Amount of Substance - Chapter 2
- Created by: 12BurtD
- Created on: 16-03-18 18:33
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- Amount of Substance
- Relative Atomic Mass
- Ar
- The average mass of an atom of an element (including isotopes) relative to 1/12 the Ar of Carbon-12
- Ar
- Relative Molecular Mass
- Mr
- The mass of a molecule compared to 1/12 the Ar of Carbon-12
- Relative Formula Mass
- Used for ions since they don't exist as Molecules
- Mr
- Avogadro Constant
- The number of atoms in 12g of Carbon-12
- The Mole
- The amount of a substance that contains Avogadro number of particles
- Equations
- n = m / Mr
- m - g n - mol
- n = cV
- n = cV / 1000
- c - mol dm^-3 V - cm^3
- c - mol dm^-3 V - dm^3
- n = cV / 1000
- PV = nRT
- P - Pa V - m^3 n - mol R - 8.31 T - K
- n = m / Mr
- Gas Laws
- Boyle's
- PV = constant
- Charles'
- V/T = constant
- Gay-Lussac's
- P/T = constant
- Boyle's
- 6.022x10^23
- Formulae
- Empiricle
- 1) Mass/%-age
- 2) Relative Mass
- 3) Moles
- 4) Divide by smallest
- 5) Make simplest ratio
- 4) Divide by smallest
- 3) Moles
- 2) Relative Mass
- 1) Mass/%-age
- Molecular
- Ar of Molecule / RM of empirical formula of molecule
- Empiricle
- Atom Economy
- (mass of desired products / total mass of reactants) x 100
- Percentage Yield
- (number of moles of specified product / theoretical max. moles of product) x 100
- Relative Atomic Mass
- Ar
- The average mass of an atom of an element (including isotopes) relative to 1/12 the Ar of Carbon-12
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