How To Use Moles - Part 2 | Chemical Calculations | Chemistry | FuseSchool
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8 سال پیش
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Carry on learning about using
Carry on learning about using moles in this part 2 of 3 parts.
Avogradro’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.
The molecular mass of a compound is found by adding up the atomic masses ofall the elements that make it, multiplied by the number of times each atom appears.
Moles say only how many particles there are, not how much is in them.
The molecular mass units are grams per mole. We can work outhow many moles we have by putting in the mass and rearranging.
In chemistry, we use moles to work out how much of each reactant to weigh out.This means we can make sure we get enough product and none of the reactants are wasted. It also makes it easier to get the product pure.
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This video is part of 'Chemistry for All' - a Chemistry Education project by our Charity Fuse Foundation - the organisation behind The Fuse School. These videos can be used in a flipped classroom model or as a revision aid. Find our other Chemistry videos here:
CHEMISTRY
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This Open Educational Resource is free of charge, under a Creative Commons License: Attribution-NonCommercial CC BY-NC ( View License Deed: http://creativecommons.org/licenses/b... ). You are allowed to download the video for nonprofit, educational use. If you would like to modify the video, please contact us: [email protected]
Avogradro’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.
The molecular mass of a compound is found by adding up the atomic masses ofall the elements that make it, multiplied by the number of times each atom appears.
Moles say only how many particles there are, not how much is in them.
The molecular mass units are grams per mole. We can work outhow many moles we have by putting in the mass and rearranging.
In chemistry, we use moles to work out how much of each reactant to weigh out.This means we can make sure we get enough product and none of the reactants are wasted. It also makes it easier to get the product pure.
SUBSCRIBE to the Fuse School YouTube channel for many more educational videos. Our teachers and animators come together to make fun & easy-to-understand videos in Chemistry, Biology, Physics, Maths & ICT.
JOIN our platform at www.fuseschool.org
This video is part of 'Chemistry for All' - a Chemistry Education project by our Charity Fuse Foundation - the organisation behind The Fuse School. These videos can be used in a flipped classroom model or as a revision aid. Find our other Chemistry videos here:
CHEMISTRY
Twitter: Twitter: fuseSchool
Access a deeper Learning Experience in the Fuse School platform and app: www.fuseschool.org
Follow us: fuseschool
Friend us: Facebook: fuseschool
This Open Educational Resource is free of charge, under a Creative Commons License: Attribution-NonCommercial CC BY-NC ( View License Deed: http://creativecommons.org/licenses/b... ). You are allowed to download the video for nonprofit, educational use. If you would like to modify the video, please contact us: [email protected]
8 سال پیش
در تاریخ 1395/01/25 منتشر شده
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