Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Reactivity 2 > Flashcards

Reactivity 2 Flashcards

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

Stoichiometry

A

The fixed relationship between the number of reactant particles and the number of product particles

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

Formula to find out the number of moles of a gas

A

Volume (V)/molar volume (Vm)

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

Molar volume definition

A

The volume occupied by one mole of any gas

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

Limiting reactant/reagent

A

The reactant that is in excess, i.e runs out first

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

Theoretical yield definition

A

Maximum amount of product that could be formed according to the balanced equation

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

Experimental yield definition

A

Actual amount of product obtained when the experiment is performed

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

Percentage yield formula

A

Experimental yield/theoretical yield x 100

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Factors that could cause the experimental yield to be lower than the theoretical yield

A
  • Side reactions occurring
  • Decomposition of reactants and/or products
  • Loss of product during purification
  • Reversible chemical reactions preventing process completion
  • Incomplete reaction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Factors that could cause the experimental yield to be higher than the theoretical yield

A
  • Impurities in a product
  • When a product hasn’t been fully dried
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

How to find atom economy (4 steps)

A
  • Write balanced equation
  • Calculate relative molar mass, and then total mass
  • Calculate relative molar mass of each desired product, and then total mass of each desired product formed
  • Find atom economy using atom economy formula
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Atom economy formula

A

Total mass of desired products/total mass of products x 100

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

If a use for the products are found in atom economy, what is the atom economy?

A

100%

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

Units for rate of reaction

A

mol dm^-3 s^-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Collision theory

A

Particles must collide at the right angle with sufficient energy

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

How does concentration increase rate of reaction?

A

More collisions will occur due to the greater number of particles in the acid

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

How does surface area increase rate of reaction?

A

Only the particles on the surface can collide, if it is in powdered form there is a much greater surface area; more collisions per second

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

How does temperature increase rate of reaction?

A

The particles are moving faster; there will be more collisions per second

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

How does a catalyst increase rate of reaction?

A

Bringing the reactive parts of the reactants into close contact with each other, lowering the activation energy; less energy will be needed to collide sufficiently

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Formula for rate of reaction

A

increase in product concentration/time taken or (-)decrease in product concentration/time taken
rise over run

20
Q

Is rate positive or negative

A

Positive

21
Q

Systematic errors

A

Inaccurate measurements
When all measurements are higher or lower than expected values
Cannot be fixed

22
Q

Random errors

A

Imprecise data
Occur due to limitations in measurement equipment (uncertainties), misinterpreted measurements or not enough trials.
Can be fixed by repeating measurements and averaging results

23
Q

Equilibrium law

A

When the rate of the forward reaction is equal to that of the reverse reaction.

24
Q

Formula for K

A

[products]/[reactants]

25
Q

If it were a reverse reaction, how would K be written?

A

K’

26
Q

What is K dependent on?

A

Temperature

27
Q

If K is big, what happened with the reaction and concentration?

A

The reaction is pretty much completed and the concentration of reactants is very small.

28
Q

If K is small, what happened with the reaction and concentration?

A

The reaction has barely taken place and the concentration of the products is very small.

29
Q

If K is around one, what happened with the equilibrium?

A

There will be a good amount of reactants and products in the equilibrium.

30
Q

Units of K

A

K has no units

31
Q

How to find K from K’

A

Reciprocal

32
Q

If you add a catalyst to a reaction, what happens to the equilibrium?

A

Nothing

33
Q

If the concentration of the products is increased, what happens to the equilibrium?

A

Shifts to the left

34
Q

If the concentration of the reactants decreases, what happens to the equilibrium?

A

Shifts to the left

35
Q

If the concentration of the products decreases, what happens to the equilibrium?

A

Shifts to the right

36
Q

If the concentration of the reactants increases, what happens to the equilibrium?

A

Shifts to the right

37
Q

If the number of mols (gas) on both sides are equal, what happens to the equilibrium?

A

Nothing

38
Q

If there are more mols on the reactant side, what happens to the equilibrium?

A

Shifts to the right

39
Q

If there are more mols on the product side, what happens to the equilibrium?

A

Shifts to the left

40
Q

In exothermic reactions, lowering the temperature will do what to the equilibrium?

A

Shift to the right

41
Q

In endothermic reactions, increasing the temperature will do what to the equilibrium?

A

Shift to the right

42
Q

In exothermic reactions, the higher the temperature gets does what to the value of K?

A

It decreases the higher the temperature

43
Q

In endothermic reactions, the higher the temperature gets does what to the value of K?

A

It increases the higher the temperature

44
Q

What thing changes the K value?

A

Temperature

45
Q

Heterogenous equilibria

A

When one or more of the reactants are in different phases.

46
Q

How to calculate theoretical yield

A

Use mole ratios- perhaps with figures given in the question

47
Q

If asked a question to calculate something measured at STP, how do you find it?

A

Multiply the ‘n’ value by 22.7 (STP value)

Chemistry (5 decks)

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