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59 Cards in this Set
- Front
- Back
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Give the Ammonia and Hydrogen Chloride test for diffusion |
Put cotton wool soaked in HCL on one side of the tube and cotton wool soaked in ammonia on the other. Ammonia diffuses quicker so the ammonium chloride will form closer to the HCL |
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Acid + metal = ? |
Salt + hydrogen |
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Name 2 ways of preventing rusting |
Galvanising and coating with plastic |
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How can you use copper to work out how much oxygen is in the air |
Fill a syringe with a recorded amount of air and heat copper inside the tube. Record the volume of air in the syringe again and whatever is missing is oxygen. |
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How can you make CO2 |
Add calcium carbonate to hydrochloric acid and collect the gas in a syringe |
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What colour is lithium in a flame test |
Crimson |
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What colour is potassium in a flame test |
Lilac |
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What colour is calcium in a flame test |
Brick red |
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What colour is sodium in a flame test |
Yellow |
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What colour precipitate does Copper 2 form with NaOH |
Blue |
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What colour precipitate does Iron 2 form with NaOH |
Sludgy green |
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What colour precipitate does Iron 3 form with NaOH |
Reddish brown |
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What does ammonia gas do to litmus paper |
Turns it from red to blue |
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How do you test for carbonates |
Add HCL to your solution and it will Give of CO2 if it is a carbonate |
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How do you test for sulfates |
Add HCL and barium chloride to your solution and it will form a white precipitate |
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How do you test for halides |
Add nitric acid and silver nitrate. Iodide turns yellow, bromide turns creamy and chloride turns white |
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How do you test for chlorine |
Add it to litmus paper and it bleaches |
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How do you test for oxygen |
Light and then put out a splint. Put it in the test tube and it'll relight if it is oxygen |
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How do you test for carbon dioxide |
Bubble it through lime water and it'll turn cloudy |
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How do you test for hydrogen |
Put a splint in it and it'll make a squeaky pop |
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General formula for alkanes |
CnH2n+2 |
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General formula for alkenes |
CnH2n |
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2 features of a homologous series |
Same physical properties Same chemical properties |
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Complete combustion equation |
Alkane + oxygen = CO2 + water |
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Incomplete combustion equation |
Alkane + oxygen = CO2 + water + CO + carbon |
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What feature of alkenes means they are unsaturated |
They can make more bonds due to their carbon double bond |
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Hydration of Ethene equation |
Phosphoric Acid 60 - 70 atm 300 degrees |
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Acid + metal oxide = ? |
Salt and water |
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Acid + metal carbonate = ? |
Salt and water and CO2 |
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How can you make a SOLUBLE salt |
Mix 2 substances with the required ions |
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How can you make an INSOLUBLE salt |
Add the metal carbonate, oxide or hydroxide to the acid. Filter. Evaporate. |
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Give the 3 steps in a titration calculation |
1- moles of substance you have (mol= conc × vol) 2- write out the equation for the reaction and work out moles of unknown substance 3- work out concentration of unknown stuff |
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Titration steps |
Add alkali and indicator to a conical flask. Fill a burette with acid. Add the acid to the alkali until the solution changes colour. Repeat. |
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Rate of reaction equation |
Product formed ÷ time taken |
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Name the 3 ways of measuring reaction speed |
Disappearing cross Change in mass Volume of gas given off |
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Exothermic |
Heat is given off. Increase in temperature. |
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Endothermic |
Heat taken in. Fall in temperature |
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Reduction definition |
Loss of oxygen |
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What is used to lower the temperature when extracting aluminium |
It is dissolved it molten cryolite |
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Describe fractional distillation |
Hot at bottom cool at top. Bubble caps. High melting point at bottom, low at top. |
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Conditions for cracking |
600-700 degrees Silica catalyst |
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Method of cracking |
Put the hydrocarbon and catalyst i a test tube connected by a delivery tube to a gas jar inverted in water. Heat the hydrocarbons then the catalyst, alternate between them. Alkanes collect in the gas jar. |
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How do you draw the repeat unit of a polymer |
Pick the part that is repeated |
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Give 2 uses of polymers |
Kettles and bags |
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Conditions for the haber process |
450 degrees 200 atm Iron catalyst |
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Diamond |
4 covalent bonds on each carbon Hardest substance |
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Giant ionic structure features |
Closely packed Strong bonds High MP and BP |
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Graphite |
3 covalent bonds on each carbon Layers Free electrons |
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Percentage yield |
Actual / theoretical |
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If H ions are present at the cathode... If the metal ions are less reactive... |
Hydrogen gas is formed Solid layer of the metal is formed |
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If OH and halide ions are present at the anode... If there are no halide ions... |
Halide molecules form Oxygen forms |
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Electrolysis calculation steps |
Balanced half equation for cathode Q=IT Q÷96000 Divide by number of electrons in half equation to get moles Mass=moles×Mr |
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Hydration of Ethene conditions |
300 degrees 60-70 atm Phosphoric acid |
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Molar enthalpy change steps |
Amount of energy transferred Moles=mass/Mr of thing produced Heat produced by 1 mole |
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Contact process conditions |
450 degrees 2 atm Vanadium Oxide |
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What is the contact process used for |
To make sulfuric acid |
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Steps of contact process |
Sulfur is burned in air Sulfur dioxide is oxidised Sulfur trioxide in dissolved in sulfuric acid Oleum diluted with water |
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How is brine electrolysed and what does it make |
Using a diaphram cell Makes Hydrogen (cathode), Chlorine (anode) and Sodium Ions (stays in solution) |
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Cathode and anode half equations of electrolysis of brine |
Cathode- 2H + 2e => H2 Anode- 2Cl => Cl2 +2e |
