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Chemistry > Quantitative Chemistry > Flashcards

Quantitative Chemistry Flashcards

1
Q

What do you compare an element to, to get its relative atomic mass

A

Carbon-12

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2
Q

When can changes of mass occur in a reaction

A

In a non-closed system

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3
Q

Example of a non-closed system losing mass

A

When a gas is produces

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4
Q

If everything is included in the reaction calculation

A

The mass stays the same

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5
Q

What is uncertainity in a experiment

A

Measure of variability

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6
Q

2 ways of measuring uncertainty

A

Use the range of results or the resolution of the equipment you used

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7
Q

Types of error

A

Random error, systematic error

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8
Q

What are random errors

A

Errors that cannot be predicted and are random

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9
Q

Examples of random errors

A

Human error for example technique while taking measurements
Instruments are faulty

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10
Q

What are systematic errors

A

Errors that are produced consistently

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11
Q

Example of systematic errors

A

Problems with experimental method
Not adjusting a scale properly

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12
Q

Uncertainty equation

A

Uncertainty = range of results/2

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13
Q

To measure concentration you must

A

Work in Dm3 for volume

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14
Q

Dm to Cm
Dm3 to Cm3

A

x10
x1000

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15
Q

Concentration equation

A

Concentration = mass /volume

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16
Q

How many particles is one mole

A

6.02 x 10^23 Avagadros constant

17
Q

The mass of one mole of a substance is

A

Equal to its relative formula mass

18
Q

Symbol for Avogadros constant

A

N with a little A at the bottom

19
Q

Number of particles in a substance equation

A

N = n x Avagadros constant

n= number of moles

20
Q

Mass moles equation

A

moles = mass/Mr

21
Q

Calculate the mass of water when burning 300g of Methane

A
  1. CH4 + O2 –> 2H2O + CO2
    2.
    3.
    4.
    5.
22
Q

What is a limiting reactant

A

The reactant that is used up first meaning the reaction can no longer take place as the other reactant(s) have nothing to react with

23
Q

How to workout the maximum mass of something produced in a reaction

A

Workout the moles of the known
Compare that to what 1 mole of the known makes of the unknown
e.g if 1 mole of iron makes 1 mole of iron oxide then 1.5 moles of iron makes 1.5 moles of iron oxide
workout mass of unknown

24
Q

Concentration moles equation

A

Concentration = moles/volume

25
Q

How to convert from mol/dm3 to g/dm3

A

Times by Mr

26
Q

Percentage yield equation

A

Actual mass of product/ theoretical mass of product
times 100

27
Q

What does the law of conservation state about a reaction

A

No atoms are lost

28
Q

Why might you not achieve the maximum theoretical mass of a product

A

Some reactants lost in the filtration process
Reaction may not go to completion
Some reactants may not react

29
Q

Atom economy definition

A

Amount of reactants that end up as useful product

30
Q

Atom economy equation

A

relative formula mass of product/relative formual mass of all reactants
REMEMBER TO USE BIG NUMBER

31
Q

5 Reasons why you would make a product a certain way

A

Higher percentage yeild
Higher atom economy
Rate of reaction
Renewable resources as products
Usefulness of byproducts

32
Q

Avagadro’s LAW

A

When temperature and pressure are the same 2 different gasses with the same volume have the same amount of molecules

33
Q

What is molar ratio

A

The ratio between the amounts in moles of any two compounds involved in a balanced chemical reaction

34
Q

What is the molar volume

A

Volume occupied by one mole of a gas

35
Q

Molar volume equation

A

Volume= amount of moles x molar volume

36
Q

What is the molar volume of any gas at room temperature

A

24dm3

Chemistry (10 decks)

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