3.1.2 Amount of substance Flashcards

1
Q

The mole

A

The amount of substance in grams that has the same amount

of particles as there are atoms in 12g of carbon-12

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2
Q

Relative Atomic Mass (Ar)

A

The average mass of an atom compared to 1/12 the mass of

an atom of carbon-12

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3
Q

Relative Molecular Mass (Mr)

A

The average mass of a molecule compared to 1/12 the mass

of an atom of carbon-12

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4
Q

Relative Formula Mass (RFM)

A

The average mass of an ionic compound compared to 1/12

the mass of an atom of carbon-12

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5
Q

Avogadro’s Constant

A

The number of particles in one mole

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6
Q

Avogadro’s Number

A

6.022 * 10^23

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7
Q

Molar Equations: M, Mr, n

A
Mass = moles * Mr
Mr = mass/moles (n)
Moles = Mass/Mr
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8
Q

Molar Equations: n, c, v

A
Moles = concentration * volume
Concentration = moles/volume
Volume = moles/concentration
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9
Q

Converting Volumes

A

Volumes must be converted to dm^3

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10
Q

cm^3 to dm^3

A

(cm^3/1000)

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11
Q

dm^3 to cm^3

A

(dm^3 * 1000)

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12
Q

Molar Equations: number of particles, n, avogadro’s number

A

Number of Particles = moles * l (l is avogadro’s number)
Moles = Number of particles/l
l= Number of particles/moles

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13
Q

Empirical Formula

A

The simplest whole number ratio of atoms of each element in

a compound

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14
Q

How to work out Emp. Formula

A

-Find n of elements by dividing mass by Mr
-Divide each mole value by the smallest one to determine the
ratio
-Determine the whole number ratio of each element

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15
Q

Water of Crystallisation

A
  • Find mass of water by subtracting anhydrous from hydrated
  • Find moles of anhydrous substance (use mass/Mr)
  • Find moles of water (use Mass/Mr)
  • Determine the ratio
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16
Q

Molecular Formula

A

-Determine the number of empirical formula units that can fit
into the Mr (Mr Molecular formula / Mr Empirical Formula)
-Multiply the empirical formula by the units

17
Q

Percentage Yield

A

Actual Yield/Theoretic Yield * 100

18
Q

Percentage Atom Economy

A

Mass of useful products / mass of all reactants * 100

19
Q

Ideal Gas Equation: What is it?

20
Q

Ideal Gas Equation: Conversion of Pressure (kPa - Pa)

A

100kPa = 100,000 Pa

21
Q

Ideal Gas Equation: Conversion of Volume (dm^3/cm^3 to

m^3)

A

cm^3 to m^3 = x/1000000

dm^3 to m^3 = x/1000

22
Q

Ideal Gas Equation: Conversion of Temperature (degrees

Celsius to Kelvin & Kelvin to degrees Celsius)

A

x (degrees Celsius) + 273 = K

x (K) - 273 = degrees Celsius

23
Q

Cations

A

Ions with a positive charge

24
Q

Anions

A

Ions with a negative charge

25
State Symbols: (s)
Solid
26
State Symbols: (l)
Liquid
27
State Symbols: (g)
Gaseous
28
State Symbols: (aq)
Aqueous/dissolved in water
29
State Symbols
Must be included in every chemical equation
30
Spectator Ions
Ions that stay in the same state throughout the equation. You can cancel these out if they come up.