How To Use Moles - Part 1 | Chemical Calculations | Chemistry | FuseSchool

Learn the basics about using moles. This is part 1 of 3 parts, teaching you about using moles, as a part of the chemical calculations topic.
Avogadro’s number describes what is known as 1 mole, or 12 g of carbon atoms. This is used in chemical calculations.
For any element, the relative atomic mass is the weight in grams for one mole.
When we compare chemicals, we compare equal numbers of particles, even though the weights are different. So if we have compounds instead of atoms, it doesn’t matter how many atoms are in the formula, only the number of compound particles.
For any compound, the relative molecular mass (or Mr) is the weight in grams for one mole, or Avogadro's Number.
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[@minyu2903]

1:50 there are 2 mole of iron for every 1 "PARTICLE" ? Well there are 2 particle of iron for every one particle. If there is 1 mole of compound so there are 2 mole . Mole and particle are not the same because 1 mole of gase is 6.023×10^23 particle.

[@geoffrjjjjjjj]

atomic number of sulfur at :40 should be 16, not 12.

[@fuseschool]

+Geoffrey Ritchey good spot - thank you for letting us know.

[@TheEncyclopaedia]

what is the software used in designing this lesson please ?? I think it is not Power point

[@fuseschool]

Our designers use the adobe creative cloud package.

[@fatimapeaceful]

Yall just go to tyler Dewitt's videos, he's a life saver. I can bet he can calrify your doubts at least 50% if not all

[@zak5972]

oh yes, im here too

[@Afewwilliams]

you should really be using "mass" instead of "weight" on these videos!

[@baladeivanai6941]

Yes... I was thinking abt it!