Question

A closed container has 6.08 ⋅ 1023 atoms of a gas. Each atom of the gas weighs 1.67 ⋅ 10–24 grams. Which of the following shows and explains the approximate total mass, in grams, of all the atoms of the gas in the container?

Answer 1

`10.1536*  10^(-1)\approx 1.02` grams.

Explanation:

We have been given that a closed container has
`6.08* 10^(23)` atoms of a gas. Each atom of the gas weighs
`1.67* 10^(-24)` grams.

To find the total mass, in grams, of all the atoms of the gas in the container, we will multiply number of atoms with mass of each atom.

`\text{Total mass}=6.08* 10^(23)* 1.67* 10^(-24)`

Using exponent property
`a^b* a^c=a^(b+c)`, we will get:

`\text{Total mass}=6.08* 1.67*  10^(23)* 10^(-24)`

`\text{Total mass}=10.1536*  10^(23+(-24))`

`\text{Total mass}=10.1536*  10^(-1)`

`\text{Total mass}=10.1536*(1)/(10)`

`\text{Total mass}=1.01536`

`\text{Total mass}\approx 1.02`

Therefore, the approximate total mass, in grams, of all the atoms of the gas in the container is
`10.1536*  10^(-1)\approx 1.02` grams.

Answer 2

Total mass = 6.08 x 10^23 * 1.67 x 10^-24 = 1.01536