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

C4-Quantitive Chemistry Flashcards

(76 cards)

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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
What is the mass of 1 mole equal to
The mass of 1 mole of a substance is equal to its relative formula mass or atomic mass in grams
26
What does a balanced equation show
Shows reacting moles of each substance(as the simplest whole number ratio)
27
How to calculate the maxiumum mass of a substance
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
28
We can only work out the limting reactant if we know
-Number of moles that react in a experiment -Balanced formula equation
29
How to measure concentration
Measured in g/dm^3 or mol/dm^3
30
What does 1dm3 equals
1000 cm3
31
How to calculate concentration
Mass/volume
32
How to calculate mass
Concentration x volume
33
Calculation to calculate moles
Concentration x volume
34
In a chemical reaction why do we not always obtain the mass of the product calculated
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
What is the yield
The amount of product obtained in a chemical reaction
36
How to calculate percentage yield
Mass of product actually made/max theoretical mass of product x100
37
Example question-Zinc reacts with copper sulfate to produce 30g of copper.The theoretical yield of copper is 35g.Calculate the percentage yield
Percentage yield=30/35 x100 85.7%
38
Why is high atom economy important
Contributes to sustainable development Saves costs
39
How to calculate atom economy
Relative formula mass of desired product/Sum of the relative formula mass of all reactants in the equation X100
40
How to calculate volumes of gasses
Mass of gas/relative formula mass x 24
41
Value for avogadros constant
6.02 x 10^23
42
If the amount of solute in a solution is increased what happens to its concentration
Increases
43
If the volume of water in a solution is increased what happens to its concentration
Decreases
44
How should solution be added from the burette close to the end point
Drop by drop,swirling in between
45
Why is a white tile used in titratiom
See colour change better
46
What is a titre
Volume of solution added from thr burette
47
What volume does one mole of any gas occupy at room temperature and pressure?
24dm^3 or 24000 cm3
48
How do we know usually if there is a gas
If the mass seems to change
49
Explanation of when the mass increases
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
when a mass increases what happens
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
Explanation of when the mass decreases
Due to one of the products being a gas and the reactants being solid liquids or aqueous
52
When a mass decreases what happend
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
How to calculate relative atomic masses
(Isotope 1 times abundance) +(isotope 2 times abundance) divided by 100
54
What is the relative formula mass equal to
It is numerically equal to the mass of one mole of a substance in grams.
55
How to calculate mass of a given number of moles
Mass=moles x relative formula mass
56
What is a standard solution
A standard solution is one of known concentration
57
How to increase the concentration of a aqueous solution
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
Name two acid/base indicators that can be used in the titration between dilute hydrochloric acid and sodium hydroxide solution.
Methyl orange,phenoplthaien
59
What colour does phenolphthalein turn in acid/after tiration and base
Colourles in acid Pink in base
60
What colour is methyl orange in acid/titration and base
Orange in base Pink in acid
61
What are the soluble salts
Sodium Lithium Ammonium Potassium Nitrate
62
What is the molar ratio
The molar ratio is the ratio between the moles of different reactants and products in a balanced equation.
63
Example of molar ratio
N2+3H2 = 2NH3 Ratio of n2:H2:NH3 is 1:3:2
64
What is the relationship between dm^3 and litres
1dm^3=1 litre
65
How to calculate dm^3
Vol in cm^3/1000
66
How to calculate concentration g/dm^3
Concentration mol/dm^3 x Mr
67
How to calculate volume
Mass/concentration
68
Define nuetralisation
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.
69
How to calculate the number of moles in a gas in dm^3
Volume/24
70
How to calculate the number of moles of a gas in cm^3
Volume/24,000
71
What is empirical formula
Ratio of atoms
72
How to calculate empircal formula
Moles = Mass ÷ Atomic Mass (Ar) 🔹 Simplest Ratio = Divide by the smallest value 🔹 Write the empirical formula using the ratio
73
What is combustioN
Burning in air
74
Example of emperical formula question
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
75
Unit for volume
Cm^3 or dm^3
76
What is the element in excess
The element which has not been fully used up.still has left

Physics And Chemistry 2024 Year 10 (9 decks)

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