Question

What is the mass, in grams, of a sample of 1.20 × 1022 atoms of mercury (Hg)? Show your work or explain the steps that you used to determine your answer.

Answer 1

Look up the atomic mass of Hg.
What is it?

Answer 2

200.59 u ± 0.02 u

Answer 3

Ok. Use 200.59.
That means 1 mole of Hg has a mass of 200.59 g.
Do you know how many atoms are in a mole?

Answer 4

Sorry, but gtg.

Answer 5

This is what you need to do.
The atomic mass of an element is the number of grams per mole for that element.
In other words, the atomic mass of an element is the mass of one mole of the element.
For mercury, it is 200.59.
1 mole of mercury has a mass of 200.59 g.
Avogadro's number tells you how many atoms are in a mole.
Avogadro's number is 6.02 * 10^23
That means that 1 mole of Hg, which is 6.02 * 10^23 atoms of mercury, has a mass of 200.59 g.
You don't have 6.02 * 10^23 atoms of mercury.
You have fewer atoms. You only have 1.20 * 10^22 atoms.
Find what fraction of Avogadro's number 1.20 * 10^22 by dividing 1.20 * 10^22 by Avogadro's number.
Then multiply that by the atomic mass of Hg, 200.59
That will give you the mass of 1.20 * 10^22 atoms of Hg.

Answer 6

Bye

Answer 7

sorry i never responded openstudy wasn't working for me but thank you

Answer 8

yw