00:01
There are multiple parts to this question with several calculations, some related to previous calculations, others not.
00:08
I'm not quite sure the purpose of this question, but it does require you to carry out several unit conversion calculations.
00:15
First, knowing the mass of a proton, a neutron, and an electron, you're asked to calculate the mass of a mole of protons, a mole of electrons, and a mole of electrons.
00:24
To do this, all you need to do is take the mass of a single one of these particles and multiply it by avogadro's number.
00:31
So we'll start with the electron.
00:34
We'll take the mass of a single electron, multiplied by avagadro's number, and we give 5 .486 times 10 to the negative 4 grams for a mole of electrons.
00:47
Now for protons, a mass of a proton is 1 .67 -262 times 10 to the negative 24 grams, multiplied by avagadro's number.
01:01
A mole of protons will be 1 .0073 grams.
01:07
A neutron has a mass a little bit greater than that of a proton.
01:12
So the mass of a mole of neutrons will be slightly greater than the mass of a mole of protons.
01:19
We'll take the mass of a neutron multiplied by avagadro's number, and we get something slightly larger, 1 .0086 grams for the mass of a mole of neutrons.
01:30
Then it gives us the mass of a single carbon 12 atom.
01:37
And to calculate the mass of a mole of carbon 12 atoms, we simply multiply by avogadro's number.
01:44
This should correspond exactly to 12 .000000, which it would if we had more significant figures for our avogadro's number and more significant figures for the mass of a single carbon 12...