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Chemistry OCR A-Level > Chapter 3 > Flashcards

Chapter 3 Flashcards

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1
Q

How are chemicals measured?

A

1) mass

2) volume

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2
Q

What is one mole?

A

The amount of a substance that contains 6.02x10^23 particles

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3
Q

What is the Avogadro constant?

A

6.01x10²³, the number of particles in each mole of carbon-12

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4
Q

What is the mass of one mole of carbon, C?

A

12.0g

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5
Q

What is the mass of one mole of hydrogen, H?

A

1.0g

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6
Q

What is molar mass, M?

A

The mass per mole of a substance

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7
Q

What are the units of molar mass?

A

g mol^-1

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8
Q

amount, n =

A

mass, m / molar mass, M

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9
Q

What is a molecule?

A

Two or more atoms held together by covalent bonds

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10
Q

What is molecular formula?

A

The number of atoms of each element in a molecule

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11
Q

What is empirical formula?

A

The simplest whole-number ratio of atoms of each element in a compound

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12
Q

What is relative molecular mass, Mr?

A

The comparison of the mass of a molecule with the mass of an atom of carbon-12

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13
Q

What is relative formula mass?

A

The comparison of the mass of a formula unit with the mass of an atom of carbon-12

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14
Q

How do you calculate relative formula mass?

A

By adding together the relative atomic masses of the elements in the empirical formula

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15
Q

How do you calculate relative molecular mass?

A

By adding together relative molecular masses of the elements making up a molecule

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16
Q

What does it mean when crystals are hydrated?

A

Water molecules are part of their crystalline structure

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17
Q

What is water of crystallisation?

A

Water molecules that are bonded into a crystalline structure of a compound

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18
Q

What is the formula of the reaction where hydrated copper(II) sulfate is heated?

A

CuSO₄•5H₂O(s) → CuSO₄(s) + 5H₂O(l)

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19
Q

What would happen if there was no water in copper(II) sulfate?

A

1) the crystalline structure would be lost

2) a white powder would remain

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20
Q

What are the 2 assumptions made when determining that an experimental formula is accurate?

A

1) all of the water has been lost

2) no further decomposition

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21
Q

What does it mean when the hydrated and anhydrous forms have different colours?

A

You can be fairly sure when all of the water has been removed

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22
Q

How can you check that all water has been removed?

A

Heat to constant mass - repeatedly reheat until the mass of the residue no longer changes

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23
Q

How are liquids and gases measured?

A

By volume

24
Q

How do you measure the mass of a solution or a gas?

A

Convert the volume into amount of substance, in moles to be able to count the particles present

25
Q

What is 1cm³ in ml?

A

1ml

26
Q

What is 1dm³ in cm³?

A

1000cm³

27
Q

What is 1dm³ in ml?

A

1000ml

28
Q

What is 1dm³ in l?

A

1l

29
Q

n =

A

c x V

30
Q

What is a standard solution?

A

A solution of known concentration

31
Q

How are standard solutions prepared?

A

1) dissolving an exact mass of the solute in a solvent

2) making up the solution to an exact volume

32
Q

What are the units for mass concentration?

A

gdm⁻³

33
Q

What is the molar gas volume Vₘ?

A

The volume per mole of gas molecules at a stated temperature and pressure

34
Q

What is RTP?

A

1) 20°C

2) 101kPa (1 atm) pressure

35
Q

At RTP, what volume does 1 mole of gas molecules have?

A

24.0dm³ = 24000cm³

36
Q

What is the molar gas volume at RTP?

A

24.0 dm³mol⁻¹

37
Q

amount n (mol) =

A

volume V / molar gas volume Vₘ

38
Q

When V is in dm³ n =

A

V(dm³) / 24.0

39
Q

When V is in cm³ n =

A

V(cm³) / 24000

40
Q

What are the assumption for the molecules making up an ideal gas?

A

1) random motion
2) elastic collisions
3) negligible size
4) no intermolecular forces

41
Q

What is the ideal gas equation?

A

pV = nRT

42
Q

pV =

A

nRT

43
Q

What is the value of R in the ideal gas equation?

A

8.314Jmol⁻¹K⁻¹

44
Q

What are the units of temperature in the ideal gas equation?

A

K

45
Q

What is absolute zero?

A

-273°C

46
Q

What are the units of pressure in the ideal gas equation?

A

Pa

47
Q

What are the units of volume in the ideal gas equation?

A

m³

48
Q

How do you convert from cm³ to m³?

A

x 10⁻⁶

49
Q

How do you convert from dm³ to m³?

A

x 10⁻³

50
Q

How do you convert from °C to K?

A

+273

51
Q

How do you convert from KPa to Pa?

A

x 10³

52
Q

What is the stoichiometry of a reaction?

A

The balancing numbers which give the ration of the amount, in moles, of each substance

53
Q

What are balanced equations used to find?

A

1) the quantities of reactant required to prepare a required quantity of a product
2) the quantities of products that should be formed from certain quantities of reactants

54
Q

What is an advantage of reactions with high atom economies?

A

1) produce a large proportion of desired products and few unwanted waste products
2) are important for sustainability as they make the best use of natural resources

55
Q

What are the effects of improving atom economy?

A

1) makes industrial process more efficient
2) preserves raw materials
3) reduces waste

Chemistry OCR A-Level (28 decks)

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