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a level chemistry - physical chemistry > 3.1.2 Amount Of Substances > Flashcards

3.1.2 Amount Of Substances Flashcards

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1
Q

Equation moles avogadro’s constant particles

A

Number of particles = Number of moles x Avogadro’s constant
Particles can be ions electrons atoms molecules etc

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2
Q

Equation moles , mass , Mr

A

Moles = Mass/Mr

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3
Q

How many particles is 1 mole

A

6.02 x 10^23

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4
Q

Equation Mass/ Moles, Concentration, Volume

A

Moles/Mass = Concentration x volume (dm^3)

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5
Q

What is the ideal gas equation + units

A

pV=nRT
p- pressure (Pa)
V- volume m3
n- number of moles
R - gas constant ( 8.31 JK^-1 mol^-1)
T p- temperature Kelvin

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6
Q

What is the name of this equation pV=nRT

A

The IDEAL gas equation

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7
Q

How to convert KPa into Pa

A

X 1000

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8
Q

How to convert between degrees and kelvin

A

0=273 kelvin
Just add onto both
E.g.
25= 273 + 25
25= 298

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9
Q

How to convert dm3 to m3

A

Divide by x10^3

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10
Q

Describe how to make a volumetric solution

A

Stage 1
Weight sample in weighing boat in mass balance
Transfers to beaker
Re weight record mass difference

Stage 2
Add deionised water
Stir with a glass rod
Until solid has dissolved

Stage 3
Transfers to volumetric flask with a 250cm^3 marking
With washings fill up to 250cm^3 mark
Invert flask

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11
Q

What is theoretical yield

A

Is the mass of product that can be formed assuming no chemical are lost in the process

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12
Q

Theoretical yield equation

A

Moles x Mr

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13
Q

In atom economy is the big number used

A

YES

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14
Q

Atom economy equation

A

Mr of desired product / sum of Mr of ALL products

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15
Q

Define relative molecular mass

A

Mass of 1 atom of carbon 12

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16
Q

Define molecular formula

A

Number of atoms of each element in a molecule

17
Q

Define empirical formula

A

Simplest ratio of atoms of each element

18
Q

Does empirical formula have to be not whole numbers?

A

NO
MUST BE WHOLE NUMBER

19
Q

Why is the percentage yield not 100%

A
  • other reactions took place simultaneously
  • the reaction does not go to completion
  • reactants or products are lost to the atmosphere
20
Q

Define meaning of mole

A

Avogadro’s number of molecules

21
Q

Define relative atomic mass

A

The average mass of an atom of an element when compared with 1/12th of the mass of an atom of carbon 12

22
Q

Formula of sulphur

A

S8

23
Q

For any acid formula what element is always present

A

Hydrogen

24
Q

The student rinses the burette with deionised water before filling with sodium hydroxide solution. State and explain the effect, in any, that rinsing will have on the value of the titre.

A

The titre value would increase because the sodium hydroxide solution would be dilute

25
Q

What units for percentage yield equation moles or grams

A

Both

26
Q

Percentage yield equasion

A

% Yield = yield /max theoretical yield

27
Q

Which compound would require the greatest amount of oxygen for complete combustion of 1 mole of the compound

A

The one with the highest ration of carbon to oxygen atoms. They require more oxygen to combine with those carbons and can’t utilise the oxygen within its structure as much

28
Q

% uncertainty equasion

A

= ( Uncertainty/ mass added) x100

29
Q

% uncertainty equasion

A

= ( Uncertainty/ mass added) x100

30
Q

Why is percentage yield important

A

Getting as much product from the reaction as possible

31
Q

Why is percentage atom economy important

A

The maximum amount of atoms end up in the desired product

32
Q

Formula of anything hydroxide

A

X OH

33
Q

Give a reason why bond enthalpy found is different to bond enthalpy in data book

A

Data book value derived from different compounds

34
Q

Percenatge uncertainty equation

A

Uncertainty/ measurement x100

35
Q

Reactivity down group 2

A

Increases

a level chemistry - physical chemistry (8 decks)

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