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CHEMISTRY FURTHER ADDITIONAL > 3b > Flashcards

3b Flashcards

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1
Q

How ‘many’ is a mole?

A

6.023 x10 to the power of 23

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2
Q

What is the concentration of a solution measured in?

A

Moles per dm3 (i.e. moles per litre)

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3
Q

What is the formula for concentration?

A

Concentration = moles / volume

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4
Q

What are the two formulas you can use to work out number of moles?

A

Number of moles = concentration x volume

Number of moles = mass / RFM

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5
Q

How can you measure the amount of energy released by a chemical reaction and what can you do to prevent the amount of energy lost to surroundings?

A

Taking the temperature of the reagents, mixing them in a polystyrene cup and measuring the temperature of the solution at the end of the reaction. Reduce energy lost to surroundings by putting the polystyrene cup into a beaker of cotton wool to give more insulation and putting a lid on the cup to reduce energy lost by evaporation

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6
Q

What is an exothermic reaction?

A

One which gives out energy to the surroundings, usually in the form of heat and usually shown by a rise in temperature

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7
Q

What is an endothermic reaction?

A

One which takes in energy from the surroundings, usually in the form of heat and usually shown by a fall in temperature

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8
Q

Is energy supplied or released in the breaking of existing bonds- is it endothermic or exothermic?

A

Energy must be supplied to break existing bonds- so bond breaking is an endothermic process

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9
Q

Is energy supplied or released when new bonds are formed- is it endothermic or exothermic?

A

Energy is released when new bonds are formed- so bond forming is an exothermic process

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10
Q

In an endothermic reaction, which is greater the energy required to break old bonds or the energy released when new bonds are formed?

A

The energy required to break old bonds is greater

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11
Q

In an exothermic reaction, which is greater the energy required to break old bonds or the energy released when new bonds are formed?

A

The energy released in bond formation

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12
Q

How is fuel energy calculated?

A

Calorimetry

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13
Q

What is the experiment for Calorimetry?

A

Water in copper can, record temp, weigh spirit burner & lid, spirit burner underneath can, heat water until 50ºc measure temp again weigh spirit burner again (with lid)

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14
Q

In exothermic reactions, is the energy change -ve or +ve?

A

Negative

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15
Q

In endothermic reactions, is the energy change -ve or +ve?

A

Positive

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16
Q

What happens to the activation energy in the presence of a catalyst?

A

The activation energy is lower

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17
Q

Is the reaction between hydrogen and water exothermic or endothermic?

A

Exothermic

18
Q

What are the two ways you can use hydrogen as a fuel?

A

Burning it in an engine or by using it in a fuel cell

19
Q

Hydrogen gas is burnt in oxygen as a fuel in the combustion engines of vehicles, name one pro and two cons of this

A

Only forms water so is very clean however you need a special and expensive engine and hydrogen is very hard to store

20
Q

What is a fuel cell?

A

A fuel cell is an electrical cell thats supplied with a fuel and oxygen and uses energy from the reaction between them to generate electricity

21
Q

Does a fuel cell run down or need recharging?

A

No, it’ll produce energy in the for, of electricity and heat as long as fuel is supplied

22
Q

Why couldn’t fuel cells completely replace conventional petrol/diesel engines?

A

Hydrogen is a gas and so takes up more space to store, very explosive so difficult to store safely, hydrogen fuel made from hydrocarbons with needs fossil fuels or electrolysis

23
Q

What kind of ions do metals always make?

A

Positive

24
Q

What colour flame does Lithium give?

A

Crimson flame

25
Q

What colour flame does Sodium give?

A

Yellow flame

26
Q

What colour flame does Potassium give?

A

Lilac flame

27
Q

What colour flame does Calcium give?

A

Red flame

28
Q

What colour flame does Barium give?

A

Green flame

29
Q

What do some metal ions form with NaOH?

A

A coloured precipitate

30
Q

What is the colour of the precipitate for Calcium?

A

White

31
Q

What is the colour of the precipitate for Copper(II)?

A

Blue

32
Q

What is the colour of the precipitate for Iron(II)?

A

Green

33
Q

What is the colour of the precipitate for Iron(III)?

A

Brown

34
Q

What is the colour of the precipitate for Aluminium?

A

White at first then redissolves in excess NaOH to form a colourless solution

35
Q

What is the colour of the precipitate for Magnesium?

A

White

36
Q

How can you test for carbon dioxide?

A

Bubbling it through limewater. If the gas present is carbon dioxide, the limewater turns cloudy

37
Q

What is another way that you can use the carbon dioxide test?

A

To test for carbonate ions since carbonates react with dilute acids to form carbon dioxide

38
Q

Acid + carbonate —> ?

A

Acid + carbonate —> Salt + water + carbon dioxide

39
Q

How can you test for Halide ions (chloride, bromide and iodide ions)?

A

Add dilute nitric acid followed by silver nitrate solution

40
Q

In the testing for Halides, what colour is the precipitate for chloride, bromide and iodide?

A 
Chloride = white precipitate of silver chloride
Bromide = cream precipitate of silver bromide
Iodide = yellow precipitate of silver iodide
41
Q

How can you test for a sulfate ion?

A

Add dilute HCl, followed by barium chloride solution, a white precipitate of barium sulphate means the original compound was a sulfate

42
Q

Name a suitable indicator you could use in the titration of sulfuric acid and sodium hydroxide

A

Phenolphthalein, universal indicator doesn’t show the definite colour change

CHEMISTRY FURTHER ADDITIONAL (2 decks)

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