3.1.2 Amount Of Substance Flashcards

1
Q

Write the formulas for the following common ions:

Silver
Zinc
Ammonium
Hydrogen

Nitrate
Sulphate
Carbonate
Hydrogencarbonate
Hydroxide
Hydride
Phosphate

A

Silver - Ag+
Zinc - Zn2+
Ammonium - (NH4)+
Hydrogen - H+

Nitrate - (NO3)-
Sulphate - (SO4)2-
Carbonate - (CO3)2-
Hydrogencarbonate - (HCO3)-
Hydroxide - OH-
Hydride - H-
Phosphate - (PO4)3-

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2
Q

How do we write chemical formulae?

A

Ensure that the charges on both ions are balanced, and therefore equal and opposite.

Eg. Barium Hydroxide

Ba2+ = 2+ charge and OH- = 1- charge

Ba(OH)2

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3
Q

What is the meaning of the ending ‘ate’?

A

Contains oxygen

Eg. Sulphate, carbonate, phosphate etc..

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4
Q

General equation for a substance reacting with oxygen?

A

Substance + oxygen -> oxides

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5
Q

General equation for reaction between metal and water?

A

Metal + water -> metal hydroxide + hydrogen

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6
Q

General equation for reaction between metal and acid?

A

Metal + acid -> salt + hydrogen

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7
Q

General equation for reaction between a hydrogencarbonate and acid?

A

Hydrogencarbonate + acid -> salt + water + carbon dioxide

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8
Q

General equation for the reaction between ammonia and acid?

A

Ammonia + acid -> ammonium salt

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9
Q

General equation for the thermal decomposition of a metal carbonate?

A

Metal carbonate -> metal oxide + carbon dioxide

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10
Q

General equation for reaction between metal oxide and acid?

A

Acid + metal oxide -> salt + water

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11
Q

General equation for reaction between metal hydroxide and acid?

A

Acid + metal hydroxide -> salt + water

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12
Q

General equation for the reaction between metal carbonate and acid?

A

Acid + metal carbonate -> salt + water + carbon dioxide

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13
Q

What is a salt?

A

When the hydrogen ion in an acid is replaced by a metal, it is a salt
-the first part of the salt is from the metal, and the second part is from the acid
-have the names: chloride, sulphate, nitrate and phosphate

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14
Q

How do you know when an equation is balanced?

A

The equation is balanced when there are the same number of each atom in the reactants, and in the products.

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15
Q

Define relative atomic mass?

A

The relative atomic mass is the average mass of one atom of an element, compared to one twelfth of the mass of an atom of carbon-12.

Ar = average mass of one atom of an element / 1/12th of the mass of an atom of carbon-12

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16
Q

How is the relative atomic mass of an element calculated?

A

-from the average mass of the isotopes of an element, weighted to their abundance

Ar = (% abundance 1 x mass 1) + (% abundance 2 x mass 2) etc… / 100

-these values are shown on the periodic table

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17
Q

Define relative molecular mass?

A

The relative molecular mass is the average mass of one molecule, compared to one twelfth of the mass of an atom of carbon-12.

Mr = average mass of one molecule / 1/12th mass of an atom of carbon-12

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18
Q

What is a molecule?

A

When there is a set number of atoms, in a set ratio.

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19
Q

What is the relative formula mass?

A

It is the relative mass used for ionic compounds, and is calculated in the same way as the Mr.

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20
Q

How is the Mr of a molecule found using Ar values?

A

By adding up the relative atomic masses of all of the atoms present in one molecule.

Eg. CO2 = 12 + (16x2) = 44

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21
Q

What is Avogadro’s constant?

A

The Avogadro’s constant is the number of particles in one mole of any substance

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22
Q

What is the value of Avogadro’s constant?

A

6.022 x 10^23

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23
Q

What is a mole?

A

A mole is an amount of a substance that contains 6.022 x 10^23 particles.
-the Ar or Mr of any atom or molecule will contain 6.022 x 10^23 individual atoms or molecules
-therefore, the Ar of an element is equal to the mass of one mole of its atoms in grams

Eg. Carbon

Ar = 12
Mass of 1 mole of carbon atoms = 12

24
Q

What is the equation linking mass, mr and moles?

A

Moles = mass/Mr

Or

Mass = Mr x moles

(Mass is measured in grams)

25
Q

What is a solvent?

A

The liquid in which the solute is dissolved to make a solution.

26
Q

What is a solute?

A

The substance that is dissolved in the solvent to make a solution. It can be a solid, liquid or a gas.

27
Q

What is a solution?

A

A solution is the substance formed when a solute has dissolved in a solvent.

28
Q

What is concentration?

A

Concentration of a solution refers to the amount of solute dissolved in a known volume of a solvent (usually in moldm-3 or gdm-3)

29
Q

How is concentration calculated?

A

Concentration = number of moles/volume

30
Q

What is the difference between a concentrated and dilute solution?

A

A concentrated solution has a high concentration of solute but a dilute solution has a low concentration of solute.

31
Q

How many cm3 are in 1 dm3?

32
Q

How do you convert from cm to dm?

33
Q

How do you convert from moles to grams?

A

divide by the Mr

34
Q

How do you calculate concentration from number of moles and volume?

A

Concentration = number of moles / volume

35
Q

What is a titration?

A

A method used to find the concentration of a solution, when one of the reagents is a standard solution.

36
Q

What is a standard solution?

A

A solution of which the exact concentration is known, so if a precise volume of it is measured, the number of moles can be calculated.

37
Q

What do we assume all gases behave like for calculations?

A

An ideal gas

38
Q

What do we assume all gases behave like for calculations?

A

An ideal gas

39
Q

How does an ideal gas behave?

A

Gas molecules are moving fast and randomly
Gas molecules do not attract or repel each other (no intermolecular forces)
The size of the particles is negligible

40
Q

What is the ideal gas equation?

A

PV = nRT

P=pressure in pascals
V=volume in m3
n=number of moles
R=molar gas constant - 8.31
T=temperature in Kelvin

41
Q

What is kelvin and how does it work?

A

Kelvin is another scale of temperature
0K = absolute zero, when particles have no kinetic energy
273K = 0*c
*c + 273 = K

42
Q

How do you covert from dm3 to m3?

43
Q

What are the standard conditions?

A

293K
100,000 Pa

1 mole of a gas under standard conditions occupies 24.3cm3.

44
Q

Define molecular formula

A

The actual number of each type of atom present in one molecule of the compound.

45
Q

Define empirical formula

A

The simplest whole number ratio of the atoms present in one molecule of a compound.

46
Q

What are the steps needed to calculate empirical formula?

A

Divide mass by Ar to calculate moles
Divide by the smallest moles to calculate mole ratio
Multiply to find the whole number ratio

47
Q

What is combustion analysis?

A

A method of determining the empirical formula
A sample of an unknown compound is burned in an excess of oxygen, and the products of combustion are analysed.
It is used for organic compounds.

48
Q

What are the 4 steps in a combustion analysis calculation?

A
  1. Mass of carbon
  2. Mass of hydrogen
  3. Mass of oxygen
  4. Calculate empirical formula
49
Q

Define anhydrous

A

An anhydrous substance is one that does not contain water.

50
Q

Define water of crystallisation

A

Water of crystallisation is water which is locked into a crystal in a fixed way.

51
Q

Define hydrated substance

A

A substance is hydrated if water, or the elects of water (hydrogen and oxygen in a 2:1 ratio) is added to it.

52
Q

What is percentage atom economy?

A

It is a method of calculating what percentage of the reactants should theoretically be converted into useful products in a reaction.
This measures the amount of waste produced and therefore the success of the reaction.

53
Q

What does it mean if a reaction has a high atom economy?

A

Mostly converted into useful product
If there is only one product, the atom economy is always 100%

54
Q

What is the equation to calculate percentage atom economy?

A

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

55
Q

What is percentage yield?

A

It gives information on the practical efficiency of a reaction, as no reactions ever produce a 100% yield.

56
Q

Why is a 100% yield never produced?

A

The reaction does not go to completion
Unwanted side reactions occur
The reaction is reversible

57
Q

What is the formula to calculate percentage yield?

A

(Mass of specific product formed / theoretical mass that could be formed) x 100