1. Mass Of 1 Mole Of Electron Used
2. Mass Of 1 Mole Of Electron Gas

One electron (e−) has a mass of 9.10938291 x 10−31kg. One mole of e− is 6.022 x 1023e−. Aug 07, 2017 Mass of one mole of electron = (6.022 × 10 23) × (9.10939 ×10 –31 kg) = 5.48 × 10 –7 kg Charge on one electron = 1.6022 × 10 –19 coulomb Charge on one mole of electron = (1.6022 × 10 –19 C) (6.022 × 10 23). 1 electron weighs approximately 9.11×10−31 Kg 1 mol weighs X Kg 1 mol is6.022×1023 particles So we put 6.022×1023 in the equation instead. How many moles of electrons weigh one kilogram? (mass of electron = 9.108 × 10−31 kg, Avogadro number = 6.023 × 1023)A: 6.023 × 1023 B: 1/9.108 × 1031 C. Aug 13, 2020 Answers: The mass of one mole of electron is 0.55.

How many electrons in ONE MOLE of carbon dioxide?

3 Answers

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

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

Fonera ip address. #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

Mass Of 1 Mole Of Electron Used

#'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))))#

Mass Of 1 Mole Of Electron Gas

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

Explanation:

First, we calculate the number of electrons in ONE MOLECULE of #CO_2#. Tricare select copay 2021. 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......?'#

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