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Chemistry A Level > Amount Of Substance > Flashcards

Amount Of Substance Flashcards

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1
Q

Gold ion ?

A

Ag +

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2
Q

Zinc ion ?

A

Zn 2+

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3
Q

Nitride ion ?

A

N 3-

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4
Q

Sulphate (vi) ion ?

A

SO4 2-

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5
Q

Sulphate (iv) ion ?

A

SO3 2-

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6
Q

Nitrate ion ?

A

NO3 -

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7
Q

Carbonate ion ?

A

CO3 2-

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8
Q

Hydroxide ion ?

A

OH -

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9
Q

Ammonium ion ?

A

NH4 +

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10
Q

Hydrogen carbonate ion ?

A

HCO3 -

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11
Q

Phosphate ion ?

A

PO4 3-

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12
Q

Nitride ion ?

A

N 3-

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13
Q

Ammonia chemical formula ?

A

NH3

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14
Q

Silica chemical formula ?

A

SiO2

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15
Q

Substance + oxygen ?

A

Oxides

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16
Q

Metal + water ?

A

Metal hydroxide + hydrogen

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17
Q

Metal + acid ?

A

Salt + hydrogen

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18
Q

Metal oxide + acid ?

A

Salt + water

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19
Q

Metal hydroxide + acid ?

A

Salt + water

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20
Q

Metal carbonate + acid ?

A

Salt + water + carbon dioxide

21
Q

Metal hydrogencarbonate + acid ?

A

Salt + water + carbon dioxide

22
Q

Ammonia + acid ?

A

Ammonium salt

23
Q

Metal carbonate (thermal decomposition) ?

A

Metal oxide + carbon dioxide

24
Q

1 ton in grams ?

A

1,000,000g

25
Q

1 kg in g ?

A

1000g

26
Q

1 mg in g ?

A

0.001g

27
Q

How would you calculate the number of moles of O atoms in CO2 ?

A
  1. Calculate moles of CO2 using mass/mr
  2. Multiply moles by the number of atoms of oxygen in the molecule (2)
28
Q

What is avogadro’s constant ?

A

Number of particles in a mole
(6.02x10^23)

29
Q

What is a mole ?

A

The amount of substance that has the same number of particles as there are atoms in 12g of C12 (avogadro’s constant)

Can be applied to electrons, atoms, molecules, ions, formulas etc.

30
Q

What is the relative atomic mass ?

A

Mean mass of an atom of an element compared to 1/12 the mass of a C12 atom

31
Q

What is the relative molecular/formula mass ?

A

Mean mass of a molecule/formula unit of a substance compared to 1/12 the mass of a C12 atom

-formula refers to ions in an ionic compound
-molecular refers to atoms in a covalent compound

32
Q

What is percentage yield ?

A

It is the ratio of the actual mass obtained during an experiment compared to the highest theoretical yield. (based on the amount of substance that you have)

33
Q

What is percentage yield dependant on ?

A

The conditions of the reaction, meaning that if we change the conditions to favour the reaction, we can maximise the yield.

34
Q

Why may we not get 100% percentage yield ?

A
  1. An alternative reaction occurs, forming another product and less of our theoretical product
  2. The reaction is reversible, so reaction does not reach completion
  3. Product is lost during separation from the reaction mixture
35
Q

What is atom economy ?

A

A measure of how many of the reactant atoms from the reagent form the useful product(s), taking into account any byproducts

36
Q

What is the formula for atom economy ?

A

total Mr of useful product(s) / total Mr of reactants
(total Mr in this scenario is calculated through the Mr of the formula x any balancing numbers)

37
Q

How can we improve atom economy ?

A

It can only become higher in a certain reaction if we can find profitable uses for the “waste” products

38
Q

What is empirical formulae ?

A

Found from practical data, it is the simplest ratio of atoms in a compound

39
Q

How do we work out the empirical formula ?

A
  1. Separate all of the elements in the formula unit into their elements
  2. Write out the %mass/mass of each element
  3. Divide each of the masses by the Mr of the element
  4. Divide all of the moles by the smallest mole
  5. Find out the smallest whole integer ratio of all of the elements
  6. Write out the formula with the number of each element
40
Q

What is molecular formulae ?

A

The actual number of atoms in each element in a compound (more useful for us to use during calculations)

41
Q

How can we work out the molecular formula ?

A

Given Mr of the molecular formula / Mr of the empirical formula. We then multiply all of the numbers in front of each element by the number from the above calculation

42
Q

What is the formula for working out concentration ? Include units

A

Concentration (g/dm3) = mass (g) / volume (dm3)

Concentration (mol/dm3) = moles (mol) / volume (dm3)

43
Q

What is the conversion for m3, cm3 and dm3 ?

A

m3 -> dm3 (x1000)
dm3 -> cm3 (x1000)

44
Q

What factors are the volume of gases dependant on ?

A

Temperature (directly proportional)
Pressure (inversely proportional)
Number of moles (directly proportional)

45
Q

What factors are the pressure of gases dependant on ?

A

Temperature (directly proportional)
Number of moles (directly proportional)

46
Q

What is the ideal gas equation ?

A

pV = nRT

where :
p = pressure (pascals)
V = volume (m3)
n = number of moles (mol)
R = gas constant
T = temperature (Kelvin)

47
Q

What is the gas constant value ?

A

8.314 KJ-1mol-1

48
Q

Why do we use Kelvin for temperature ?

A

As an substance may be a gas at a negative temperature. This would give us negative solutions, which are incorrect so Kelvin is used as it is absolute.

49
Q

What is the conversion from degrees Celsius to Kelvin ?

A

degrees Celsius + 273 (273 is absolute zero, so the Kelvin scale starts from this value)

Chemistry A Level (3 decks)

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