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Chemistry 2 Erin's > C2b > Flashcards

C2b Flashcards

1
Q

What 4 things does rate of reaction depend on?

A

Temperature, concentration/pressure, catalyst, surface area (solids)

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2
Q

What are the 2 ways rate of reaction can be measured?

A

How quickly reactants are used up

How quickly the products are formed

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3
Q

What is the formula for rate of reaction?

A

Amount of reactant used/product formed ÷ time

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4
Q

What 3 things can rate of reaction be measured by?

A
  1. Precipitation- cloudy solution- cross under flask
  2. Change in mass- gas given off- mass balance
  3. Volume of gas given off- gas syringe
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5
Q

What are the 3 rate of reaction experiments and what do they measure?

A
  1. Hydrochloric acid and marble chips- gas given off
  2. Reaction of magnesium metal with hydrochloric acid- change in mass
  3. Sodium thiosulfate and hydrochloric acid- precipitation
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6
Q

What is the collision theory?

A

The more collisions in particles = the faster the rate of reaction

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7
Q

What 3 things increase collisions and why?

A
  1. Higher temperature- more kinetic energy so particles move quicker
  2. Higher concentration/pressure- more particles of reactant knocking water particles/pressure means particles are squashed together
  3. Larger surface area- particles around it in solution will have more area to work on
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8
Q

Reactions can only happen if…

A

particles collide with enough energy

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9
Q

What’s a catalyst?

A

A substance that speeds up the rate of reaction without changing it or being used up in the reaction

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10
Q

How does a solid catalyst work?

A

It gives the reacting particles something to stick to, increasing the number of successful collisions

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11
Q

How do catalysts reduce costs in industrial reactions?

A

They increase the rate of reaction- this saves money because plants and machines don’t need to operate for as long. The reaction can operate at a lower temperature which reduces energy needed- saves money/sustainable

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12
Q

What are the disadvantages of using catalysts in the industry?

A
  • Expensive to buy
  • Need to be removed from product and cleaned
  • Different reactions need different catalysts
  • Can sometimes be poisoned by impurities so they stop working
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13
Q

What’s an exothermic reaction?

A

One which transfers energy to the surroundings, usually in the form of heat and is shown by a rise in temperature

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14
Q

What’s an example of an exothermic reaction?

A

Burning fuels (combustion)

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15
Q

What everyday items use exothermic reactions?

A

Handwarmers/self heating cans

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16
Q

What’s an endothermic reaction?

A

One which takes energy from the surroundings (in the form of heat) and is shown by a fall in temperature

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17
Q

What’s an example of an endothermic reaction?

A

Thermal decompositions

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18
Q

What everyday items use endothermic reactions?

A

Sports injury ice packs

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19
Q

In a reversible reaction, if a reaction is endothermic in one direction, it will be…

A

exothermic in the other direction

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20
Q

What is the pH scale and what does it go up to?

A

A scale used to measure how acidic or alkaline a solution is, it goes from 0-14

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21
Q

Which side of the pH scale is acidic?

A

0-6

22
Q

Which number on the pH scale is neutral?

A

7

23
Q

WHich side of the pH scale is alkaline?

A

8-14

24
Q

What is indicator?

A

A dye that changes colour depending on whether it’s above or below a certain pH

25
Q

What’s a base?

A

A substance with a pH greater than 7- and alkali is a base that dissolves in water

26
Q

What type of ions do alkalis form?

A

OH-

27
Q

What type of ions do acids form?

A

H+

28
Q

What’s the word equation for neutralisiation?

A

acid + base = salt + water

29
Q

What’s the word equation for acids reacting with metals?

A

Acid + metal = salt + hydrogen

30
Q

The more reactive the metal, the faster the reaction, true or false?

A

True

31
Q

When metals react with acids, what’s the speed of reaction indicated by?

A

The rate at which bubbles are given off

32
Q

How is hydrogen confirmed in a reaction?

A

The burning splint test- squeaky pop

33
Q

Which salts will hydrochloric acid produce?

A

Chloride salts

34
Q

Which salts will sulfuric acid produce?

A

Sulfate salts

35
Q

What are metal oxides and metal hydroxides?

A

Bases

36
Q

All metal oxides and hydroxides react with acids to form…

A

salt and water

37
Q

What does hydrochloric acid + copper oxide make?

A

Copper chloride and water

38
Q

What does sulfuric acid + zinc sulfate make?

A

Zinc sulfate and water

39
Q

What does nitric acid + magnesium oxide make?

A

Maagnesium nitrate and water

40
Q

What neutralises ammonia to make fertiliser?

A

HNO3

41
Q

Briefly describe the steps to make soluble salts using a metal or insoluble base:

A
  • Pick the right acid plus a metal of insoluble base
  • Add to the acid and wait for the solid to dissolve as it reacts
  • Filter out the excess metal to get the salt solution
  • Evaporate some of the water and leave the rest to exaporate slowly- crystalisation
42
Q

Briefly describe the steps to make soluble salts using an alkali:

A
  • Add exactly the right amount of alkali to neutralise the acid (using indicator first, then without)
  • Then evaporate off the water to crystalise the salt
43
Q

Briefly describe the steps of making insoluble salts using a precipitation reaction:

A
  • You need 2 solutions with the ions you need
  • Once the salt has precipitated out, filter it from the solution
  • Wash&dry it on filter paper
44
Q

What does electrolysis mean?

A

Splitting up with electrons

45
Q

Briefly describe the process of electrolysis:

A
  • An electric current through an ionic substance that’s molten or in solution, it breaks down into the element it’s made from
  • Requires a liquid to conduct the electricity- electrolyte
  • Electrolytes contain free ions that conduct electricity
  • Electrons are taken away from ions at the positive electrode and given to other ions at the negative electrode
46
Q

Electrolysis always involves oxidation and reduction- what are these?

A

Oxidation: Loss of electrons (gain of oxygen) OIL
Reduction: The gain of electrons RIG

47
Q

What do half-equations show?

A

The reactions at the electrodes

48
Q

How is aluminium extracted from its ore?

A

Using electrolysis

49
Q

What’s the process of removing aluminium from its ore?

A
  • Aluminium oxide is dissolved in molten cryolite (metling point brought down to 900 degrees)
  • Aluminium forms at the negative electrode and oxygen forms at the positive one
50
Q

What is electroplating?

A

When electrolysis is used to coat the surface of one metal with another metal

51
Q

In electroplating what is the negative electrode and what is the positive electrode?

A

Negative: Object you want to plate
Positive: The pure metal you want it to be plated with

52
Q

What are the uses for electroplating?

A

Decoration and conduction

Chemistry 2 Erin's (2 decks)

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