Unit 6 Flashcards

1
Q

System

A

the place that the experiment is held

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2
Q

surroundings

A

everything that surrounds the system

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3
Q

open system

A

energy and matter is transfered from surroundings

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4
Q

closed system

A

only energy is transferred from the surroundings

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5
Q

isolated system

A

nothing is transferred from the surroundings

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6
Q

State Function

A

a measurement of thermodynamics that only depends on the initial and final states, nothing in between matters

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7
Q

extensive properties

A

properties at non standard states

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8
Q

intensive properties

A

properties at standard states, signified by naught

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9
Q

standard state

A

1 atm
1 mol/whatever stochiometric coeff

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10
Q

exo -

A

negative value

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11
Q

endo -

A

positive value

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12
Q

Kinetic Energy (KE) equation

A

1/2 (mass)(volume)^2 = (kg) x (m/s)^2 = Joules

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13
Q

Potential Energy (PE)

A

stored energy

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14
Q

Potential Energy equation

A

K(qq / r ) = (constant) [(charges) / (distance)]

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15
Q

Energy equation

A

E = PE + KE

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16
Q

First Law of Thermodynamics Law of Conservation

A

Energy cannot be created or destroyed

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17
Q

How do we measure Energy?

A

heat

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18
Q

Specific heat

A

Raising one gram of a substance by one C

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19
Q

1 calorie is…

A

4.184 Joules

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20
Q

heat equation (q)

A

q = mcΔT

m = mass in grams
c = specific heat
T = temp change in Kelvin or C

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21
Q

What is the unit of heat?

22
Q

Equation of Delta E

A

q + w
= (heat) + (work)

q + PΔV

23
Q

Hess’s Law

A

Operation performed on equation is performed on the heat of the reaction

24
Q

Formation Reaction

A

Where reactants are made from their basic elements from their purest form
1 mol
1 atm

25
Q

Heat of Formation

A

the amount of heat needed for a formation reaction

26
Q

ΔH (naught) equation for a reaction

A

Σ(ΔH of formation of products) - Σ(ΔH of formation of reactants)

OR

ΔH ≈ Σ(bond energies of reactants) - Σ(bond energies of products).

27
Q

specific heat capacity vs molar heat capacity

A

one gram vs one mol

28
Q

If work is done ON the system, the sign is…

29
Q

If work is done BY the system, the sign is…

30
Q

Enthalpy

A

Heat produced or absorbed by a reaction

31
Q

Delta H/Enthalpy change equation

A

(H products) - (H reactants)

32
Q

Bomb Calorimeter

A

Constant Volume

33
Q

Bomb Calorimeter Equation of Delta E

34
Q

Pressure constant Calorimeter

A

ΔE = ΔH - PΔV

35
Q

Energy needed to break bonds are always…

36
Q

What does Gibbs Free Energy Measure?

A

Determining the amount of energy available from any chem reaction, which determines spontaneity

37
Q

Gibbs Free Energy Equation

A

ΔG = ΔH - TΔS

OR

ΔG _0 (products) - ΔG _0(reactants)

38
Q

What type of reactants are spontateous?

A

NEGATIVE G value

39
Q

ΔG _0

A

At standard temp

40
Q

ΔG _0 and ΔG relationship

A

ΔG = ΔG° + RTlnQ

41
Q

When is Q = K, and what does K tell us?

A

at equilibrium

k > 1 = products are favored, spontaneous
k < 1 = reactants are favored, nonspontaneous

42
Q

Entropy (S)

A

The number of disorders in a system

43
Q

higher particles mean…

A

higher entropy

44
Q

higher volume mean..

A

higher entropy

45
Q

change of state (!) mean…

A

higher entropy

46
Q

above all, more gaseous particles mean…

A

higher entropy

47
Q

Entropy of elements are…

A

NOT zero, like delta H and delta G

48
Q

Boltzmann Equation

A

S = k ln W

k = constant
W = microstates

49
Q

Delta S naught

A

ΔS° = Σ (ν * S°(products)) - Σ (ν * S°(reactants))

50
Q

Entropy in a reversable process

A

S = q rev / T = ( heat added) / (T) = J / K