Brainscape's Knowledge GenomeTM

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


See full index

Chemistry 3.1 > 1.2 Amounts of substances > Flashcards

1.2 Amounts of substances Flashcards

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

What is the definition of Relative Atomic Mass?

A

average mass of an atom of an element

on a scale where an atom of carbon-12 has a mass of 12

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

Relative Molecular Mass

A

Average mass of a molecule on a scale where an atom of carbon-12 has a mass of 12

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

Diff between Relative Formula mass and Mr

A

For ionic compounds (that do not exist as molecules) the term relative formula mass is used instead.

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

Formula of Complex Ion Manganate (VII)

A

MnO4-

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

Complex Ion Chromate

A

CrO2^-

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

Complex Ion Dichromate

A

Cr2O7^2-

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

Why are ionic compounds in Relative Formula Mass?

A

Because ionic compounds don’t really form molecules (they form large lattices) we cannot talk about molecular units.

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

Chromium (III) sulphate formula

A

Cr2(SO4)3

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

Ammonium nitrate

A

NH4NO3

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

Copper (II) sulphide

A

CuS3

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

Diff btw sulphide and phate

A

Ide- just ion with oxygen

ate- with oxygen SO4

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

Deduce the formula of the compound that contains 2+ ions and 3− ions that both have the same electron configuration as argon.

A

Originally had two more electrons than Ar, 2+ ion = Ca2+
Originally had three less than Ar, 3- ion = P3-
Ca3P2

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

Significant figures for calculations involving

multiplication / division

A

Your final answer should be given to the same number of significant figures as the least number of significant figures in the data used.

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

Significant figures for calculations involving

addition/subtraction ONLY

A

Here the number of significant figures is irrelevant – it is about the place value of the data. We round our answer to the data with the fewest number of decimal places.
answer cannot have more decimal places than
either of the original numbers

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

SI Units

A

Amperes, Kelvin (temp), Kilograms (mass), Candela (light), Moles, Seconds (time), Metres

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

Calculate Mr of aspirin (search up skeletal structure)

A

C9H804

17
Q

What are the two formulas for moles that link?

A

moles = mass (g)/ Mr

moles in solution =
concentration c (mol dm-3) x volume V (cm^3)
18
Q

One mole of any substance contains the same amount of particles…

A

6.022 x 10^23

19
Q

What is the limiting factor?

A

In the real world of chemistry, it is rare that we react the exact right amount of chemicals together. Usually, we have more than we need of one of the reactants and so it doesn’t all react – it is in excess.

Sometimes in calculations, we need to work out if one of the reactants is in excess. The reactant that is not in excess is sometimes called the limiting reagent.

Basically- reactant that is used up the fastest and produces the least amount of product- reactant not in excess

20
Q

Three step to work out limiting factor and do example from white cards

A

1) Find masses and Mrs
2) Mol for one reactant
3) Look at big no. to find theoretical moles for other reactacnt- multiply moles by big no.
4) Find actual moles for reactant
5) Compare- if actual is less than theoretical then reactant is limiting
6) Limiting (actual) moles x big no. in front of product is product moles

21
Q

Steps to work out the empirical formula

A

Write the % or mass of each element

Divide each % or mass by that element’s Ar

Divide each answer by the smallest answer from above to find the simplest ratio

Def:The lowest whole number ratio of atoms of elements in a compound

Molecular formula= molar/empirical
Then multiply answer by empirical

Divide the actual molar mass by the mass of one mole of the empirical formula.

22
Q

Caffeine has a molar mass of 194 g. what is its molecular formula? Empirical formula = C4H5N2O1

A

molecular formula
= molar mass/ empirical formula mass
194/97=2

2 x C4H5N2O1= C8H10N402

23
Q

What do the gas laws look at relationships between?

A

Temp, pressure and volume

24
Q

Boyle’s Law

A

Boyle’s law -describes the relationship between PRESSURE and VOLUME.

The product of pressure multiplied by the volume of a gas in an enclosed container remains the same if either the pressure or volume changes and the temperature remains constant so…

P↑, V↓ and vice versa

If you double the pressure, vol of gas halves

PV= constant

25
Q

Charles’ Law

A

TEMP and VOLUME

If you DOUBLE the absolute temperature of a gas, the volume DOUBLES.

T↑V↑

V/T= constant

26
Q

Gay-Lussac’s law

A

Relationship between TEMP and PRESSURE

The pressure of a gas VARIES DIRECTLY with the absolute temperature of the gas when volume remains constant. (e.g think of empty deodorant can- is cold when empty)

T↑P↑

P/T= constant

27
Q

Combined Gas Laws- equation, what constant depends on, units etc

A

PV/T= constant

constant depends on the conditions used e.g- temp, press, moles of gas

If we have one mole of gas at a standard temp + press we can call this the gas CONSTANT represented by R

PV= nRT

R (given in Q)= 8.31 JK -1 mol-1
P= Pascals (Nm-1)
V=m^3
T=K

28
Q

Ideal gas equation

A

PV= nRT

R (given in Q)= 8.31 JK -1 mol-1
P= Pascals (Nm-1)
V=m^3
T=K
n= no. of moles
29
Q

Ideal Gas Def

A

In an ideal gas…

  1. Collisions are perfectly elastic
  2. No intermolecular attractive forces (i.e all internal energy = kinetic energy)
  3. Therefore does not condense into a liquid when cooled.

In reality, there are no gases that fit this definition perfectly. We assume that gases are ideal to simplify our calculations.

30
Q

Molar Volume def, how it can be calculated, rtp, equation, what it is at rtp

A

The volume occupied by 1 mole of a gaseous substance is called its molar volume.

Molar volume can be calculated from the density of the gas and its formula mass, Mr.

Since volume depends on both temperature and pressure, molar volume is generally measured at “room temperature and pressure”, rtp, which is about 20oC and 1 atmosphere.

DMV-
Density = mass/volume
rearranging this we get….

Molar volume = mass of 1 mole (Mr) /density at rtp.

The molar volume of any gas at rtp is approximately 24 dm3. Or, since there are 1000 cm3 in 1 dm3 The molar volume is also 24000 cm3.

31
Q

What can we calc from a balanced equation

A

How much of any given product can be made.

In the real world of industry there are 2 further important factors

  1. The yield of a reaction. (Usually expressed as a %)
  2. Atom economy. This is a theoretical value.
32
Q

Why might the theoretical yield fall short? What is the theoreyical yield equation?

A

Not all product is recovered (e.g. spattering, loss)

Reactant impurities (e.g. weigh out 100 g of chemical which has 20 g of junk)

A side reaction occurs

The reaction does not go to completion

Inaccuracy in measurement

(no. of moles of product/theoretical max no. of moles of product) x100
(actual/theoretical)x 100

33
Q

What is the % yield of NH3 if 40.5 g NH3 is produced from 20.0 mol H2 and excess N2?

A

Step 1: write the balanced chemical equation
N2 + 3H2 → 2NH3

Step 2: Calculate theoretical yield (actual is given):
1 mol H2 ≡ 2/3 mol NH3
20.0 mol H2 ≡ 13.3 mol NH3
Mass of NH3
13.3 x 17.0=227

Step 3: Calculate % yield

act/theo
(40.5/227)x100=17.87%

34
Q

cm3 to dm3 to m3

A

x1000→x1000→

/1000←/1000←

35
Q

Two moles calcs (one spec for titrations)

A 
mol/mass = conc x vol
mol= mass/Mr
36
Q

What does M mean in terms of conc?

A

Concentration is usually measured in mol/dm3 (moldm-3)
Sometimes concentration is referred to as ‘molar’
i.e 2M NaOH
This means the same as 2 moldm-3 of NaOH

37
Q

You have an unknown acid. How can you determine the concentration of this unknown acid?

A

We can use an alkali to react with the acid.

When the acid has been neutralised, the amount of alkali added allows us to determine the concentration of acid.

38
Q

You have an unknown concentration of HCl acid. 25.0cm3 of this acid is neutralised by 30.0cm3 of 0.10M NaOH. What is the concentration of acid?

A

1) Balanced eq
NaOH (aq) + HCl (aq) → NaCl (aq) + H2O (l)

2)moles of NaOH (known conc)
Moles NaOH = 0.10 x 30/1000 = 3.0 x 10-3 mol

3) Balanced equation: check mole ratio:
NaOH : HCl is 1:1

4) Amount (moles) HCl)
Moles = 3.0 x 10-3

5) Concentration of HCl
Conc. = 3.0 x 10-3/0.025= 0.12moldm-3

Chemistry 3.1 (8 decks)

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