Question

How many atoms are in 85.1 grams of neon?
help ppl I need steps I am so confused

Answer 1

Given weight of Neon \((\mathsf{Ne})\) = 85.1 grams.

Molar mass of Ne = 20 grams.

Since no. of moles (n) = \(\cfrac{\textbf{Given weight}}{\textbf{Molar Mass}} \)

So, no. of moles (n) of Neon = \(\cfrac{85.1}{20} \) = \(4.255\)

Now, use the following formula :

\(\textbf{No. of particles in the entity } =\bf{ n \times N_A }\)

Where : n = no. of moles
\(N_A\) = Avogadro's number = \(\large 6.022 \times 10^{23} \)

So, you get : \(\textbf{No. of atoms in Neon} = 4.255 \times 6.022 \times 10^{23}\)

Solve it further.

Answer 2

If you need further clarification, I just explained a step by step process to someone else: http://openstudy.com/study#/updates/51ad25d8e4b06ee3ee25b0c9

Answer 3

Although I think @Thoughts did a great job explaining.

Answer 4

Thanks @abb0t . And really, good work there (in the link)