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High School > Chem 30 Unit 1 > Flashcards

Chem 30 Unit 1 Flashcards

1
Q

the original source of energy on earth is….

A

the sun

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2
Q

chemical energy

A

energy released when substances undergo a chemical reaction (e.g. combusion) to transform into other substances (e.g. burning of fossil fuels)

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3
Q

Nuclear energy

A

form of energy released from the nucleus of atoms.

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4
Q

nuclear fission

A

the splitting of an atomic nucleus into two smaller nuclei (releasing nuclear energy)

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5
Q

nuclear fusion

A

combining two atomic nuclei to produce one larger nucleus (releasing nuclear energy)

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6
Q

solar energy

A

energy from teh sun

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7
Q

geothermal energy

A

heat energy from the earth (e.g. geysers, hotsprings)

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8
Q

Laws of Thermodynamics

A
  1. Law of Conversation of Energy
  2. Law of Heat Exchange or Transfer
  3. Total heat lost = total heat gained
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9
Q

Law of Conversation of Energy

A

Energy cannot be created or destroyed; can be converted
from one form to another.

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10
Q

Law of Heat Exchange or Transfer

A

Heat flows from hot to cold until thermal equilibrium

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11
Q

Total heat lost = total heat gained

A

energy lost by the hot object is equal to the energy gained by the cold object.

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12
Q

Exothermic

A

energy produced, given off by the reactants. Releases heat to the surroundings. Has a negative ΔH.

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13
Q

Endothermic

A

energy is required, reaction needs energy to occur. Absorbs energy from the surroundings. Has a positive ΔH.

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14
Q

cellular respiration is…

A

exothermic

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15
Q

photosynthesis is…

A

endothermic

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16
Q

Kinetic molecular theory

A

the smallest particles of any substance are in continuous motion

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17
Q

translational motion

A

straight line motion (gases)

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18
Q

rotational motion

A

spinning or turning (liquids)

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19
Q

vibrational motion

A

oscillation (back/forth) motion (solids)

20
Q

temperature is …

A

the average kinetic energy of the particles of the substance.

21
Q

Change in temperature =

A

change in average kinetic energy

22
Q

specific heat capacity

A

the quantity of heat required to raise/lower the temp of a substance per unit mass per degree celsius.

23
Q

calorimetry

A

a substance is burned in pure oxygen in a reaction chamber. heat released flows into surrounding water, changing its temperature. use data collected to calculate heat given off.

24
Q

Enthalpy (ΔH):

A

measure of the energy content of a system

25
Q

open system

A

allows both energy and matter to flow in and out of the system

26
Q

closed system

A

only allows the transfer of energy in and out (does not allow transfer of matter)

27
Q

enthalpy of a system is

A

the total kinetic energy and potential energy of a system under constant pressure

28
Q

kinetic energy

A

energy of an object due to motion (change in temp)

29
Q

potential energy

A

energy of an object due to position (chemical change)

30
Q

molar enthalpy

A

= molar heat of combustion

31
Q

molar enthalpy/molar heat is…

A

positive/negative depending on if water was heated/cooled

32
Q

positive enthalpy change means….

A

endothermic reaction

33
Q

negative enthalpy change means….

A

exothermic reaction

34
Q

for calorimetry questions that include both the water and calorimeter…

A

chemical energy = calorimeter (water + calorimeter)

35
Q

molar enthalpies for decomposition

A

switch sign of data book value

36
Q

potential energy diagrams…

A

shows the change in potential energy during a chemical reaction.

37
Q

in an exothermic potential energy diagram…

A

there is a step down (reactants have more Ep than products)

38
Q

in an endothermic potential energy diagram…

A

there is a step up (reactants have less Ep than products)

39
Q

Axis for a potential energy diagram:

A

x axis: progress of reaction
y axis: potential energy (Ep)

40
Q

difference between the Ep of reactants and products =

A

ΔH (change in enthalpy)

41
Q

catalyst

A

makes the reaction happen faster, but does not hange the reaction. Does not
change the ΔH.

42
Q

Activation energy

A

energy needed to get the reaction started (do not include when calculating ΔH in a Ep diagram).

43
Q

Hess’s Law

A

the enthalpy of reaction is the same regardless of whether a reaction occurs in one step or in several steps.

44
Q

ΔH =

A

products - reactants

45
Q

ΔH of elements =

A

0 kJ

High School (18 decks)

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