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Chemistry Challenge > Physical > Flashcards

Physical Flashcards

1
Q

Methyl orange

A

0-3 red
3-6 orange
6-14 yellow

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2
Q

Phenolphthalein

A

0-10 colourless

10-14 red

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3
Q

Acid def

A

A substance that dissolved in water to produce hydrogen ions (H+)

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4
Q

Litmus paper

A

0-4 red
5-8 purple
8-14 blue

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5
Q

Acid + metal

A

Salt + hydrogen

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6
Q

Acid+ metal carbonate

A

Salt + CO2 + water

When testing wait till no more bubbles form to show complete neutralisation

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7
Q

Acid + metal oxide

A

Salt + water

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8
Q

Acid + metal hydroxide

A

Salt + water

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9
Q

Solubility

Nitrates

A

All

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10
Q

Solubility

Chlorides

A

All but silver and lead

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11
Q

Solubility

Sulfates

A

All but barium, calcium and lead 2

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12
Q

Solubility

Sodium, potassium and ammonium salts

A

All

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13
Q

Solubility

Sodium, potassium and ammonium carbonates

A

All

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14
Q

Insoluble base + acid test

A
  • heat acid
  • add base a little at a time
  • till excess
  • filter (to remove access)
  • hydrous? Heat till at least 2/3 of the water had left
  • leave to crystallise in a warm place
    Remove crystals and then dry
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15
Q

Soluble base + acid test

A
  • aqueous solution of alkali into conical flask and add indicator
  • add dilute acid until change in colour
  • add powdered charcoal and shake to remove colour
  • filter to remove charcoal
  • obtain crystals from filtrate
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16
Q

Preparation of insoluble salts

A

Precipitation reactions!

(Insoluble solid made by chemical reaction in an aqueous solution)

  • mix 2 aqueous solution
  • one of then contains +ve ion other
  • ve ion
  • filter
  • with the filtrate wash with distiller water to remove traces of the solution formed
  • leave to dry
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17
Q

Make ammonia

A

Whenever ammonium salt reacts with an acid

Indicator needed to decide whether or not reaction is complete
- acid alkali titration

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18
Q

Acid- alkali titration

A

To find given volume of acid required to react exactly with the given volume if alkali

  • use pipette add 25cm3 of alkali solution into conical
  • add few drops of indicator
  • put acid into a burette and note initial reading
  • add acid till change in colour
  • not how much was added
  • repeat without indicator but the exact volume
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19
Q

Exothermic

A

Energy given out

Rise in temp

——–\______

^H = negative

20
Q

Endothermic

A

Energy taken in

Fall in temp

_____/———

^H = positive

21
Q

Measure heat change

A

Place acid into polystyrene cup
Record temp of acid
Tip excess powder into acid
Measure and record highest Reno reached by mixture

  • rise in temp
  • heat given out
22
Q

Heat given out equation

A

Mass of solution x specific heat capacity x temp rise

E = mc^T

23
Q

Bond energies

A

Energy required to break a bond

24
Q

Bond energy measured in…

A

Kj per mol

KJ/mol

25
Q

Breaking bonds

A

Takes in energy

Endothermic process

26
Q

Making bonds

A

Gives out energy

Exothermic process

27
Q

How to calculate /\ H

A

Bonds broken- bonds made

28
Q

Rate of reaction def

A

Rate = change of conc of reactant / time

29
Q

Factors there affect rate of reaction (3)

A

Conc of reactant
Temp at which reaction takes place
State of division

30
Q

Conc rates

A

Increasing conc increases no of particles in a given volume hence increasing the frequency of collisions
This means there will be more successful collisions per second

Same as increasing pressure

31
Q

Temp rates

A

Increased average kinetic energy of the reactant particles therefore more of the collisions will have the required activation energy needed to be successful

32
Q

State of division rates

A

Smaller the pieces the larger the surface area
More particles exposed to other reactant
More successful collisions per sec
Most effective in powder form

33
Q

Effect of catalyst

A

Provides an alternate pathway for the reaction
Has a lower activation energy than the original pathway
Means that more of the collisions will have the necessary activation energy

34
Q

Catalyst def

A

A substance that increases the rate of a chemical reaction but is chemically unchanged at the end of the reaction

35
Q

Reaction that goes both ways

A

Reversible

36
Q

Example of a reversible reaction

A 
Copper 2 sulfate crystals 
Hydrous and anhydrous 
Heating and adding water
Water of crystallisation 
From white to blue with water
37
Q

2nd example of reversible reaction

A

Heating ammonium chloride

White solid crystals -> colourless gases

NH4Cl -> HCl + NH3

The gases rise and cool to form back

38
Q

Dynamic equilibrium

A

If reaction reversible is carried out in a closed container then it is possible for the reaction to reach a position of dynamic equilibrium

When rate if forward is equal to rate of backward
Amounts of reactants and products remain CONSTANT
Properties relying on amounts of reactants/ products remain constant (colour or pressure)

39
Q

Shift the position of equilibrium

A

To the right

To the left

40
Q

Equilibrium increase pressure

A

Shifts in direction that produces the smaller number of molecules of gas

41
Q

Equilibrium increase in temp

A

Moves in endothermic direction

42
Q

Equilibrium decrease in temp

A

Moves in Exothermic direction

43
Q

Equilibrium model answers

Temperature

A

The equilibrium shifts to the (left/right) because the (forward/backward) reaction is Exothermic

44
Q

Equilibrium model answer

Pressure

A

The equilibrium shifts to the (left/right) because there are fewer molecules of gas in the (left/right)

45
Q

Equilibrium model answer

Adding or removing substances

A

The equilibrium shifts to the (left/right) because the (forward/backward) reaction uses/produces the _____

46
Q

Equilibrium

Increasing temp will favour the….

A

Endothermic reaction because this reaction needs heat to occur
Decreasing will favour Exothermic because less heat means that the endothermic reaction can’t happen as much

Chemistry Challenge (8 decks)

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