Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Rates and Equillibrium > Flashcards

Rates and Equillibrium Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

explain how increasing the SA increases the rate of reaction

A
  • increases the number of particles available for reaction
  • this increases the frequency of collisions
  • meaning more collisions in a given period of time have the required activation energy
  • this increases the rate of reaction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

what are the 3 ways to measure a rate of reaction

A
  1. measure the rate at which a reactant is used up over time
  2. measure the rate at which a product is formed up over time
  3. measure the decreasing light passing through a solution
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what is the equation to measure the rate at which a reactant is used up over time

A

rate of reaction = quantity of reaction used / time

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what is the equation to measure the rate at which a product is formed over time

A

rate of reaction = quantity of product formed / time

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what does collisions mean

A

chance of reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

what does activation energy mean

A

the minimum amount of energy required for a reaction to take place

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

why does raising the temperature increase the rate of reaction

A

collisions theory tells us:

  • particles collide more often
  • particles collide with more energy
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

why does particles colliding more often and with more energy increase the rate of reaction

A

more often: more chances for them to react

more energy: particles moving around more quick]kly have more energy - any collisions they have will be more energetic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

what is a catalyst

A

substances that speed up chemical reactions without being used up in the reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what does a catalyst do and how

A

increases the rate of reaction

by providing an alternative pathway

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

do catalysts produce more product

A

no, always the same amount of product just more quickly

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

how much catalyst is needed to increase the rate of reaction

A

only a very small amount

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

describe the practical decomposition of hydrogen peroxide experiment

A
  1. measure 10cm cubed of hydrogen peroxide solution into conical flask
  2. add the potential catalyst (measure with a spatula) to the hydrogen peroxide solution
  3. reassemble apparatus quickly (and start stopwatch) to avoid losing any gas
  4. note time taken for 20cm cubed of gas to be collected
  5. repeat steps with each potential catalyst
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

independent variable of the practical decomposition of hydrogen peroxide experiment

A

catalyst

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

dependent variable of the practical decomposition of hydrogen peroxide experiment

A

the reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

control variable of the practical decomposition of hydrogen peroxide experiment

A

the 10 cm cubed of hydrogen peroxide solution

17
Q

what is an irreversible reaction

A

A + B -> C + D

has one arrow pointing to the products

18
Q

what is a reversible reaction

A

A + B C + D

products C + D can react with each other to reform reactants A + B

19
Q

is a reversible reaction endothermic or exothermic

A

in any reversible reaction, one reaction will be exothermic and the other will be endothermic

20
Q

what is a salt

A

when an acid is neutralised with a base

21
Q

what is water of crystallisation

A

water molecules in the latice structure

22
Q

write a word equation to show the equilibrium between hydrated and anhydrous copper sulfate crystals
And how to reverse it

A

hydrous copper sulfate (heat, endothermic, putting energy in) –> anhydrous copper sulfate + water
REVERSE REACTION:
add water back to anhydrous copper sulfate
energy released and reaction gets hot, exothermic

23
Q

what colour is hydrous copper sulfate

A

blue

24
Q

what colour is anhydrous copper sulfate

A

white

25
Q

what could anhydrous copper sulfate crystals be used to test for

A

water

26
Q

how can we change the direction of reversible reactions

A

by changing the conditions

27
Q

what is meant by equilibrium

A

when the forward and reverse reactions take place at exactly the same rate

Chemistry (8 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions