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Physical Chemistry Flashcards

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1
Q

What PH does the strongest acid have?

A

0PH

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2
Q

What PH does the strongest alkali have?

A

14PH

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3
Q

What PH is neutral (water)

A

7PH

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4
Q

What does an indicator do?

A

Change colour to show the PH of a solution

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5
Q

What colours does universal indicator show?

A

Acidic: Red
Neutral: Green
Alkali: Purple

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6
Q

What colours does litmus paper show?

A

Acidic: Red
Neutral: Purple
Alkali: blue

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7
Q

What colours does phenolphthalein show?

A

Acidic: Colourless
Alkaline: Pink

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8
Q

What colours does Methyl orange show?

A

Acidic: red
Alkaline: yellow

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9
Q

What’s an acid?

A

Source of hydrogen ions (H+) with a PH less than 7

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10
Q

What’s a base?

A

A substance which can neutralise an acid

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11
Q

What’s an alkali?

A

Soluble base with a source of hydroxide ions, (OH-) and PH greater than 7

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12
Q

What’s a neutralisation reaction?

A

Acid + Base = salt + water, or H+ + OH- = H2O

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13
Q

What PH are the products after a neutralisation reaction?

A

7 neutral

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14
Q

What’s the equation when an acid and a metal oxide react?

A

Acid + metal oxide = Salt + water

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15
Q

If the acid is hydrochloric acid what will the metal salt be?

A

A chloride

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16
Q

If the acid is Sulphuric acid what will the metal salt be?

A

A sulphate

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17
Q

If the acid is Nitric acid what will the metal salt be?

A

A nitrate

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18
Q

What’s the equation for an acid and a metal Carbonate?

A

Acid + Metal Carbonate = Salt + water + Carbon dioxide

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19
Q

What does soluble mean?

A

Can dissolve in water

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20
Q

What does insoluble mean?

A

Can’t dissolve in water

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21
Q

Which salts are soluble?

A

All except carbonates (few exceptions)

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22
Q

How do you make a soluble salt with an acid and an insoluble base?

A

Mix the acid (Nitric acid), and insoluble base (copper carbonate) They will produce crystals, filter and evaporate them

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23
Q

How do you make an insoluble salt?

A

A precipitation reaction

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24
Q

What’s a precipitation reaction?

A

Mixing 2 solutions with ions you require, to make an insoluble salt and eg barium chloride + Sulphuric acid= Barium Sulphate + hydrochloric acid

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25
Q

What are titrations used for?

A

To find out how much acid is needed to neutralise an alkali (or vice versa)

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26
Q

Method for a titration?

A

Add alkali to a conical flask with an indicator

Put acid in a burette and add to the alkali until there’s the required colour change, and measure how much was used

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27
Q

How to work out the concentration from a titration calculation?

A

Work out the moles of the substance you have
Write the equation for the reaction, and compare the ratio to work out the amount of moles in unknown substance
Work out the concentration of the unknown stuff

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28
Q

What’s a slow reaction?

A

Rusting

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29
Q

What’s a moderate reaction?

A

Magnesium reacting with acid

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30
Q

What’s a fast reaction?

A

An explosion

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31
Q

What does the rate of reaction depend on?

A

Temperature
Concentration (or pressure for gasses)
Catalyst
Size of particles (surface area)

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32
Q

Formula for rate of reaction?

A

Rate of reaction= Amount of reactant used or amount of product formed / Time

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33
Q

What’s the precipitation method of measuring a rate of reaction?

A

When the product is a precipitate which clouds a solution and you measure how long until you can’t see through the solution

34
Q

What’s the change in mass method of measuring a rate of reaction?

A

Place the reaction on scales and measure how the mass drops as the reaction goes on

35
Q

What’s the measuring volume of gas given off method in measuring the rate of reaction?

A

Use a gas syringe to measure the amount of gas given off during the reaction

36
Q

What’s a way of proving that bigger surface area means faster reaction?

A

React hydrochloric acid with marble chips, with different size chips, and notice the smaller chips produce more gas

37
Q

Why does a larger surface area increase the rate of reaction?

A

More frequent collisions

38
Q

What’s a method to prove that a higher concentration of acid increases the rate of reaction?

A

React magnesium metal with dilute HCL, and see when the acid is a higher concentration the mass drops down faster

39
Q

How to show how temperature effects the rate of reaction?

A

Sodium Thiosulfate and HCL produce a cloudy precipitate, so see how long it takes until you can’t see through the flask

40
Q

How to show how a catalyst effects the rate of reaction?

A

Via the decomposition of hydrogen peroxide into water, add manganese to see it increase the rate of reaction

41
Q

What’s collision theory?

A

States that the rate of reaction, depends on how hard and how often the reacting particles collide

42
Q

How does a higher temperature increase the rate of reaction?

A

Particles have more energy so move quicker, so they collide more often

43
Q

How does a Higher concentration ( or pressure) increase the rate of reaction?

A

Particles closer together so the important particles will collide and react more often

44
Q

How does a larger surface area increase the rate of reaction?

A

The particles will have more area to react with, so there will be more successful collisions

45
Q

How does a catalyst increase the rate of reaction?

A

Gives the reacting particles an area to stick to

Increasing the successful collisions by lowering the activation energy

46
Q

What causes faster collisions?

A

Hot temperature

47
Q

Why does a hot temperature cause faster collisions and more successful ones?

A

Particles have more energy so move faster, and have enough energy to make the reaction happen

48
Q

What happens in a chemical reaction?

A

Old bonds broken, new bonds made

49
Q

What process is bond breaking?

A

Endothermic, as energy is supplied to make the bonds

50
Q

What process is bond making?

A

Exothermic as energy is released when new bonds are formed

51
Q

What’s an exothermic reaction?

A

Gives out energy, in the form of heat, shown by a rise of temperature in the surroundings

So the bond formation is energy is greater than bond breaking energy

52
Q

What’s an endothermic reaction?

A

Takes in energy, in the form of heat, shown by a fall of temperature in the surroundings

So the bond formation is energy is smaller than bond breaking energy

53
Q

What’s the overall change in energy in a reaction called?

A

The enthalpy change ( Delta H)

54
Q

What unit is Delta H?

A

kj/mol

55
Q

If Delta H is Negative then the reaction is?

A

Exothermic as heat is given out

56
Q

If Delta H is positive then the reaction is?

A

Endothermic, as heat is taken in

57
Q

Pointers for Exothermic reaction graph?

A

Reactants higher than products
Difference in height shows energy change
The initial shows the activation energy

58
Q

What’s the activation energy?

A

The energy required to break the old bonds

59
Q

Pointers for an endothermic graph?

A

Reactants lower than products

Difference in height shows energy change

60
Q

What are the axis on an energy level diagram?

A 
X= Progress of reaction
Y= Energy
61
Q

How do catalysts reduce the activation energy?

A

They give an alternative reaction pathway

62
Q

What’s the formula for finding enthalpy change?

A

Enthalpy change Delta H = Total energy absorbed breaking bonds - total energy released making bonds

63
Q

Method for finding the Enthalpy change?

A

Draw out the molecules already there and the molecules made, and using the table work out the total energies

Use enthalpy change equation

64
Q

Experiment to work out enthalpy change?

A

Calorimetry

65
Q

What’s calorimetry used to work out energy transferred in neutralisation, dissolving and displacement reactions
?

A

Measure the heat of the reagents, then the heat of the solution, whilst insulating it

66
Q

What’s combustion calorimetry?

A

Burn a fuel to see how much fuel it takes to heat water to 50C

Use copper can, and reduce draughts to make it more accurate

67
Q

Equation for energy transferred, in calorimetry?

A

Energy transferred (joules) = mass of water g x temp change C x 4.2 (energy to heat 1 g of water by 1C)

68
Q

Method for working out energy transferred?

A

Work out all the things required for the energy transferred equation

Use the energy transferred equation

Work out the mass of fuel used, and work out how much energy whatever mass of the fuel produces

69
Q

What’s the molar enthalpy change?

A

The enthalpy change given out by one mole of the reactant

70
Q

How to work out the molar enthalpy change?

A

Calculate the amount of energy transferred
Work out the moles of fuel produced the heat by using the mass and Mr
Then divide the energy change (if it was exothermic this number will be negative) by the amount of moles to find the Kj/mol

71
Q

What’s a reversible reaction?

A

Where the products of one reaction, can themselves react to make the original reactents

72
Q

What’s an example of a reversible reaction?

A

Thermal decomposition of ammonia chloride (S)

Breaks down to make ammonia (G) and hydrogen (G) chloride

Which can then re form to make ammonia chloride

73
Q

What’s dynamic equilibrium?

A

Where the forward and backward reactions are equal so the overall effect is nil, happens in a closed sytem (no product can escape)

74
Q

What are all reactions in directions?

A

Endothermic one way, endothermic the other way

75
Q

How does increasing the temperature effect the reaction?

A

Endothermic increases to use extra heat up

76
Q

How does reducing the temperature effect the reaction?

A

Exothermic increases to give more heat out

77
Q

What’s the position of equilibrium?

A

The relative amount of products and reactents

78
Q

What do all gaseous reactions have?

A

More molecules on one side than the other

79
Q

How does raising the pressure effect the reaction?

A

Encourages the reaction which produces fewer molecules of gas

80
Q

How does decreasing the pressure effect the reaction?

A

Encourages the reaction which produces more molecules of gas

Chemistry (9 decks)

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