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BMAT > Chemistry 7-Rate of Reaction > Flashcards

Chemistry 7-Rate of Reaction Flashcards

1
Q

Rate of reaction depends on what 4 things

A

Temperature
Catalyst
Concentration (pressure for gasses)
Surface area of solids(smaller bits higher rate)

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2
Q

Rate of reaction =

A

amount used or formed / time

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3
Q

How does the precipitation method of observing rate of reaction work?

A

Observe a mark on a beaker and wait until you cant see it anymore

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4
Q

Change in mass is measured how?

A

Production of a gas leads to a decrease in the mass of a scale

The quicker the readings drop the faster the reaction

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5
Q

Name one more more method of observing rate of reaction

A

Volume of gas given off

Using syringe

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6
Q

If you were to double the quantity of small chips present in a HCl solution, what happens?

A

Quicker reaction

More gas created

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7
Q

Which method would you use for HCl and Marble Chips

A

Volume given off (Syringe)

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8
Q

Which method would you use for magnesium metal and HCl

A

Mass scales + gas given off

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9
Q

why is the mass scale method good?

A

Can help work out the measuring effects of increased concentration as H+ is given off

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10
Q

Sodium Thiosulfate + HCl produce what precipitate

A

Cloudy yellow

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11
Q

sodium thiosulfate and HCl are what colour?

A

clear

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12
Q

What can we do with the sodium thiosulphate and HCl reaction when repeating it?

A

Use of different temperatures via a waterbath

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13
Q

What is the precipiate formed with sodium thiosulphate and HCl

A

Sulphur

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14
Q

Hydrogen peroxide breaks down into what?

A

Water / oxygen

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15
Q

What 3 things can speed up the rate of reaction with hydrogen peroxide breakdown

A

Manganse (IV) oxide catalyst

Potato Peel

Blood

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16
Q

Name the main benefit from an industrial point of view on catalyst

A

Never get used up in the reaction

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17
Q

What can poison the iron catalyst in the Haber process?

A

sulphur impurities

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18
Q

Name an example of an exothermic reaction

A

Burning fuels (Combustion)

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19
Q

Acid + Alkali are what type of reaction?

A

Exothermic

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20
Q

Sodium and water is what type of reaction

A

exothermic

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21
Q

Handwarmers use what to generate heat

A

oxidation of iron in air

with salt solution catalyst to generate heat

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22
Q

Thermal decomposition is what type of reaction

A

Endothermic

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23
Q

Give an example of a endothermic reaction in practical use

A

Sports injury pack

They take in heat which makes the pack very cold

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24
Q

What must be supplied to decompose calcium carbonate?

What sort of reaction is this?

A

Heat

Endothermic reaction

25
Q

Hydrated copper sulphate –> anhydrous copper sulphate and water

what type of reaction?

A

Endothermic

26
Q

Anhydrous Copper sulphate + water –>Hydrate copper sulphate

what type of reaction

A

exothermic

27
Q

Heating blue copper (2) sulphate turns it what colour?

A

White

28
Q

Bond breaking is what type of reaction

A

endothermic

29
Q

bond formation is what type of reaction

A

exothermic

30
Q

In an endothermic reaction, the energy required to break old bonds is what?

A

Greater than the energy released when new bonds are formed

31
Q

In an exothermic reaction, the energy released in bond formation is what?

A

Greater than the energy used in breaking old bonds

32
Q

How can you measure the amount of energy released in a chemical reaction?

A

taking temperature of the reagents at start / and at end

33
Q

What method is used to measure the amount of energy released?

A

Polysteyrene cup + beaker of cotton wool and a lid

34
Q

What type of reactions is using the polysteryne cup good for?

A

Solids with water

neutralisation reactions

35
Q

Working out using Calorimetry equation

A

mass of water x specific heat capacity (4.2) x change in temperature

36
Q

In exothermic reactions, the reactants always have what?

A

more starting energy

hence -H

37
Q

In endothermic reactions, the products always have what?

A

Greater initial energy

hence +H

38
Q

Dynamic equiibrium is what

A

Where both sides of the reaction are happening simultaneously but no overall net change

39
Q

Equilibrium in a reaction only happens in what type of system?

A

Closed system

40
Q

What 3 things can change equilibrium?

A

Temperature

pressure

concentration

41
Q

Adding a catalyst doesnt do what

A

change the equilibrium position

42
Q

Decreasing the temperature of a reaction, will shift the equilibrium why

A

Moves in to exothermic direction to produce more heat

43
Q

Increasing the temperature causes the equilibrium to move where

A

endothermic direction to try and decrease the temperature

44
Q

Changing pressure only affects what

A

gases

45
Q

Increasing the pressure changes the equilibrium how and why

A

It tries to reduce it by moving equilibrium in the direction where there are fewer molecules (the side with less moles)

46
Q

Increasing the concentration of the reactants will do what to the equilibrium?

A

Tries to decrease it by making more product (shifts to the right)

47
Q

Increasing the concentration of a product will do what to equilibrium?

A

Shift to the left by creating more reactant

48
Q

Nitrogen and Hydrogen form what

A

Ammonia

49
Q

Hydrogen can be obtained how?

A

Natural gas / crude oil

50
Q

With the haber process, which is the exothermic reaction?

A

forward reaction

51
Q

What happens in the Haber process when increasing pressure?

A

More ammonia formed

increased %yield

52
Q

Lowering the temperature does what for the reaction?

A

Increases the yield (favours exothermic reaction)

However it takes longer

53
Q

what is the correct temperature for Haber

A

450*

54
Q

Ammonia is formed as what?

What happens to the nitrogen/hydrogen

A

Formed as gas then cooled to form liquid

recycled

55
Q

What catalyst is used in the haber process? what does it NOT change

A

iron catalyst

decreases the temperature required

56
Q

Whats the ideal conditions for the Haber process?

A

High pressure and low temperature

57
Q

Draw the % yield of ammonia to pressure

A

=

58
Q

Draw the % yield of ammonia to temperature

A

=

BMAT (21 decks)

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