C5

Front 1

Word equation for thermal decomposition?

Back 1

metal carbonate--> metal oxide + carbon dioxide

Front 2

git good

Back 2

shut up cranky

Front 3

Relative atomic mass is?

Back 3

Average mass of an element compared to the mass of one twelfth of an atom of carbon 12.

Front 4

Mole equation?

Back 4

mass of chemical / molar mass --> #of moles

Front 5

How do you work out the empirical formula?

Back 5

1.Write down mass of each element

2.Get relative mass of each

3.Work out how many mols in each

4.Choose smallest amount

5.Divide mols of all other elements by the amount in the smallest one

6.Cry

Front 6

How do you calculate percentage mass?

Back 6

(mass of element in compound / relative formula mass) x 100

Front 7

How do you calculate empirical formulae from percentage composition by mass?

Back 7

1.Mass of each element in 100g of acid

2.Relative atomic mass of each element

3.Convert to mols of each element

4.Choose element least present

5.Divide all by smallest

Front 8

What does mols mean?

Back 8

The mass of substance containing the same number of fundamental units as there are atoms in exactly 12.000 g of 12C

Front 9

If you have 1cm3 of a solution, how much water must be added to make it ten times more dilute?

Back 9

(10-1=9)

9cm3

Front 10

How do you convert cm3 to dm3?

Back 10

Divide by 1000

Front 11

What's the concentration equation?

Back 11

concentration= amount in moles / volume dm3

Front 12

What does GDA stand for?

Back 12

Guideline Daily Amount

Front 13

How do you calculate the amount of sodium to salt?

Back 13

Salt it 2.5 times mass of sodium- so multiply by 2.5

Front 14

What happens in a titration?

Back 14

An acid and an alkali neutralise.

Front 15

What colour will litmus paper go in acid and alkali?

Back 15

Acid: red

Alkali: blue

Front 16

What colour will phenolpthalein go in acid and alkali?

Back 16

acid: colourless

alkali: pink

Front 17

What colour will screened methyl orange go in acid and alkali?

Back 17

acid: pink

alkali: green

Front 18

To show an end point, which indicator should be used and why?

Back 18

A single one like phenolthalein or methyl orange or litmus because they give a sharp colour change- not universal indicator which gives a range of colours and thus is hard to measure.

Front 19

How to work out the concentration of a solution in titration?

Back 19

1.Work out moles of acid used

2.Work out how many moles of alkali used

3.Link the acid with the alkali (whatever the hell that means miss gibbo)

Front 20

What three ways can you measure the amount of gas produced in a reaction?

Back 20

1.Upturned burette or measuring cylinder filled with water

2.Burette which works the same

3.Gas syringe

Front 21

At room temp and pressure, 1 mole of gas takes up ____dm3

Back 21

24

Front 22

What is the limiting reactant?

Back 22

The one that gets used up first

Front 23

What is equilibrium?

Back 23

When a balance of amounts of reactants and products is reached

Front 24

Equilibrium only works in a closed system, why?

Back 24

The chemicals can't get out.

Front 25

How does equilibrium work?

Back 25

Initially the forward reaction is fast but then slows as reactants are used up. At the same time, the backward reaction rate increases as more is available to react. Eventually, both are going as fast as each other.

Front 26

What factors can alter equilibrium position?

Back 26

Temperature

Pressure

Concentration

Front 27

What is the contact process?

Back 27

A reaction between sulfur dioxide and oxygen to make sulfur trioxide. It's carried out at a compromise temperature of 450 degrees at atmospheric pressure using vanadium pentoxide as the catalyst. Forward is EXO and back is ENDO.

Front 28

What makes strong acids strong?

Back 28

ALL hydrogen atoms ionise, whereas in weak only a few do

Front 29

Complete:

strong acid <--> ____ + ______

Back 29

hydrogen ions + other ions

Front 30

How do you define a strong acid?

Back 30

Complete ionisation in water (like hydrochloric) with many H+ ions

Front 31

Why do weak acids react slower?

Back 31

In reactions, it's the H+ ions that actually react. Weak acids have less of those and thus collisions are less frequent.

Front 32

How are kettles de scaled?

Back 32

Using acid to react with the calcium carbonate. Weaker acids are used because stronger acids work so quick that it runs the risk of reacting with the element.

Front 33

Give an example of a weak acid

Back 33

Ethanoic

Front 34

What is pH used to show?

Back 34

Concentration of H+ ions

Front 35

Complete:

CH3COOH <--> ____ + ____

Back 35

H+

CH3COO

Front 36

Strong acids ionise completely in water, complete the equation:

HCl --> ___ + ___

Back 36

H+

Cl-

Front 37

Despite the fact weak acids do not conduct as well as strong ones, the same amount of gas will eventually be made if the same amount of reactants are used- why?

Back 37

Weak acids will use some H+ ions to react and be used up first so more molecules of acid will ionise producing more H+ ions. Either way, the same amount is produced at the end as if a strong acid was used.

Front 38

What does concentration tell us?

Back 38

How many moles of acid there are in 1dm3 of a solution.

Front 39

Word equation for when Barium Chloride is added to sodium sulfate?

Back 39

barium chloride + sodium sulfate --> barium sulfate + sodium chloride

Front 40

What are the 4 steps to creating clean, insoluble salt?

Back 40

1. Mix barium chloride and sodium sulfate to make barium sulfate and sodium chloride

2. Filter the precipitate (barium sulfate)

3. Wash the precipitate with distilled water to remove traces of sodium chloride

4. Dry by leaving in warm place so water evaporates

Front 41

What are spectator ions?

Back 41

Don't directly take part in the reaction. E.g. sodium iodide and lead nitrate react but only lead and iodide ions do anything, so the nitrate and sodium are spectators.

Front 42

Hi chloe

Back 42