OpenStax Chapter 5 Key Terms Flashcards

1
Q

thermochemistry

A

study of the heat absorbed or released during chemical and physical changes

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2
Q

work

A

process of causing matter to move against an opposing force

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3
Q

potential energy

A

the energy that an object has because of its relative position, composition, or condition

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4
Q

kinetic energy

A

energy that an object possesses because of its motion

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5
Q

thermal energy

A

kinetic energy
associated with the random motion of atoms and molecules

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6
Q

exothermic process

A

releases heat
system gets colder, surroundings get warmer

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7
Q

endothermic process

A

absorbs heat
system gets warmer, surroundings get colder

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8
Q

temperature

A

quantitative measure of “hot” or “cold”
K, C, F

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9
Q

calorie

A

amount of energy required to increase the temperature of one gram of water 1 C

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10
Q

joule

A

amount of energy used when a force of 1 N moves an object one meter

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11
Q

heat capacity

A

quantity of heat (q) absorbed or released by a body of matter when it experiences a temperature change of 1 C
extensive

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12
Q

specific heat

A

quantity of heat required to raise 1 gram of a substance by 1 C
intensive

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13
Q

molar heat capacity

A

quantity of heat required to raise 1 mol of a substance by 1 C

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14
Q

calorimetry

A

method for measuring the amount o heat transferred to or from a substance

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15
Q

system

A

the substance or substances undergoing the chemical or physical change

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16
Q

surroundings

A

all other matter, including components of the measurement apparatus, that serve to either provide heat to the system or absorb heat from the system

17
Q

chemical thermodynamics

A

study of the relationship between heat, work, and other forms of energy involved in the

18
Q

internal energy

A

state function
energy associated with particles of the substance
depends on the state of the system
U = q + w

19
Q

expansion/pressure-volume work

A

expansion work
P𝚫V=-w
if work is done on the system, 𝚫V = -
if work is done by the system 𝚫V = +

20
Q

state function

A

depends only on the state of the system and not how the state is reached

21
Q

enthalpy

A

sum of the system’s internal energy (U) and the system’s pressure-volume work
H = U + PV
cannot be directly measured, so instead measure the change in enthalpy at constant pressure
extensive

22
Q

standard state conditions

A

1 atm, 1 M, 25 C

23
Q

enthalpy of combustion

A

enthalpy change when one mole of a substance burns under standard state conditions
reactants - products

24
Q

enthalpy of formation

A

enthalpy change for a reaction in which exactly one mole of a pure substance formed from free elements in their most stable form under standard state conditions

25
Hess's Law
if a process can be written as a sum of the several stepwise steps, the enthalpy change of the total process equals the sum of the enthalpy changes of the steps
26
heat of reaction
equal to the enthalpy under constant pressure