What is the mass of a sample of pure gold containing 3.00 x 1024 gold atoms?

a. 981 g

b. 196.97 g

c. 39.5 g

d. 6.56 x 10^-23 g

e. 1.52 x 10^22 g

The mass is 980.6g of Gold.

Explanation:

We begin by looking for the number of moles equivalent to 3.0 x 10^24 gold atoms.

Using the Avogadro's number,

6.02 x 10^23 atoms of gold make up 1 mole of gold.

3.0 x 10^24 atoms would make up: 1 / 6.02 x 10^23 x 3.0 x 10^24 = 4.98moles.

Now that we know the number of moles, we can then look for the mass using the formular:

Moles = mass/ molar mass

4.98 = mass / 196.9 (atomic mass of gold)

Making "mass" the subject of formula : mass = 4.98 x 196.9= 980.6g

it is a good conductor

explanation: