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CHEMY102 > Physical Chemistry > Flashcards

Physical Chemistry Flashcards

1
Q

What is Boyles law

A

Relationship between pressure and volume

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2
Q

What is Boyles equation

A

P1V1=P2V2

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3
Q

What is Charles law

A

The relationship between volume and temperature

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4
Q

What is Charles equation

A

V1/T1=V2/T2

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5
Q

What is Avogadro’s law

A

The relationship between quantity and volume

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6
Q

What is Avogadro’s equation

A

V1/n1=V2/n2

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7
Q

What is Amontons law

A

The relationship between pressure and temperature

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8
Q

What is Amontons equation

A

P1/T1=P2/T2

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9
Q

What is the overall gas law equation

A

PV=nRT

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10
Q

What is the value of the R constant and what are the two common units used

A

8.314 JK-1Mol-1
Or
8.314 KPaLK-1Mol-1

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11
Q

What is Daltons law

A

The overall pressure is a sum of the partial pressures of the individual gases

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12
Q

To convert from 1 letre to m3 you must….

A

Divide by 1000

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13
Q

What does volatile mean

A

High boiling point

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14
Q

What is Grahams law

A

If P and T are constant, the rate of diffusion is inversely proportional to the square root of the gasses molar mass

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15
Q

What is effusion compared to diffusion

A

Effusion is the act of forcing a gas through a hole smaller than the mean path of partials. Diffusion is through a gap as big or bigger than the mean path of particals

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16
Q

What is a rigid thermodynamic system

A

A system that transfers heat but not work

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17
Q

What is an adiabatic thermodynamic system

A

A system that transfers work but not heat

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18
Q

What is the first law of thermodynamics

A

Energy is always conserved

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19
Q

What is the second law of thermodynamics

A

The entropy of the universe increases with a spontaneous reaction, if left alone a reaction will tend towards a higher probibility.

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20
Q

What is the third law of thermodynamics

A

That a pure crystalline solid at 0 Kalvin will have a delta S of zero

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21
Q

What is the equation demonstrating the first law of thermodynamics

A

deltaU=q+w (the sum of heat and work done)

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22
Q

What are state functions

A

‘Path independent’. It is determined by the initial and final states, not all the states to get to the final state.

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23
Q

What does PV mean and what is the equation

A

Pressure-volume work when gas undergoes a volume change

w=-PdeltaV

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23
Q

What is the opposite of state function

A

Path function

23
Q

What is enthalpy in terms of internal energy and PV work

A

H=U+PV

24
Q

What is the term for a reaction under constant pressure

A

Isobaric

24
Q

What is Hess’s law

A

The sum of enthalpy changes for a whole reaction can be found using the enthalpy change of differing reaction steps as enthalpy is a state function and pathway independent

24
Q

What is the term for a reaction under constant volume

A

Isochoric

25
Q

Does enthalpy tabulated data have a zero value

A

No

26
Q

What is deltaHf

A

This is the enthalpy change in formation of the species from its elements in their standard states

27
Q

What is the deltaHf of elements in their most stable state. E.G. O2

A

Zero

28
Q

What does deltaHr’ mean

A

This is a reactions enthalpy in standard conditions (1 bar pressure and 25 degrees). This allows for reactions to be comparable

29
Q

What is the heat capacity refer to

A

The amount of heat required to heat to raise the temperature by 1 degree

30
Q

What is the difference between heat capacity “C” and “c”

A

C is for molar, c is for grams (specific heat capacity)

31
Q

What is the equation for c

A

c=q/(mxdeltaT)

32
Q

What is the difference between K and Q

A

Q refers to the reaction quotient when the reaction is not in equilibrium. K refers to the reaction equilibrium when the reaction is at equilibrium, denoted with ‘e’ beside the concentrations

33
Q

What can be used instead of concentration in the equilibrium constant if only gasses are involved

A

Partial pressures

34
Q

What does it mean if K=Q

A

Equilibrium

35
Q

What does it mean if Q>K

A

The concentration of products exceeds reactants

36
Q

What does it mean if Q<K

A

The concentration of reactants exceeds the products

37
Q

Does entropy have an absolute zero

A

Yes

38
Q

What is a reversible reaction

A
  • Conceptual
  • Occurs over a infinite tine
  • system and surroundings return to their original states
  • always in equilibrium
  • results in max work done by the system
39
Q

Total entropy of a reaction is……..

A

deltaS surroundings+deltaSsystem

40
Q

What is Gibbs free energy and its equation

A

Alternative function to entropy to predict natural direction. deltaG=deltaH-deltaSxT

41
Q

Why is Gibbs preferred

A

You only have to know the data for the system

42
Q

What is the reaction for deltaG in not standard state

A

deltaG=deltaG’+RTlnQ

43
Q

What unit must be used for deltaG’

A

JMol-1

44
Q

What 4 things affect kinetics of a reaction

A
  • Physical states
  • Concentration of reactants
  • The temperature that the reaction occurs at
  • The presence of a catalyst
45
Q

What is the rate of reaction for 2A -> B

A

-1/2[A]/dT = [B]/dT

46
Q

What is the unit for a zero order reaction

A

MolL-1s-1

47
Q

What is the unit for a first law reaction

A

s-1

48
Q

What is the unit for a second law reaction

A

LMol-1s-1

49
Q

What is the unit for a third law reaction

A

L2Mol-2s-1

50
Q

What is the cool feature of one of the rate order half life plot

A

First order reaction has a constant half life length

51
Q

What is theorized to exist at the peak of the activation energy curve

A

A activator complex at the transition state

52
Q

What does the Arrhenius equation involve

A

Links the rate constant to activation energy

53
Q

What does A refer to in the Arrhenius equation

A

This is the preexponential factor, the frequency of collisions and the probibility the collisions are successful- slight dependance on temperature so only approx

54
Q

What is a homogenous catalyst

A

A catalyst in the same phase as the reactants, is regenerated

55
Q

What is a heterogenous catalyst

A

A catalyst that is of differing phase to the reactants, usually a metal that the reactants can react on, provides surface area for reactants to get into correct orientation

CHEMY102 (4 decks)

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