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chem 30 > thermochemistry (unit a) > Flashcards

thermochemistry (unit a) Flashcards

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1
Q

spontaneous

A

something inclined to happen
-driven toward the end

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2
Q

potential energy

A

stored energy

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3
Q

kinetic energy

A

energy of motion
-movement
-temperature

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4
Q

kelvin equivalent to celcius

A

0C=273.15K

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5
Q

changes in motion correspond with changes in

A

kinetic energy

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6
Q

entropy

A

measure of disorder in a system
-randomness and speed

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7
Q

increased entropy factors

A

-increase in moles of gas molecules
-state changes
-increase in temperature
generally more motion

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8
Q

kinetic molecular theory

A

moving particles will interact more or less strongly with each other
-depending on the states
-motion inc as temp inc

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9
Q

temperature increase affects motion…

A

motion increases

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10
Q

temperature

A

measure of average kinetic energy of the particles of a system

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11
Q

heat

A

transfer of thermal energy between two systems

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12
Q

where is potential energy stored

A

within bonds between molecules and within molecules

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13
Q

energy is ____ to break bonds

A

required

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14
Q

energy is ____ when bonds are formed

A

released

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15
Q

enthalpy change

A

basis of all change due to energy transformation

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16
Q

simple example of enthalpy change

A

solar energy - glucose - hydrocarbons

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17
Q

second law of thermodynamics

A

heat will flow from a high to low until thermal equilibrium is reached
-warm cup of tea

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18
Q

how exactly does heat transfer

A

as particles collide they transfer energy via conduction until all paarticles have the same kinetic energy

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19
Q

kinetic energy calculation FORMULA

A

Q= mcΔt

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20
Q

specific heat

A

amount of energy required/released when one kilogram of the substance is raised or changes in temperature by one degree

21
Q

when is Q positive

A

energy is being released from system
-exothermic
-Δt is also positive

22
Q

when is Q negative

A

energy is being absorbed from surroundings
-endothermic
-Δt is negative

23
Q

endothermic reaction

A

absorgbs energy from surroundings
-reactants has less potential than products
-ΔH is (+)

24
Q

energy has been put into the reaction

A

endothermic

25
Q

exothermic reaction

A

energy is being released to surroundings
-reactants has more potential than products
-ΔH is (-)

26
Q

something that is endothermic in one direction will be _____ in the other direction

A

exothermic

27
Q

collision theory

A

in order for a reaction to happen
-molecules must collide
-in proper orientation
-minimum amount of energy (activation energy)

28
Q

activation energy

A

minimum amount of energy required to initiate reaction
-increase frequency of collisions

29
Q

factors of a faster reaction

A

increased collisions
-increased concentration
-increased temperature
-increased surface area (solid)

30
Q

activated complex

A

temporary chemical species, temporarily formed by reactant molecules as a result of collision
-prior to product

31
Q

breaking bonds

A

absorbs energy
-endothermic
bonded particle + energy –> seperate particle

32
Q

making bonds

A

releases particles
-exothermic
seperate particles —> bonded particle + energy

33
Q

catalysts

A

changes the rate of reaction without being used up
-same amount of particle
-lowers activation energy
-doesn’t alter enthalpy change

34
Q

potential energy of the reactants and particles is ____ with or without a catalyst

A

the same

35
Q

enthalpy change

A

the difference between enthalpies of the products and the enthalpies of the reactants
-total energy change for a chemical reaction

36
Q

molar enthalpy change

A

the enthalpy change per one mole of any substance involved in the chemical reaction
-porportions that react

37
Q

calorimeter

A

device used to measure energy changes in a chemical reaction, results in temperature change

38
Q

exothermic calorimeter

A

increase kinetic energy of the water
-inc temperature

39
Q

endothermic calorimeter

A

decrease kinetic energy of the water
-decrease temp

40
Q

assumptions of calorimeters

A

there is no energy lost
-same amount absorbed and released

41
Q

first law of thermodynamics

A

energy can be transferred or change form
-cannot be created or destroyed

42
Q

second law of thermodynamics

A

energy flows from high regions to low until equilibrium is established

43
Q

four calorimeter assumptions

A
  1. heat is not lost (isolated)
  2. heat not absorbed by calorimeter
  3. specific heat capacity is water
  4. reactions take place at constant pressure
44
Q

heat capacity

A

-heat required to raise temperature of an object by one degree celcius
-no mass

45
Q

Hess law

A

principal of addivity of reaction traits that are not able to be experimentally determined

46
Q

formation reaction

A

assemblying a compound from its elements

47
Q

decomposition reaction

A

dissassemblying a compoound into its elements

48
Q

hess law formula

A

sum of products - sum of reactants

49
Q

efficiency

A

actual divided by theoretical
output divided by input

chem 30 (3 decks)

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