Ph 2 Amount of substance Flashcards

1
Q

moles of a solid equation

A

mass / Mr

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

moles of a solution equation

A

concentration x volume

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

ideal gas equation

A

pressure x volume = moles x gas constant x temperature

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

what is mass measured in for solid moles

A

grams

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

unit of concentration

A

mol dm-3

g dm-3

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

how to convert between units of concentration

A

multiply mol dm -3 by the Mr to get g dm-3

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

what is volume measured in for solutions equation

A

dm3

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

what are the units in the ideal gas equation

A
volume= m3
pressure = Pa
temperature = Kelvins
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

1 ton in grams

A

1,000,000 grams

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

1 kg in grams

A

1,000 grams

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

1mg in grams

A

0.001 grams

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

limiting reagent

A

the reactant that limits the amount of moles of product that can be made, the other product is in excess meaning there will be some left over after the reaction.

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

m3 conversion =

A

cm3/1,000,000

dm3/1,000

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

pressure conversion

A
Pa = KPa x 1000
Pa= MPa x 1,000,000
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

temperature conversion

A

k=c + 273

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

what is an ideal gas?

A

a gas with no forces between molecules, all particles size is negligible

17
Q

what can the ratio of the equation be used for

A

moles

volume of a gas

18
Q

final volume

A

volume of products + volume of excess left over

19
Q

what is atom economy?

A

a measure of the amount of starting materials that end up as useful products in theory

20
Q

equation for atom economy

A

(total Mr of desired product / total Mr of reactants ) x 100

21
Q

what is percentage yield?

A

Compares the mass of product you produce to the amount you expected. Practical based.

22
Q

equation to calculate percentage yield

A

( actual yield / theoretical yield ) x 100

23
Q

reasons why the actual yield may be lower than the theoretical yield

A

reversible reaction
reaction did not reach completion
other reactions occurred
product lost during isolation

24
Q

what is relative molecular mass

A

the average mass of one molecule relative to 1/12 the mass of one atom of carbon twelve

25
Q

what is the empirical formula

A

the simplest ratio of atoms of each element in a compound

26
Q

what is the molecular formula

A

the actual ratio of atoms of each element in a compound

27
Q

steps to find the empirical formula

A

1) write out the mass of percentage of that element in the compound
2) Divide by the Ar of the element
3) Divide by the smallest to get a to one ratio
4) Make ratio to whole numbers

28
Q

how to find the molecular formula from the empirical formula

A

1) Find the Mr of the compound
2) divide the Mr of the compound by the Mr of the empirical formula
3) Multiply the empirical formula values by this amount.

29
Q

how to find the mass of an element in a compound of known mass

A

mass of compound x (Ar of element/Mr of compound)