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14 Cards in this Set
- Front
- Back
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Mole |
The amount of substance in grams that has the same number of particles as there are atoms in 12 grams of carbon-12 |
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Relative atomic mass |
Weighted mean mass of an atom compared to one twelfth of an atom of carbon-12 |
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Molar mass |
Mass in grams of 1 mole of a substance (g/mol) |
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Avogadro's constant |
No. of particles = number of moles × avogadro's constant 6.02 × 10^23 |
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Number of moles equation |
n = m / Mr n = number of moles m = mass (g) Mr = molar mass |
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Empirical formula |
Simplest ratio of atoms of each element in a compound 1) find the n = m / Mr 2) divide each answer by the smallest 3)find the ratio |
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Molecular formula |
Actual number of atoms of eacg element in a compound 1)find the empirical formula 2)calculate the Mr of empirical formula 3) divide actual Mr by empirical Mr (= whole number) 4)multiple empirical formula a certain number of times |
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Hydrated salts |
A hydrated salt contains water of crysrallisation (water in the crystalline structure) 1)calculate the n (= m / Mr) 2)divide water by n of substance to get ratio |
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Gases |
At RTP one mole of gas occupies 24dm^3 (24000 cm^3) |
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Ideal gas equation |
pV= nRT p=pressure V=volume (m^3) n= No. Of moles R= Ideal gas constant (8.314 DATA SHEET) T= temperature (K) |
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Ideal gas equation assumptions |
•gases are in constant, random, straight line motion •all of their collisions are elastic (no energy lost) •volume of particles is negligible •no intermolecular forces |
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Moles ratio |
1)write moles ratio on a balanced equation 2)calculate the number of moles 3)multiply by moles ratio 4)convert into quantity relevant to question |
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Percentage yield |
%yield = (actual yield / theoretical yield) ×100 |
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Atom economy |
Take into account number in front if substances (Sum of Mr of desired products / sum of Mr of all products) × 100 |
