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Physics And Chemistry 2024 Year 10 > C4-Quantitive Chemistry > Flashcards

C4-Quantitive Chemistry Flashcards

1
Q

What is the conservation of mass

A

The law of conservation of mass states that no atoms are lost or made during a chemical reaction so the mass of the products equals the mass of the reactants.

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2
Q

What is the limiting reactant

A

The reactant that is completely used up since it limits the amount of products formed

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3
Q

What is a mole

A

The mole is the unit for amount of substance. The symbol for the unit mole is mol.

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4
Q

What is a relative formula mass

A

The sum of the relative atomic masses of the atoms in the numbers shown in the formula.

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5
Q

What is the percentage yield

A

The percentage ratio of the actual yield of product from a reaction compared with the theoretical yield.

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6
Q

What is concentration

A

The amount of substance in a certain volume of solution

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7
Q

What is the actual yoeld

A

Amount of product actually produced by a feaction

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8
Q

What is atom economy

A

The measure of the amount of starting materials that end up as useful products

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9
Q

What is the theoretical yield

A

The maximum amount of product that could be produced from the given reactants assuming a complete reaction takes place

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10
Q

How to get the relative formula mass

A

Its mass number added to another

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11
Q

How to calculate the % mass of an element in a compound

A

Relative atomic mass x number of atoms of that element/relative formula mass times 100

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12
Q

Example to find the % mass of an element in a compound. Na2CO3.Finding sodium in it

A

Ar of sodium=23 Ar of carbon=12. Ar of oxygen=16
Relative formula mass=(2x23)+12+(3x16)=106
23x2/106 x100=43%

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13
Q

A mixture contains 20% iron irons by mass.What mass of iron chloride (Fecl2) would you need to provide the iron ions in 50g of the mixture? Example

A

Ar of Fe=56 Ar of cl=35.5
Mixutre of ion contains=10g of iron
56/56(2x35.5) x100=44.09%
10/44.09/100=23 g

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14
Q

What is percentage composition also know as?

A

Percentage mass

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15
Q

How to calculate relative atomic mass

A

Its a numbers mass number

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16
Q

How to calculate the number of moles

A

Mass in g (of an element or compound) / Ar or Mr(of the element or compound)

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17
Q

What is avogardos constant

A

the number of atoms, molecules, or ions in a mole of any substance (i.e., 6.02 × 10-23 per mol)

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18
Q

What is titration

A

a method for measuring the volumes of two solutions that react together

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19
Q

What is the end point

A

the point in a titration where the reaction is complete and titration should stop

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20
Q

What is burette

A

a long glass tube with a tap at one end and markings to show volumes of liquid; used to add precisely known volumes of liquids to a solution in a conical flask below it

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21
Q

What is the concordant

A

when you have two titration results that are within 0.1cm3 of each other. These precise results can then be used to
calculate an accurate mean

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22
Q

What is a bulb pipette

A

a glass tube used to measure accurate volumes of liquids

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23
Q

What is uncertainty

A

Range of measurements each side of the mean

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24
Q

How to calculate uncertainty

A

Calculate mean and then calculate range and the difference is the uncertainty.Make sure before you always add a +/-

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25
Q

What is the mass of 1 mole equal to

A

The mass of 1 mole of a substance is equal to its relative formula mass or atomic mass in grams

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26
Q

What does a balanced equation show

A

Shows reacting moles of each substance(as the simplest whole number ratio)

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27
Q

How to calculate the maxiumum mass of a substance

A

Step 1. note what you know and what to calculate - you can ignore the other substances
Ignore the big numbers for the moment - we will use them later
Step 2. Calculate the moles of the substance that you know the mass of
Step 3. Use the ratio of moles from the balanced equation to work out the number of moles of the substance with unknown mass ratio of moles is 2: 2
So there will be 0.675 moles of MgO as well
Rearrange and calculate the answer

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28
Q

We can only work out the limting reactant if we know

A

-Number of moles that react in a experiment
-Balanced formula equation

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29
Q

How to measure concentration

A

Measured in g/dm^3 or mol/dm^3

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30
Q

What does 1dm3 equals

A

1000 cm3

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31
Q

How to calculate concentration

A

Mass/volume

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32
Q

How to calculate mass

A

Concentration x volume

33
Q

Calculation to calculate moles

A

Concentration x volume

34
Q

In a chemical reaction why do we not always obtain the mass of the product calculated

A

Gases from the air may react with the chemicals in the beaker, increasing the mass.
Gaseous products may escape from the beaker into the air, decreasing the mass.

35
Q

What is the yield

A

The amount of product obtained in a chemical reaction

36
Q

How to calculate percentage yield

A

Mass of product actually made/max theoretical mass of product x100

37
Q

Example question-Zinc reacts with copper sulfate to produce 30g of copper.The theoretical yield of copper is 35g.Calculate the percentage yield

A

Percentage yield=30/35 x100
85.7%

38
Q

Why is high atom economy important

A

Contributes to sustainable development
Saves costs

39
Q

How to calculate atom economy

A

Relative formula mass of desired product/Sum of the relative formula mass of all reactants in the equation X100

40
Q

How to calculate volumes of gasses

A

Mass of gas/relative formula mass x 24

41
Q

Value for avogadros constant

A

6.02 x 10^23

42
Q

If the amount of solute in a solution is increased what happens to its concentration

43
Q

If the volume of water in a solution is increased what happens to its concentration

44
Q

How should solution be added from the burette close to the end point

A

Drop by drop,swirling in between

45
Q

Why is a white tile used in titratiom

A

See colour change better

46
Q

What is a titre

A

Volume of solution added from thr burette

47
Q

What volume does one mole of any gas occupy at room temperature and pressure?

A

24dm^3 or 24000 cm3

48
Q

How do we know usually if there is a gas

A

If the mass seems to change

49
Q

Explanation of when the mass increases

A

If the mass increases its probably because one of the reactants is a gas that is found in air and all the products are solid liquids or aqueous.

50
Q

when a mass increases what happens

A

Before the reaction the gas is floating around in the air.Its there but its not contained in the reaction vessel,so you cant account for its mass
When the gas reacts to form part of the product it becomes contained inside the reaction vessel so the total mass of the stuff increases

51
Q

Explanation of when the mass decreases

A

Due to one of the products being a gas and the reactants being solid liquids or aqueous

52
Q

When a mass decreases what happend

A

Before the reaction all the reactants are contained in the reaction vessel.

After if the vessel isnt enclosed then the gas can escape from the reaction vessel as irs formed.Its no longer contained in the reaction vessel so you cant account for its mass.The total mass of the stuff inside decreases

53
Q

How to calculate relative atomic masses

A

(Isotope 1 times abundance) +(isotope 2 times abundance) divided by 100

54
Q

What is the relative formula mass equal to

A

It is numerically equal to the mass of one mole of a substance in grams.

55
Q

How to calculate mass of a given number of moles

A

Mass=moles x relative formula mass

56
Q

What is a standard solution

A

A standard solution is one of known concentration

57
Q

How to increase the concentration of a aqueous solution

A

adding more solute and dissolving it in the same volume of its solution

evaporating off some of the water from the solution so you have the same mass of solute in a smaller volume of solution.

58
Q

Name two acid/base indicators that can be used in the titration between dilute hydrochloric acid and sodium hydroxide solution.

A

Methyl orange,phenoplthaien

59
Q

What colour does phenolphthalein turn in acid/after tiration and base

A

Colourles in acid
Pink in base

60
Q

What colour is methyl orange in acid/titration and base

A

Orange in base
Pink in acid

61
Q

What are the soluble salts

A

Sodium
Lithium
Ammonium
Potassium
Nitrate

62
Q

What do acid and metal carbonate produce

A

Salt +hydrogen

63
Q

Acid + alkali/base

A

Salt + water

64
Q

Acid + metal carbonate/metal hydroxide

A

Salt water + carbon dioxide

65
Q

What is the molar ratio

A

The molar ratio is the ratio between the moles of different reactants and products in a balanced equation.

66
Q

Example of molar ratio

A

N2+3H2 = 2NH3
Ratio of n2:H2:NH3 is 1:3:2

67
Q

What is the relationship between dm^3 and litres

A

1dm^3=1 litre

68
Q

How to calculate dm^3

A

Vol in cm^3/1000

69
Q

How to calculate concentration g/dm^3

A

Concentration mol/dm^3 x Mr

70
Q

How to calculate volume

A

Mass/concentration

71
Q

Define nuetralisation

A

Neutralisation is when an acid reacts with a base, to form a neutral solution. A base that can dissolve in water is called an alkali.

72
Q

How to calculate the number of moles in a gas in dm^3

73
Q

How to calculate the number of moles of a gas in cm^3

A

Volume/24,000

74
Q

What is empirical formula

A

Ratio of atoms

75
Q

How to calculate empircal formula

A

Moles = Mass ÷ Atomic Mass (Ar)
🔹 Simplest Ratio = Divide by the smallest value
🔹 Write the empirical formula using the ratio

76
Q

What is combustioN

A

Burning in air

77
Q

Example of emperical formula question

A

Given percentages:

Carbon (C): 72%
Hydrogen (H): 12%
Oxygen (O): 16%
Step 1: Divide by Atomic Mass (Ar)
Carbon: 72 ÷ 12 = 6
Hydrogen: 12 ÷ 1 = 12
Oxygen: 16 ÷ 16 = 1
Step 2: Divide by the Smallest Number
Carbon: 6 ÷ 1 = 6
Hydrogen: 12 ÷ 1 = 12
Oxygen: 1 ÷ 1 = 1
Step 3: Write the Empirical Formula
C₆H₁₂O

78
Q

Unit for volume

A

Cm^3 or dm^3

Physics And Chemistry 2024 Year 10 (6 decks)

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