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Chemistry > 1.2 Amounts Of Substance (part 1) > Flashcards

1.2 Amounts Of Substance (part 1) Flashcards

1
Q

Relative atomic mass

A

Weighted average mass of all the isotopes relative to 1/12th mass of an atom of carbon-12

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2
Q

Relative molecular mass

A

Mass of a molecule of the compound relative to 1/12th of the mass of an atom of carbon-12

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3
Q

Relative formula mass

A

Mass of one formula unit of an ionic compound relative to 1/12th mass of an atom of carbon-12

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4
Q

Mole

A

Amount of substance that contains as many particles as there are in exactly 12g of carbon-12

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5
Q

Avogadros constant

A
  1. 02x10 (to the power) 23

or. There are 6.02x10 (to the power) 23 atoms of carbon in 12g carbon-12

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6
Q

Does a mole of one substance contain the same number of particles as a mole of any other substance

A

Yes

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7
Q

What do you need to know to calculate moles in a solid

A

Mass

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8
Q

What do you need to calculate the number of moles in a gas

A

Volume

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9
Q

What do you need to know to calculate the number of moles in a solution

A

Volume and concentration

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10
Q

How do you get from Mg to mg

A

/1000

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11
Q

How to you get from mg to g

A

/1000

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12
Q

How do you get from Mg to g

A

/1000000

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13
Q

How to get from g to kg

A

/1000

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14
Q

How to get from kg to tonnes

A

/1000

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15
Q

How to get from g to tonnes

A

/1000000

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16
Q

How to get from tonnes to kg

A

X1000

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17
Q

How to get from kg to g

A

X1000

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18
Q

How to get from tonnes to g

A

X1000000

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19
Q

How to get from g to mg

A

X1000

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20
Q

How to get from mg to Mg

21
Q

How to get from g to Mg

22
Q

Formula for calculating moles in solids

A

Mass (in g) = moles x Mr

23
Q

How to calculate the number of atoms in a gives mass

A

First calculate number of moles using mass/Mr

Then calculate number of atoms using moles x avogadros constant

24
Q

How to get from centimetres cubed to decimetres cubed

25
Q

How to get from decimetres cubed to centimetres cubed

26
Q

What do you need to know in order to calculate the number of moles in a solution

A

Volume in demimetres cubed

Concentration in moles per decimetres cubed

27
Q

What is concentration

A

The number of moles of a solute dissolved in one decimetre cubed of solution

28
Q

What is the formula to work out the number of moles in a solution

A

Moles = volume x concentration

29
Q

How to calculate the concentration of a solution given the mass and volume

A 
Moles= mass/Mr
Concentration= moles/volume in decimetres cubed
30
Q

What are the assumptions made when using the ideal gas equation to

A
  • there are no intermolecular forces between the molecules

* the volume occupied by the molecules is entirely negligible relative to the volume of the container

31
Q

What is the ideal gas equation

32
Q

What unit is the answer always given in

A

Metres cubed

33
Q

What is pressure measured in

A

Pascals, Pa

34
Q

How to get from kPa to Pa

35
Q

How to get from MPa to Pa

36
Q

What is volume measured in

A

Metres cubed

37
Q

How to get from centimetres cubed to metres cubed

38
Q

How to get from decimetres cubed to metres cubed

39
Q

What is n

A

Number of moles

40
Q

What is R

A

Gas constant: 8.314

41
Q

What is T measured in

42
Q

How to get from Celsius to kelvin

43
Q

How to get from kelvin to Celsius

44
Q

What is density

A

It’s mass per unit volume

45
Q

Formula for density

A

Mass = density x volume

46
Q

What is density usually measured in

A

Grams per centimetre cubed

47
Q

Empirical formula

A

Simplest whole number ratio of atoms of each element present in a molecule

48
Q

Molecular formula

A

Actual number of atoms of each element present in a molecule

49
Q

How to calculate molecular formula

A

Calculate empirical formula
Calculate relative mass of empirical formula
Use Mr to calculate how many times bigger molecular formula needs to be compared to empirical
Times number of atoms by how many times bigger mr is than empirical formula mass

Chemistry (42 decks)

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