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Physical Flashcards

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1
Q

What is the zeroth law of thermodynamics?

A

If system A is in thermal equilibrium with B, and B is in thermal equilibrium with C, then C is also in equilibrium with A

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2
Q

What is the first law of thermodynamics?

A

Energy cannot be created or destroyed but it can be converted into another form

ΔU = q + w

ΔU = internal energy
q = heat
w = work
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3
Q

When work is done on a system, is w positive or negative?

A

Positive

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4
Q

When heat is gained by a system, is q positive or negative?

A

Positive

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5
Q

What are adiabatic systems?

A

Thermally insulated, isolated systems

Heat is not involved

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6
Q

What is an isothermal system?

A

Closed, not thermally isolated systems

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7
Q

What is an isovolumetric process?

A

Volume is constant, pressure and temperature can change

Heat is allowed to enter

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8
Q

What is an isobaric process?

A

Pressure is constant, volume and temperature can change

Heat is allowed to escape

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9
Q

What is an isothermal process?

A

Temperature is constant, pressure and volume can change

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10
Q

Adiabatic process

A

Pressure, volume and temperature can all change

Heat isn’t allowed to escape

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11
Q

What is the second law of thermodynamics?

A

ΔS univ > 0

Heat cannot spontaneously flow from a colder location to a hotter location

The total entropy of the universe always increases

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12
Q

What is the third law of thermodynamics?

A

S T=0 >= 0

As a system approaches absolute zero all thermal processes cease and entropy approaches a minimum

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13
Q

What is a perfect crystal?

A
  • when entropy = 0

- atoms or ions are arranged in a regular, uniform way

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14
Q

What is enthalpy and how can it be calculated from internal energy?

A

A measure of the total energy of a thermodynamic system

H = U + PV

U= internal energy

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15
Q

What are the two types of calorimeter?

A
  • constant volume

- constant pressure

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16
Q

Define specific heat capacity

A

The energy required to raise the temperature of 1g of substance by 1°C

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17
Q

State Hess’s Law

A

The enthalpy change for a reaction is independent of the route taken

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18
Q

Define electron affinity

A

The energy released when an electron is added to a gaseous atom

X(g) + e- -> X^- (g)

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19
Q

Define energy of atomisation

A

The energy needed to transform an element in its standard state into 1 mole of gaseous atoms

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20
Q

How does heat differ from temperature?

A

Heat is a measure of thermal energy flow

Temperature is the average thermal energy per atom

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21
Q

What is thermal energy?

A

The kinetic and potential energy associated with the movement of individual molecules and atoms

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22
Q

What is bond dissociation enthalpy and how does it differ from bind energy?

A

Bind dissociation enthalpy is the energy required to break 1 mole of specific binds at RTP

BDE is specific for a particular bind in a particular molecule

Bond energy is the average value to break a bond across various molecules

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23
Q

What is a spontaneous reaction?

Study These Flashcards
A

A reaction that does occur under specific conditions

24
Q

What is a non-spontaneous reaction?

Study These Flashcards
A

A reaction that does not occur under specific conditions

25
Define standard entropy of reaction
The entropy change for a reaction carried out at 1 atm and 298K Units of J K-1 mol-1
26
Define Gibbs free energy
The energy available to do work at constant pressure
27
Which gas law relates pressure and volume? | Give the equation for it
Boyle's law P1 V1 = P2 V2
28
What does Gay-Lussac's law involve? Give the equation
Temperature and pressure P1 / T1 = P2 / T2
29
What does Charles's law relate? Give the equation
Temperature and volume V1 / T1 = V2 / T2
30
What relates volume and amount in gases? Give the equation
Avogadro's law V1 / n1 = V2 / n2
31
Explain why the behaviour of a real gas might be different to predictions made using the ideal gas law
In an ideal gas, molecules do not attract or repeal one another The volume is negligible compared with the volume of the container Real gases act like ideal gases at 0°C and 100 kPa
32
How would you calculate the density of a gas?
d = Mr P / RT
33
What is the equation for calculating concentrations of gases?
C = P /RT
34
What is Dalton's law of partial pressures?
The total pressure of a mixture of gases is just the sum of the pressures that each gas would exert if it were present alone
35
What does Boyle's law state?
For a fixed mass of gas at constant temperature, the volume is inversely proportional to the pressure
36
What does Charles's law state?
For a fixed mass of gas at constant pressure, the volume is directly proportional to the temperature
37
What does Gay-Lussac's law state?
The pressure of a fixed amount of gas at a constant volume is proportional to temperature
38
What does Avogadro's law state?
The volume of a gas maintained at a constant pressure and temperature is proportional to the amount of gas
39
What is the equation for calculating the partial pressure of a gas?
P = mole fraction x total pressure
40
What is the equation for calculating mole fraction of a gas?
X = no. of moles of gas A / total number of moles of gas
41
What is Le Cháteliers principal?
A system at equilibrium will oppose any change made to the system
42
Equation that links equilibrium constant with Gibbs free energy
ΔG° = -RT ln(k)
43
What is a bronsted acid?
Proton donor
44
What is a bronsted base?
A proton acceptor
45
What is the Henderson-Hasselbalch equation?
pH = pKa + log10([A-] / [HA])
46
Explain what is meant by rate law and reaction order
Rate law expresses the relationship of the rate of a reaction to the rate constant and the concentrations of the reactants raised to some power Reaction order is the sum of the individual orders in a reaction (the overall order)
47
What is the intergrated rate equation for a zeroth order reaction?
[A] = [A]0 - nkt
48
What is the equation for calculating the half-life of a zeroth order reaction?
t 1/2 = [A]0 / 2nk
49
What is the integrated rate equation for a first order reaction?
[A] = [A]0 e^(-nkt)
50
What is the equation for calculating the half-life of a first order reaction?
t 1/2 = ln(2) / nk
51
What is the integrated rate equation for a second order reaction?
1/[A] = 1/[A]0 + nkt
52
What is the equation for calculating the half-life of a second order reaction?
t 1/2 = 1/ nk [A]0
53
What is half-life?
The time taken for the concentration of a reactant to drop to half of its initial value
54
What is the equation relating Kp to Kc?
Kp = Kc (RT)^Δn
55
What is the equation relating Kp to Kc?
Kp = Kc (RT)^Δn

CHEMISTRY (18 decks)

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