Question

How many electrons in ONE MOLE of carbon dioxide?

Answer 1

first calculate moles of `CO2`

Explanation:

first calculate the moles of `CO2` = 100/44
= 2.27 mol
now number of electrons in `CO2` are obtained by adding total electrons in each of the three atoms i.e. two O and one C = 6+8+8
= 22
thus one mole of `CO2` has `22 * 6.022 * 10^23` electrons and 2.27 mol has `2.27 * 22 * 6.022 * 10^23` electrons = `301.1 * 10^23` electrons

Answer 2

`3 * 10^(25)`

Explanation:

The first thing to do here is to calculate the number of moles of carbon dioxide present in your sample. To do that, use the compound's molar mass

`100 color(red)(cancel(color(black)("g"))) * "1 mole CO"_2/(44.0color(red)(cancel(color(black)("g")))) = "2.27 moles CO"_2`

Next, use Avogadro's constant to figure out the number of molecules of carbon dioxide present in the sample.

`2.27 color(red)(cancel(color(black)("moles CO"_2))) * (6.022 * 10^(23)color(white)(.)"molecules CO"_2)/(1color(red)(cancel(color(black)("mole CO"_2))))`

`=1.37 * 10^(24)` `"molecules CO"_2`

Now, every molecule of carbon dioxide contains

• one atom of carbon, `1 xx "C"`
• two atoms of oxygen, `2 xx "O"`

This means that your sample contains

`1.37 * 10^(24)color(red)(cancel(color(black)("molecules CO"_2))) * "1 atom C"/(1color(red)(cancel(color(black)("molecule CO"_2))))`

`= 1.38 * 10^(24)` `"atoms of C"`

and

`1.37 * 10^(24) color(red)(cancel(color(black)("molecules CO"_2))) * "2 atoms O"/(1 color(red)(cancel(color(black)("molecule CO"_2))))`

`= 2.74 * 10^(24)` `"atoms of O"`

Next, grab a periodic Table and look for the atomic numbers of the two elements. You will find

`"For C: " Z = 6`

`"For O: " Z = 8`

As you know, a neutral atom has equal numbers of protons located inside its nucleus and electrons surrounding the nucleus.

Therefore, you can say that every atom of carbon will contain `6` electrons and every atom of oxygen will contain `8` electrons.

This means that you will have

`"total no. of e"^(-) = overbrace(6 * 1.37 * 10^(24))^(color(blue)("coming from C atoms")) + overbrace(8 * 2.74 * 10^(24))^(color(purple)("coming from O atoms"))`

`"total no. of e"^(-) = (8.22 + 21.92) * 10^(24)`

which gets you

`color(darkgreen)(ul(color(black)("total no. of e"^(-) = 3 * 10^(25))))`

The answer must be rounded to one significant figure, the number of sig figs you have for the mass of carbon dioxide.

Answer 3

Approx. `3xx10^25` `"electrons........"`

Explanation:

First, we calculate the number of electrons in ONE MOLECULE of `CO_2`. There is ONE CARBON ATOM, that is 6 electrons; and TWO OXYGEN ATOMS, that is 16 electrons, i.e. 22 electrons per molecule.

And then we calculate the number of carbon dioxide molecules in a mass of `100*g` of gas. How do we do this? We use the mole as a counting unit, i.e. `6.022xx10^23` molecules of `CO_2` have a mass of `(12.01+2xx15.999)*g*mol^-1=44.0*g*mol^-1`

`"Moles of carbon dioxide"` `=` `(100*g)/(44.01*g*mol^-1)=2.27*mol`.

And (finally) we solve the product:

`22xx(100*g)/(44.01*g*mol^-1)xx6.022xx10^23*"electrons"*mol^-1=`

`"how many electrons...........?"`