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Chem - Gas Laws Unit > Cards > Flashcards

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1
Q

Mass per periodic table

A

Mass increase down a group and the number of energy levels increases by 1 down a group

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2
Q

Empirical Formula of an ionic compound

A

Is the same as the formula compound

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3
Q

Hydrates

A

Compounds that have a specific number of water molecules attached to them

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4
Q

To find how many water molecules

A

We can heat the compound, the difference between the initial mass and the mass of the anhydrous compound is equal to the mass of water

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5
Q

Relation between coefficients and moles

A

They are equivalent (2 H2O = 2 moles)

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6
Q

Limiting Reactant

A

The substance that controls the quantity of product that can form in a chemical reaction

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7
Q

Theoretical yield

A

The maximum amount of product that can be produced from a given amount of reactant

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8
Q

Factors that may cause the experimental yield to be lower

A
  • Loss of products during purification
  • An incomplete reaction
  • Side reactions occurring
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9
Q

Factors that may cause the experimental yield to be higher

A
  • Impurities in a product
  • A product hasn’t been fully dried
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10
Q

Percentage yield

A

experimental yield/theoretical yield x 100

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11
Q

% atom economy

A

MM of Desired Product / MM of All Products x 100

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12
Q

Solute vs. Solvent

A

Solute : What is dissolved in a solution(salt)
Solvent : What dissolves the solute(water)

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13
Q

Concentration unit

A

mol dm-3 OR g dm-3

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14
Q

Molar concentration formula

A

c=n/v

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15
Q

Procedure for Preparing a Solution

A
  1. Accurately measure the mass of a solute
  2. Pour some distilled water to the volumetric flask
  3. Carefully add the solid to the flask
  4. Swirl the flask until all of the solute is dissolved
  5. Add the liquid solvent until it reacher the meniscus
  6. Place a cover on the flask and invert it back and forth to mix it
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16
Q

Moles in a solution vs diluted solution

A

The moles of the solute stay the same, adding more solvent

17
Q

Concentration and volume equation

A

C1V1 = C2V2

18
Q

Serial dilution

A

The process of diluting a sample several times

19
Q

Spectrophotometry

A

Measurement of the absorption of electromagnetic radiation of a substance at different wavelengths of the spectrum
Using to determine the concentration of coloured solutions
Interpolating on a graph

20
Q

Titration

A

A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete (neutralized)

21
Q

End point vs equivalence point

A

End point - experimental
Equivalence point - theoretical

22
Q

Avogradros law

A

States that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules and moles

23
Q

Volume vs mole

A

Proportional - as the number of particles of gas increase, the volume does if the pressure and temp are constant

24
Q

Ideal Gases

A

The volumes of the particles are barely anything compared to the volume that the gas occupies (spaces between particles are very large)
There are no intermolecular forces except when the particles collide

25
Q

Kinetic energy of gas particles

A

Is proportional to their temperature

26
Q

Pressure

A

The amount of force that is applied to a surface, more collisions = more pressure

27
Q

Volume and Pressure

A

When the volume of a gas increases, the pressure decreases

28
Q

Temperature and Pressure

A

Directly proportional

29
Q

Real gases pressure

A

There is less space between the wall and particles which creates more collisions but since there are intermolecular forces there is a lower pressure

30
Q

Boyles Law

A

If we increase the pressure of a fixed mass of a gas at a constant temperature, the volume will decrease
Inversely proportional
P = 1/V

31
Q

Boyles Law Equation

A

P1V1=P2V2
If temperature and number of molecules stays the same

32
Q

Charles Law

A

The law that states that for a fixed amount of gas at a constant pressure, the volume of the gas increases as the temperature of the gas increases and the volume of the gas decreases as the temperature of the gas decreases

33
Q

Charles Law Equation

A

V1/T1=V2/T2

34
Q

Kelvin vs Celsius

A

K= C + 273.15
C = K - 273.15

35
Q

Avrogado’s Law

A

One mole of any gas occupies the same volume at the same temperature and pressure

36
Q

STP Conditions

A

Temperature = 273 K
Pressure = 100 kPa
1 mol = 22.7dm3

37
Q

Combined Gas Law

A

(P1V1)/T1=(P2V2)/T2

38
Q

Ideal gas law

A

PV=nRT
Where R = 8.31

Chem - Gas Laws Unit (1 decks)

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