molar mass of the solute

The molar mass of of magnesium = 24.30 g/mol

*** Third step: make the ratio mass / mol with atoms

1 mol we have 6.02*10²³ atoms

1 mole of Mg we have 24.30 g

Then we have:

24.30 g ------------- 6.02*10²³ atoms

x ----------------------- 6.98*10^24 atoms

`(24.30)/(x) = (6.02*10^(23))/(6.98*10^(24))`

multiply cross

`6.02*10^(23)*x = 24.30*6.98*10^(24)`

`6.02*10^(23)\:x = 1.69614*10^(26)`

`x = (1.69614*10^(26))/(6.02*10^(23))`

`\boxed{\boxed{x \approx 281.75\:grams}}\end{array}}\qquad\checkmark`

I Hope this helps, greetings ... DexteR! =)