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Chemistry > Stoichiometry > Flashcards

Stoichiometry Flashcards

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1
Q

Define an element

A

a substance that is made up of only one type of atom

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2
Q

Define compound

A

a substance made up of two or more elements that are chemically bonded together

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3
Q

Define mixture

A

a substance made up of two or more elements that are not chemically bonds together

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4
Q

Difference between homogeneous and heterogeneous mixture

A

Homogeneous: has the same uniform appearance and composition throughout
Heterogeneous: has non-uniform appearance and composition throughout

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5
Q

What are the different types of states of matter + describe them

A

melting (solid - liquid), freezing (liquid - solid), boiling (liquid -gas), condensation (gas - liquid), sublimation (solid- gas), deposition (gas - solid)

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6
Q

Properties of solids

A
  • particles are packed closely together
  • particles vibrate
  • has definite volume, shape
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7
Q

Properties of liquids

A
  • particles slide over each other
  • has definite volume but no definite shape
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8
Q

Properties of gas

A
  • particles are very far apart
  • has no definite volume or shape
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9
Q

Physical change vs chemical change

A

Physical: no new substances are made + reversible
Chemical: new substance are made + irreversible

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10
Q

Define mole

A

the amount of substance that contains the same number of specified particles s there is in 12g of carbon-12

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11
Q

What is the value of the Avogadro constant

A

6,02x10^23

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12
Q

Define Relative Atomic Mass

A

the weighted average mass of one atom compared to 1/12th of the mass of an atom of carbon-12

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13
Q

How to calculate the relative isotopic mass

A

Multiply the atomic mass by the percentage abundance for each isotope and add them all together. Divide by 100 to get average relative atomic mass.

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14
Q

What are the units of molar mass

A

g/mol

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15
Q

How to find the number of particles

A

Avogadro’s constant X n° moles
be careful if they ask particles or molecules
(O2 = 2 particles but 1 molecule)

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16
Q

How to find the mass

A

moles X Mr

17
Q

How to find the Mr

A

Mass÷moles

18
Q

How to find the number of moles

A

Mass÷Mr OR n° particles÷Avogadro

19
Q

Empirical formula definition

A

The simplest whole-number ratio of each element in a compound

20
Q

Formula for atom economy

A

(total mass of desired products÷total mass of all products) x 100

21
Q

How to calculate the empirical formula

A

1) Write each elements % composition or mass
2) Divide the % or mass by the relative atomic mass and calculate the ratio
3) Divide each ratio by the smallest ratio above to get a whole number ratio

22
Q

How to calculate the molecular formula

A

1) Calculate the relative mass of the empirical formula
2) Divide the relative mass of x by its empirical formula’s lass
3) Multiply the empirical formula by the number found

23
Q

What is the limiting reactant

A

The reactant that is going to be used up first

24
Q

How to find the limiting reactant

A

Divide the moles by the leading coefficient (the smaller t one is the limiting reactant)

25
Q

Percentage yield formula

A

actual yield/theoretical yield

26
Q

What is the ideal gas formula

A

Pv=nRT
P=(Pa), V=m3, n= n° moles, R= gas constant, T= (K)

27
Q

Characteristics of Ideal Gases

A
  • volume of gas is negligible
  • have perfect elastic collision
  • no intermolecular forces
28
Q

State 2 reasons why which cause deviations from ideal gas behaviour

A
  • volume ( a large volume)
  • intermolecular forces (stronger intermolecular forces like H bonds)
29
Q

When do real gases behave the most like ideal gases

A

high pressure and low temperatures

30
Q

How to calculate the gas volume

A

moles X 22.7dm3

31
Q

What is Boyle’s law (relationship between pressure and volume)

A

volume is inversely proportional to pressure (at constant temperature)
P=1/V (straight line)

32
Q

What is Charles’ Law (relationship between volume and temperature)

A

volume is directly proportional to temperature (at constant pressure)
V=T

33
Q

What is Lussac’s Law (relationship between temperature and pressure)

A

pressure is directly proportional to temperature (at constant volume)
P=T

34
Q

What is the combined gas law formula

A

P1V1/T1 = P2V2/T2

35
Q

How to calculate concentration

A

moles/volume

Chemistry (12 decks)

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