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17 Cards in this Set
- Front
- Back
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Relative atomic mass |
The average mass of an atom of an element taking into account its naturally accruing isotopes compared to 1/12th of carbon-12. |
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Relative molecular mass |
The relative molecular mass of a molecule compared to 1/12th of carbon-12. |
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Avogadro constant |
The amount of atoms in in one gram of hydrogen 6.022*10^23 |
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The mole |
One mole is the amount of substance that has 6.022*10^23 atoms |
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Avogadro constant definition |
Avogadro constant or Avogadro number is the atoms in 12 grams of carbon -12 |
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One mole volume |
22.4 at standard STP temperature 273k 100 KPa. |
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Moles equation |
Number of moles = mass\mr |
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No. Of moles at STP |
Volume in dm-3 /22.4 litres= No.moles |
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Ideal gas equation |
PV=NRT. P= pressure V= volume N= moles. R= 8.31. T=temperature |
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PV=NRT units and conversion |
Pressure in pa or pascals. KPa =*1000 Volume in M-3 Cm-3 to m-3= *10^-6 N moles R T in kelvin Degrees to k = +273 |
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Work out concentration |
C=no.Of moles / volume in dm-3 |
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Convert cm-3 to dm-3. |
1dm-3= 1000cm-3 so divide by 1000 |
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Volumetric analysis |
Remember times by ten for actual because of 25 to 250 |
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Empirical formula |
The simplest ratio of atoms of each element on a compound. Find percentage divide by the Mr of each find the smallest then divide all by this number. |
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Molecular formula |
Shows the exact amount of atoms of each element in one compound |
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Percentage yield |
%yield= actual yield of product /maximum yield of product |
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%atom economy= mass desired product/ total mass reactants. |
Atom economy |
