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62 Cards in this Set
- Front
- Back
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Molar Mass |
Relative atomic masses of each element added in a molecule |
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Moles No. Equation |
Mass / Molar Mass |
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The total mass of reactants before a reaction are the same as the total mass after a reaction. This is because no ______ are created or destroyed during the reaction |
Atoms |
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Thermal Decomposition Reaction |
One substance breaks down to form two or more other substances using heat |
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Factors Affecting the Mass of the Product |
Can be greater if a gas has been gained from the air Lost if water vapour or gas has escaped |
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Copper Oxide + Hydrogen --------> (And Conditions) |
Copper + Water Copper must be hot Hydrogen must be burned off to make it safe |
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Percentage of An Element in a Molecule Equation |
Mass of element/ Mass of molecule x 100 |
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Method of Working Out the Empirical Formula |
1) Write each element 2) Write each element's mass 3) Right each element's molar mass 4) Find the number of moles (Mass/Molar Mass) 5) Divide each by smallest result 6) Intergers written into formula |
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Measurements for the Volume of Liquids |
Cm3-Cubic Centimetres dm3-Cubic Decimetres 1dm3 = 1000cm3 = 1 litre |
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Measurements for the Concentration of a Solution |
g/dm3 (grams per cubic decimetre) mol/dm3 (moles per cubic decimetre) |
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Examples of when Dilution is Used |
Too dilute medicine won't work properly Too concentrated medicine might increase illness Incorrect dilution of babies milk may harm the baby
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Concentration Equation |
Concentration = Mole/Volume |
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Volume of Water to Add Equation |
((Starting concentration / target concentration) -1) x Starting Volume |
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Sodium in 1g of Salt |
O.39g |
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Neutralisation Reaction |
Acid + Alkali -------> Salt + Water |
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Equipment Used in a Neutralisation Reaction |
Burette used to add the alkali Pipette used to measure the alkali using a pipette filler Conical Flask for the reaction to take place in
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End Point |
When the acid and alkali neutralise each other |
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Phenolphthalein (Colours in Acid and Alkali) |
Pink in Alkali Colourless in Acid |
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Litmus (Colours in Acid and Alkali) |
Blue in Alkali Red in Acid |
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Universal Indicator (Colours in Acid and Alkali) |
Contains several different indicators Displays a gradual change of colour, giving a more evident pH No. Not helpful in seeing the exact end point |
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Titre |
The amount of alkali used to neutralise an acid |
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Sodium Azide Reaction Products |
Sodium + Nitrogen |
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Gas Syringe |
Gas-tight glass syringe that usually measures a volume of 100cm3 |
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Measuring Gas Volumes |
Upturned measuring Cylinder in water connected to a delivering tube from the reaction. The gas from the reaction will collect in the cylinder to make the volume measurable. |
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Magnesium + Hydrochloric Acid ------> |
Magnesium Chloride + Hydgrogen |
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Limiting Reactant |
The reactant that runs out first stops the whole reaction, making it the limiting reactant. |
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Moles of Gas = |
Volume of Gas/Molar Volume |
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Reversible Reactions |
When a reaction can take place forward and backwards |
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Equilibrium |
When the rate of the forward reaction is equal to the rate of the backwards reaction When the amount of product is equal to the amount of reactants, equilibrium will be reached One will be exothermic, the other will be endothermic Closed System |
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Position of the Equilibrium |
If there is more reactants than products, the equilibrium is on the left If there is more products than reactants, the equilibrium is on the right |
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Pressure Changes and Equilibrium |
If the pressure increases, the equilibrium moves to the side with the lower amount of gas molecules |
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Temperature Changes and Equilibrium |
If the temperature increases, the equilibrium will move in the direction of the endothermic reaction as it will take in the heat. The reaction will speed up as the particles are receiving more energy with the excess heat. |
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Uses of Sulfuric Acid |
Fertilisers Chemicals Processing Metal Ores Paper Production Oil Refining Making Polymers |
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Raw Materials in the Contact Process |
Sulfur Water Oxygen |
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Stage One of the Contact Process (With Symbol Equation) |
Sulfur burned in air to produce sulfur dioxide S + O2 -------> SO2 |
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Stage Two of the Contact Process (With Symbol Equation) |
Sulfur dioxide and oxygen react to produce sulfur trioxide 2SO2 + O2 ------> 2SO3 Reversible reaction |
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Stage Three of The Contact Process (With Symbol Equation) |
SO3 + H2O --------> H2SO4 |
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Conditions of The Contact Process |
Vanadium Oxide (V3O5) 450 degrees (forward reaction is exothermic (greater yield achieved by a lower temperature) but the reaction would be too slow at a lower temperature)-Compromise Atmospheric Pressure
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Ionisation in Strong Acids |
Strong acids ionise completely in solution to produce H+ Ions |
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Ionisation in Weak Acids |
Weak Acids only partly ionise in solution, many molecules not producing H+ Ions Reaction is reversible |
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Solutions Containing Ions in Electrolysis (The role of Ions) |
Ions are free to move and so carry the electricity from on electrode to the other. Acids containing H+ Ions therefore conduct electricity |
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Electrical Conductivity |
Stronger acids have a higher electrical conductivity as they produce more H+ Ions then weaker acids, allowing more electricity to be conducted by the ions |
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Limescale |
Deposit of Calcium Carbonate that coats the surface of different appliances that require a heating element |
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Getting Rid of Limescale |
Weak acids will react with the limescale, removing it, without damaging the appliance |
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Reaction Rate in Strong and Weak Acids |
Strong acids have a quicker reaction rate as they have more H+ ions which fully ionise in solution Weak acids have a slower reaction rate due to less H+ ions to ionise |
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Volume of Gas Production in Weak Acids |
The same as strong acids as the equilibrium will eventually change, releasing more H+ ions to continue the reaction. The reaction rate is slower but the amount of gas produced is the same. |
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Precipitation Reaction |
When two different solutions form together to form a solid precipitate. |
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Lead Nitrate + Pottasium Iodide |
Potassium Nitrate + Lead Iodide |
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Collision Frequency for Ions in Solution |
As ions are free to move when in solution, collision frequency is very fast. The reaction is really fast. |
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(s) |
Solid |
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(g) |
Gas |
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(aq) |
Aqueous |
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(l) |
Liquid |
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Creation of an Insoluble Salt |
1) Suitable combination of solutions mixed together to create an insoluble precipitate 2) Mixture is filtered out and separated from the other substances 3) Precipitate is washed with water and dried with heat |
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Uses of Barium Sulfate |
X-rays pass through it with difficulty so patients needing an x-ray image of their digestive system would digest Barium Sulfate to create an image of the area |
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Creation of Barium Sulfate |
Barium Chloride + Sodium Sulfate ---> Barium Sulfate + Sodium Chloride |
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Testing for Sulfate Ions |
White precipitate forms with the addition of hydrochloric acid |
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Chloride Ions Precipitate |
White Precipitate |
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Bromide Ions Precipitate |
Cream Couloured Precipitate |
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Iodide Ions Precipitate |
Yellow Precipitate |
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Testing for Halide Ions |
Colour of halide precipitate is formed with the addition of nitric acid |
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Spectator Ions |
Ions that are present but not involved in the actual reaction |
