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Chemistry R120 > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

What is energy?

A

ability to do work or transfer heat

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2
Q

What is work?

A

energy used to cause an object that has mass to move over some distance

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3
Q

What is heat?

A

energy used to cause the temperature of an object to rise

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4
Q

What is thermodynamics?

A

the study of energy transformations

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5
Q

What is thermochemistry?

A

applies thermodynamics to chemcial reactions

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6
Q

What is kinetic energy?

A

energy an object has due to its motion

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7
Q

What is the equation of kinetic energy (KE)?

A

KE = 1/2 mv^2

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8
Q

What is potential energy?

A

energy an object has due to its position in space or chemcial composition (bonds it has)

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9
Q

What is electrostatic potential energy?

A

the potential energy in molecules | E(el)

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10
Q

What is the equation for electrostatic potential energy?

A

E(el) = (k Q1 Q2) / d

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11
Q

What is “k” in the electrostatic potential energy equation?

A

proportionality constant = 8.99 * 10^9 Jm/C^2

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12
Q

How many joules is 1 calorie?

A

4.18 J

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13
Q

What is the First Law of Thermodynamics?

A

energy is neither created nor destroyed as it can be converted into different forms

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14
Q

What is a “system”

A

the parts/stuff we want to study

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15
Q

What is “surroundings”?

A

everything else that surrounds the system

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16
Q

What is the equation for work?

A

w = Force x distance

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17
Q

What are 3 types of systems?

A

open | closed | isolated

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18
Q

What is an open system?

A

matter and energy can be exchanged with their surroundings

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19
Q

What is a closed system?

A

ONLY energy can be exchanged with surroundings NOT matter

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20
Q

What is an isolated system?

A

NEITHER energy and matter can be exchanged with surroundings

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21
Q

What is internal energy?

A

E | sum of ALL kinetic and potential energies of all components of the system

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22
Q

What are the 3 parts of thermodynamic quantities?

A

number | unit | sign (+) or (-)

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23
Q

What does a (+)delta E mean?

A

Ef > Ei | endergonic energy change

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24
Q

What is an endergonic energy change?

A

system GAINED / ABSORBED energy from surroundings

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25
Q

What does a (-)delta E mean?

A

Ef < Ei | exergonic energy change

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26
Q

What is an exergonic energy change?

A

system LOST / RELEASED energy into surroundings

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27
Q

What is the equation for the change in internal energy (delta E)?

A

q (heat) + w (work)

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28
Q

What does a +q mean?

A

system GAINS heat (increase temperature)

29
Q

What does a -q mean?

A

system LOST heat (decreased temperature)

30
Q

What does a +w mean?

A

work is done ON the system

31
Q

What does a -w mean?

A

work is done BY the system

32
Q

What is endothermic?

A

heat ABSORBED by the system

33
Q

What is exothermic?

A

heat RELEASED by the system

34
Q

What is a state function?

A

property of a system that is determined by specifiying the system’s condition/state in terms of temperature, pressure, etc.

35
Q

What does the value of the state function depend on?

A

ONLY the present state of the system INDEPENDENT from the path it took to get there

36
Q

How is internal energy (E) a state function?

A

depends ONLY on the initial and final states of the system | q and w are not state functions

37
Q

What is enthalpy?

A

heat flow

38
Q

What is the equation for enthalpy?

A

E + PV

39
Q

What is pressure-volume work (PV)?

A

work involved in the expansion or compression of gases

40
Q

What does deltaH = q(p) mean?

A

the change in enthalpy equals the heat (q) gained or lost at constant pressure

41
Q

What does a (-)deltaH mean?

A

exothermic

42
Q

What does a (+)deltaH mean?

A

endothermic

43
Q

What is the equation for deltaH for chemcial reactions?

A

Hproducts - Hreactants

44
Q

What is enthalpy of reaction?

A

enthalpy change that accompanies a reaction | deltaHrxn = heat of reaction

45
Q

What are thermochemical equations?

A

balanced chemical equations that show the associated enthalpy change

46
Q

What are the 3 “truths” about enthalpy?

A

its an extensive property | (+)deltaH in forward direction and (-)deltaH in reverse direction | deltaH for reactions depends on the state of products and reactants

47
Q

What does it mean that enthalpy is an extensive property?

A

magnitude of deltaH is proportional to the amount of reactant consumed in the process

48
Q

What is calorimetry?

A

the measurement of heat flow

49
Q

What is a calorimeter?

A

device used to measure heat flow

50
Q

What is heat capacity?

A

amount of energy required to raise the temperature of a substance by 1 K (1 degC) for 1 mol substance

51
Q

What is specific heat capacity?

A

amount of energy required to raised the temperature of 1g of substance by 1 K (1 degC)

52
Q

What is the equation for specific heat capacity (Cs)?

A

heat transferred (q) / (mass x temperature change)

53
Q

What must first be done when carrying out a reaction in aqueous solution in a constant-pressure calorimetry?

A

calculate the heat change for the water in the solution first

54
Q

In a constant-pressure calorimetry, what does exothermic indicate?

A

reaction lost heat which water gains (water is surroundings)

55
Q

In a constant-pressure calorimetry, what does exothermic indicate?

A

reaction gains heat which water lost

56
Q

What is q(soln)?

A

the heat gained or lost by the solution

57
Q

What is q(rxn)?

A

the heat gained or lost by the reaction

58
Q

What is the relationship between q(rxn) and q(soln)?

A

opposites of each other | q(soln) = -q(rxn)

59
Q

What is the Cs (specific heat capacity) of water?

A

4.184 J/gk

60
Q

What is the equation for heat(q)?

A

m Cs (deltaT) “mcAT”

61
Q

What is a bomb calorimeter?

A

constant-volume calorimetry that carries out combustion reactions

62
Q

What is a “bomb”?

A

small cup with insulated sealed vessel carrying out combustion reactions | designed to withstand high pressures

63
Q

What is a combustion reaction?

A

compound reacts completely with excess O2

64
Q

What is the heat equation for a bomb calorimetry?

A

q(rxn) = - C (deltaT)

65
Q

What does Hess’s Law state?

A

because H is a state function = deltaH for the overall reaction SHOULD EQUAL the sum of all enthalpy changes of each reaction from each step | H1 = H2 + H3

66
Q

What are enthalpies of formation (deltaHf)

A

enthalpy change for the reaction in which a compound is made from its constituent elements in their elemental forms

67
Q

What is the standard enthalpy of formation (deltaHof)?

A

enthalpy change of a compound for a reaction forming 1 mol compound

68
Q

What is bond enthalpy?

A

the enthalpy change for breaking a bond in 1mol of a gas

Chemistry R120 (18 decks)

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