Quantative Chemistry
- Created by: CharlotteStyles
- Created on: 26-10-16 14:05
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- Quantative Chemistry
- Relative Formula Mass
- All of the relative atomic masses added together
- How heavy an atom is compared with the mass of an atom of carbon 12 - usually the mass number
- One mole
- Number of moles is the mass in g/Mr
- All of the relative atomic masses added together
- Percentage by mass
- At x number of atoms / Mr x100
- Empirical Formula
- Simplest ratio of the number of atoms in the molecule
- 1) list all elemnts in compound
- 2) write percentage over relative formula/atomic mass
- 3) use the answer of the first fraction to get 1 then use the answer to the 2nd fraction over the answer to the 1st fraction
- This will give you the ratio, simplify if needed
- 3) use the answer of the first fraction to get 1 then use the answer to the 2nd fraction over the answer to the 1st fraction
- 2) write percentage over relative formula/atomic mass
- Calculating Masses
- 1) write out the balanced equation
- 2) write the molar ratio
- 3) use the formula n=m/mr
- 4) substitute into the molar ratio
- 5) rearrange the equation to get the mass
- 4) substitute into the molar ratio
- 3) use the formula n=m/mr
- 2) write the molar ratio
- 1) write out the balanced equation
- Percentage yield
- Shows the overall success of the experiment
- percentage yield = amount of product produced / minimum amount of product possible x100
- Amount of product you get is the yield
- Why you don't get 100% yield
- impurities in reaction
- other products being producd
- residue loss to surroundings
- reversible reactions
- reaction can go both ways, never converted to products
- Why you don't get 100% yield
- Shows the overall success of the experiment
- Relative Formula Mass
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