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igcse chemistry > stoichiometry > Flashcards

stoichiometry Flashcards

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1
Q
A
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2
Q

What is relative atomic mass (Ar)?

A

average mass of naturally occurring atoms of an element on a scale where the 12C atom has a mass of exactly 12 units

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2
Q

What is relative atomic mass (Ar)?

A

average mass of naturally occurring atoms of an element on a scale where the 12C atom has a mass of exactly 12 units

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3
Q

What is relative molecular mass? (Mr)

A

sum of the relative atomic masses

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4
Q

What is relative formula mass?

A

Relative molecular mass for ionic compounds

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5
Q

How can solution concentrations be expressed?

A

mol/dm3 or g/dm3

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6
Q

Moles =

A

Concentration x Volume

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7
Q

What is a mole?

A

the number of particles which is equal to the number of atoms in 12g of carbon 12

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8
Q

What is Avogadro’s constant? (3)

A

number of particles / atoms / ions / molecules in one mole of a substance the number of particles / molecules in 24dm3 of a gas at RTP

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9
Q

What is the number of particles in 24 dm3 of a gas at RTP?

A

6 to 6.0^23 × 10^23 atoms (Avogadro’s constant)

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10
Q

no. of moles =

A

mass of substance taken/mass of one mole of substance

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11
Q

What is the limiting reactant?

A

the one that is not in excess

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12
Q

How can we calculate the limiting reactant?

A

Calculate which reactant has the lower number of moles

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13
Q

Excess of substance =

A

moles of substance at start - moles of substance at end

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14
Q

n =

A

M/mr

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15
Q

concentration =

A

number of moles / volume

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16
Q

volume of gas (in dm3) =

A

number of moles x 24

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17
Q

% by mass of element in compound =

A

sum of Mr/ relative formula mass of compound x 100

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18
Q

% yield =

A

actual yield/predicted yield x 100

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19
Q

% purity =

A

mass of pure product/mass of impure product x 100

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20
Q

What are the 6 formulas you need to know?

A

.

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21
Q

What is relative molecular mass? (Mr)

A

sum of the relative atomic masses

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22
Q

What are the 6 formulas you need to know?

A

.

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23
Q

% purity =

A

mass of pure product/mass of impure product x 100

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24
Q

% yield =

A

actual yield/predicted yield x 100

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25
Q

% by mass of element in compound =

A

sum of Mr/ relative formula mass of compound x 100

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26
Q

volume of gas (in dm3) =

A

number of moles x 24

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27
Q

concentration =

A

number of moles / volume

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28
Q

n =

A

M/mr

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29
Q

Excess of substance =

A

moles of substance at start - moles of substance at end

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30
Q

How can we calculate the limiting reactant?

A

Calculate which reactant has the lower number of moles

31
Q

What is the limiting reactant?

A

the one that is not in excess

32
Q

no. of moles =

A

mass of substance taken/mass of one mole of substance

33
Q

What is the number of particles in 24 dm3 of a gas at RTP?

A

6 to 6.0^23 × 10^23 atoms (Avogadro’s constant)

34
Q

What is Avogadro’s constant? (3)

A

number of particles / atoms / ions / molecules in one mole of a substance the number of particles / molecules in 24dm3 of a gas at RTP

35
Q

What is a mole?

A

the number of particles which is equal to the number of atoms in 12g of carbon 12

36
Q

Moles =

A

Concentration x Volume

37
Q

How can solution concentrations be expressed?

A

mol/dm3 or g/dm3

38
Q

What is relative formula mass?

A

Relative molecular mass for ionic compounds

39
Q

What is relative molecular mass? (Mr)

A

sum of the relative atomic masses

40
Q

What is relative formula mass?

A

Relative molecular mass for ionic compounds

41
Q

How can solution concentrations be expressed?

A

mol/dm3 or g/dm3

42
Q

Moles =

A

Concentration x Volume

43
Q

What is a mole?

A

the number of particles which is equal to the number of atoms in 12g of carbon 12

44
Q

What is Avogadro’s constant? (3)

A

number of particles / atoms / ions / molecules in one mole of a substance the number of particles / molecules in 24dm3 of a gas at RTP

45
Q

What is the number of particles in 24 dm3 of a gas at RTP?

A

6 to 6.0^23 × 10^23 atoms (Avogadro’s constant)

46
Q

no. of moles =

A

mass of substance taken/mass of one mole of substance

47
Q

What are the 6 formulas you need to know?

A

.

48
Q

% purity =

A

mass of pure product/mass of impure product x 100

49
Q

% yield =

A

actual yield/predicted yield x 100

50
Q

% by mass of element in compound =

A

sum of Mr/ relative formula mass of compound x 100

51
Q

volume of gas (in dm3) =

A

number of moles x 24

52
Q

concentration =

A

number of moles / volume

53
Q

n =

A

M/mr

54
Q

Excess of substance =

A

moles of substance at start - moles of substance at end

55
Q

How can we calculate the limiting reactant?

A

Calculate which reactant has the lower number of moles

56
Q

What is the limiting reactant?

A

the one that is not in excess

57
Q

What is relative atomic mass (Ar)?

A

average mass of naturally occurring atoms of an element on a scale where the 12C atom has a mass of exactly 12 units

58
Q

What are the 6 formulas you need to know?

A

.

59
Q

% purity =

A

mass of pure product/mass of impure product x 100

60
Q

% yield =

A

actual yield/predicted yield x 100

61
Q

% by mass of element in compound =

A

sum of Mr/ relative formula mass of compound x 100

62
Q

volume of gas (in dm3) =

A

number of moles x 24

63
Q

concentration =

A

number of moles / volume

64
Q

n =

A

M/mr

65
Q

Excess of substance =

A

moles of substance at start - moles of substance at end

66
Q

How can we calculate the limiting reactant?

A

Calculate which reactant has the lower number of moles

67
Q

What is the limiting reactant?

A

the one that is not in excess

68
Q

no. of moles =

A

mass of substance taken/mass of one mole of substance

69
Q

What is the number of particles in 24 dm3 of a gas at RTP?

A

6 to 6.0^23 × 10^23 atoms (Avogadro’s constant)

70
Q

What is Avogadro’s constant? (3)

A

number of particles / atoms / ions / molecules in one mole of a substance the number of particles / molecules in 24dm3 of a gas at RTP

71
Q

What is a mole?

A

the number of particles which is equal to the number of atoms in 12g of carbon 12

72
Q

Moles =

A

Concentration x Volume

73
Q

How can solution concentrations be expressed?

A

mol/dm3 or g/dm3

74
Q

What is relative formula mass?

A

Relative molecular mass for ionic compounds

75
Q

What is relative molecular mass? (Mr)

A

sum of the relative atomic masses

76
Q

What is relative atomic mass (Ar)?

A

average mass of naturally occurring atoms of an element on a scale where the 12C atom has a mass of exactly 12 units

igcse chemistry (14 decks)

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