Difference between revisions of "Mole"
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Number of [[Mole]]s of an [[Element]] = ([[Mass]] of [[Element]])/([[Relative Atomic Mass]] of [[Element]]) | Number of [[Mole]]s of an [[Element]] = ([[Mass]] of [[Element]])/([[Relative Atomic Mass]] of [[Element]]) | ||
| − | Number of [[Mole]]s = <math>{\frac{ | + | Number of [[Mole]]s = <math>{\frac{m}{A_r}}</math> |
Where: | Where: | ||
| − | + | m = The [[mass]] of [[element]] being used. | |
A<sub>r</sub> = The [[Relative Atomic Mass]] of the [[Element]] | A<sub>r</sub> = The [[Relative Atomic Mass]] of the [[Element]] | ||
| Line 21: | Line 21: | ||
Number of [[Mole]]s of a [[Compound]] = ([[Mass]] of [[compound]])/([[Relative Formula Mass]] of [[compound]]) | Number of [[Mole]]s of a [[Compound]] = ([[Mass]] of [[compound]])/([[Relative Formula Mass]] of [[compound]]) | ||
| − | Number of [[Mole]]s = <math>{\frac{ | + | Number of [[Mole]]s = <math>{\frac{m}{M_r}}</math> |
Where: | Where: | ||
| − | + | m = The [[mass]] of [[compound]] being used. | |
M<sub>r</sub> = The [[Relative Formula Mass]] of the [[compound]] | M<sub>r</sub> = The [[Relative Formula Mass]] of the [[compound]] | ||
Revision as of 18:09, 2 January 2019
Key Stage 4
Meaning
A mole is an SI Unit used to show 6.02x1023 particles of a chemical.
About Moles
- Moles are based on the number of Carbon atoms in exactly 0.012kg (12g) of Carbon.
- Moles are used to give a conversion between the number of atoms in a substance and useful quantities for chemical reactions. It would not be useful to talk about 1,000,000,000 atoms in a chemical reaction because that would be such a small amount of the chemical (0.0000000000000017g).
- The relative atomic mass of an element is the mass of 1 mole or the mass of 6.02x1023 atoms. So 1g of Hydrogen is 1 mole and contains 6.02x1023 atoms. 235g of Uranium-235 is 1 mole and contains 6.02x1023 atoms.
Calculating Moles
Number of Moles of an Element = (Mass of Element)/(Relative Atomic Mass of Element)
Number of Moles = \({\frac{m}{A_r}}\)
Where:
m = The mass of element being used.
Ar = The Relative Atomic Mass of the Element
Number of Moles of a Compound = (Mass of compound)/(Relative Formula Mass of compound)
Number of Moles = \({\frac{m}{M_r}}\)
Where:
m = The mass of compound being used.
Mr = The Relative Formula Mass of the compound