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IB Chemistry SL > Stoichiometric Relationships > Flashcards

Stoichiometric Relationships Flashcards

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1
Q

What are the different changes of state

A

melting, freezing, vaporization (evaporation and boiling), condensation, sublimation and deposition.

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2
Q

What is a homogenous mixture

A

A homogeneous mixture is simply any mixture that is uniform in composition throughout. (components are combined)

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3
Q

what is a heterogenous mixture

A

A heterogeneous mixture is a mixture that composes of components that are physically separate

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4
Q

what do physical and chemical properties depend on

A

the way atoms combine

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5
Q

What is a mole?

A

a mole is the amount of substance that contains L particles of that substance.
The mass of one mole of any substance is known as the molar mass and has the symbol M.

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6
Q

What is the RAM

A

the relative atomic mass of an element (Ar) is the weighted mean of all the naturally occurring isotopes of the element relative to carbon-12.
Units: mol^-1 or Mr
-used to compare the masses of moles

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7
Q

What is avagadros constant for 1 mole

A

6.022 x10^23

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8
Q

what is avagadros law

A

THE EQUAL VOLUMES OF DIFFERENT GASES AT THE SAME TEMPERATURE AND PRESSURE CONTAIN THE SAME NUMBER OF MOLES

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9
Q

what does avagadros law explain

A

one mole of any gas will occupy the same volume at the same temperature and pressure. This is known as the molar volume of a gas.

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10
Q

what variables do you change for a fixed mass in gas

A

temperature (kinetic energy), volume(concentration of particles) and pressure( decrease in volume=increase in concentration=faster moving particles)

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11
Q

properties of chemical reactions

A
  • new substances are formed
  • bonds in the reactants are broken and bonds in the products are formed resulting in an energy change between the reacting system, and its surroundings
  • there is a fixed relationship between the number of particles of reactants and products resulting in no overall change in mass- this is known as the stoichiometry of the reaction
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12
Q

State symbols

A

(s) -solid
(l) -liquid
(g) -gas
(ag) - in an aqueous solution

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13
Q

What 3 formulas for compounds exist

A

empirical, molecular, structural

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14
Q

what is the empirical formula

A

simplest whole number ratio of atoms of each element in a particle of substance

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15
Q

what is the molecular formula

A

shows the actual number of atoms of each element in a molecule of the substance. Can be obtained from the empirical formula if the molar mass of the compound is known.

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16
Q

what is the structural formula

A

-shows the arrangement of atoms and bonds within a molecule

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17
Q

properties of the solid state

A
  • fixed shape
  • fixed volume
  • particles held together by intermolecular forces in a fixed position
  • particles can vibrate about a fixed point but do not translational velocity
  • as heat is supplied at a certain temperature the vibration is sufficient to overcome the attractive forces holding the solid together and the solid melts
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18
Q

properties of the liquid state

A
  • fixed volume
  • takes up shape of the container
  • particles held closely together by intermolecular forces
  • particles have translational velocity so diffusion can occur
  • as heat is supplied the liquid particles move faster than others and escape from the surface of the liquid to form a vapour. Once the pressure of the vapour is equal to the pressure above the liquid; the liquid boils
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19
Q

properties of the gaseous state

A
  • widely spaced particles that completely fill the container
  • pressure of the gas due to gaseous particles colliding with the walls of the container
  • intermolecular forces between particles negligible
  • volume occupied by molecules themselves negligible compared with total volume of gas
  • particles moving with rapid, random motion so diffusion can occur
20
Q

units of molar mass (M)

A

g mol

21
Q

what is a standard solution

A

a solution of known concentration, consisting of a solute and a solvent

22
Q

what can can reactants sometimes be

A

limiting or excess (stoichiometry CHECK)

23
Q

what is the experimental yield and the theoretical yield

A

experimental yield= substance produced in experiment

theoretical yield= substance on average theoretically produced

24
Q

what is a mixture

A

when substances combine without chemical interaction

25
Q

in what states does matter exist and what is it determined by

A

solids, liquids and gases:

determined by temperature, volume and pressure and the increasing kinetic energy of particles

26
Q

what is kinetic energy

A

energy that a body possesses by virtue of being in motion

27
Q

what is the kinetic theory of matter

A

the average kinetic energy of the particles is directly related to the temperature of the system

28
Q

what are inter-particle forces

A

the state of matter at a given temperature and pressure determined by the strength of the forces between particles

29
Q

Changes of state explanation

A

As the solid is heated, the vibrational energy of its particles increases and so the

temperature increases.

b–c This is the melting point. The vibrations are suf ciently energetic for the

molecules to move away from their xed positions and form liquid. Energy

added during this stage is used to break the inter-particle

forces, not to raise the kinetic energy, so the temperature

remains constant.

c–d As the liquid is heated, the particles gain kinetic energy and so

the temperature increases.

d–e This is the boiling point. There is now suf cient energy to

break all of the inter-particle forces and form gas. Note that

this state change needs more energy than melting, as all the

inter-particle forces must be broken. The temperature remains

constant as the kinetic energy does not increase during this

stage. Bubbles of gas are visible throughout the volume of the

liquid.

e–f As the gas is heated under pressure, the kinetic energy of its

particles continues to rise, and so does the temperature.

30
Q

difference between Mr and Ar

A

Mr:relative formula mass: used to compare masses of compounds
Ar: relative molecular mass: used to compare masses of atoms

31
Q

what is hydrated salt

A

compounds that contain a fixed ratio of of water molecules (water of crystallization)

32
Q

what reactant determines the quantity of product

A

the limiting reactant

33
Q

formula for percentage yield

A

experimental yield/theoretical yield x100

34
Q

what does the atomic theory state

A

all matter is composed of atoms that can’t be created or destroyed, and are rearranged during chemical reactions

35
Q

classification of matter into elements, compounds and mixtures

A

MATTER

  1. Mixture
    a. homogenous
    b. hetergenous
  2. Pure Substance
    a. element
    b. compound
36
Q

Boyle’s Law Formula (pressure and volume)

A

V1P1=V2P2

37
Q

Charles Law Formula (temperature and volume)

A

V1/T2=V2/T2

38
Q

Gay-Lussacs Formula (Temperature and pressure)

A

P1/T2=P2/T2

39
Q

Combined Gas Formula (T, P and V)

A

p1V1/t1=p2v2/t2

40
Q

what is the volume of 1 mole of any gas at STP

A

22.7 dm3

41
Q

what is STP

A

standard temperature pressure

42
Q

what is RTP

A

room temperature pressure

43
Q

how do you convert celsius to kelvin +what are the units

A

C + 273= kPA

44
Q

concentration formula

A

concentration= n(number of moles)/v(volume in dm3)

45
Q

atom economy formula

A

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

IB Chemistry SL (7 decks)

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