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Chemistry R120 > Chapter 5 > Flashcards

Chapter 5 Flashcards

(68 cards)

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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
What does a (-)delta E mean?
Ef < Ei | exergonic energy change
26
What is an exergonic energy change?
system LOST / RELEASED energy into surroundings
27
What is the equation for the change in internal energy (delta E)?
q (heat) + w (work)
28
What does a +q mean?
system GAINS heat (increase temperature)
29
What does a -q mean?
system LOST heat (decreased temperature)
30
What does a +w mean?
work is done ON the system
31
What does a -w mean?
work is done BY the system
32
What is endothermic?
heat ABSORBED by the system
33
What is exothermic?
heat RELEASED by the system
34
What is a state function?
property of a system that is determined by specifiying the system's condition/state in terms of temperature, pressure, etc.
35
What does the value of the state function depend on?
ONLY the present state of the system INDEPENDENT from the path it took to get there
36
How is internal energy (E) a state function?
depends ONLY on the initial and final states of the system | q and w are not state functions
37
What is enthalpy?
heat flow
38
What is the equation for enthalpy?
E + PV
39
What is pressure-volume work (PV)?
work involved in the expansion or compression of gases
40
What does deltaH = q(p) mean?
the change in enthalpy equals the heat (q) gained or lost at constant pressure
41
What does a (-)deltaH mean?
exothermic
42
What does a (+)deltaH mean?
endothermic
43
What is the equation for deltaH for chemcial reactions?
Hproducts - Hreactants
44
What is enthalpy of reaction?
enthalpy change that accompanies a reaction | deltaHrxn = heat of reaction
45
What are thermochemical equations?
balanced chemical equations that show the associated enthalpy change
46
What are the 3 "truths" about enthalpy?
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
What does it mean that enthalpy is an extensive property?
magnitude of deltaH is proportional to the amount of reactant consumed in the process
48
What is calorimetry?
the measurement of heat flow
49
What is a calorimeter?
device used to measure heat flow
50
What is heat capacity?
amount of energy required to raise the temperature of a substance by 1 K (1 degC) for 1 mol substance
51
What is specific heat capacity?
amount of energy required to raised the temperature of 1g of substance by 1 K (1 degC)
52
What is the equation for specific heat capacity (Cs)?
heat transferred (q) / (mass x temperature change)
53
What must first be done when carrying out a reaction in aqueous solution in a constant-pressure calorimetry?
calculate the heat change for the water in the solution first
54
In a constant-pressure calorimetry, what does exothermic indicate?
reaction lost heat which water gains (water is surroundings)
55
In a constant-pressure calorimetry, what does exothermic indicate?
reaction gains heat which water lost
56
What is q(soln)?
the heat gained or lost by the solution
57
What is q(rxn)?
the heat gained or lost by the reaction
58
What is the relationship between q(rxn) and q(soln)?
opposites of each other | q(soln) = -q(rxn)
59
What is the Cs (specific heat capacity) of water?
4.184 J/gk
60
What is the equation for heat(q)?
m Cs (deltaT) "mcAT"
61
What is a bomb calorimeter?
constant-volume calorimetry that carries out combustion reactions
62
What is a "bomb"?
small cup with insulated sealed vessel carrying out combustion reactions | designed to withstand high pressures
63
What is a combustion reaction?
compound reacts completely with excess O2
64
What is the heat equation for a bomb calorimetry?
q(rxn) = - C (deltaT)
65
What does Hess's Law state?
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
What are enthalpies of formation (deltaHf)
enthalpy change for the reaction in which a compound is made from its constituent elements in their elemental forms
67
What is the standard enthalpy of formation (deltaHof)?
enthalpy change of a compound for a reaction forming 1 mol compound
68
What is bond enthalpy?
the enthalpy change for breaking a bond in 1mol of a gas

Chemistry R120 (18 decks)

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