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Perryland Chemistry Honors > Honors - Unit 9 - Thermochemistry > Flashcards

Honors - Unit 9 - Thermochemistry Flashcards

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1
Q

Thermochemistry

A

The study of energy changes during a chemical reaction or change of state (solid, liquid, gas).

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2
Q

Chemical Potential Energy

A

The energy stored in chemical bonds. (Lines with no Slope on the Heating Curve)

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3
Q

Heat

A

Energy that transfers from one object to another due to a difference in temperature between them. Heat always flows from the warmer to the cooler object.

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4
Q

Calorimeter

A

The device used to measure the quantity of heat flow in a reaction.

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5
Q

Calorimetry Steps

A
  1. Use a well known substance (water) 2. Run the reaction and let heat go into or out of the water 3.Measure the waters change in temperature
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6
Q

The heat lost in a reaction (Q lost) = ?

A

Q lost = Q gained

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7
Q

Melting

A

Make or become liquefied by heat. (Solid to Liquid)

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8
Q

Freezing

A

Freezing or solidification is a phase transition in which a liquid turns into a solid when its temperature is lowered below its freezing point. (Liquid to Solid)

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9
Q

Condensation (Precipitation)

A

The conversion of a vapor or gas to a liquid.

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10
Q

Vaporization (Evaporation)

A

The conversion of a liquid into a gas.

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11
Q

Heat of Fusion

A

The energy required to change a gram of a substance from the solid to the liquid state without changing its temperature.

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12
Q

Solidification

A

Freezing or solidification is a phase transition in which a liquid turns into a solid when its temperature is lowered below its freezing point. (Liquid to Solid)

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13
Q

Heat

A

A form of energy that flows between two samples of matter because of their differences in temperature.

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14
Q

Temperature

A

A measure of the intensity of heat, i.e. the hotness or coldness of a sample. or object.

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15
Q

Kinetic Energy

A

In Thermochemistry, the energy an object possesses due to its change in temperature is called kinetic energy. (Sloped lines on the Heating Curve)

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16
Q

Potential Energy

A

Potential energy is that energy which an object has because of its position. It is called potential energy because it has the potential to be converted into other forms of energy, such as kinetic energy. (Lines with no Slope on the Heating Curve

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17
Q

Endothermic

A

Reaction in which the system absorbs energy from its surroundings in the form of heat.

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18
Q

Exothermic

A

An exothermic reaction is a chemical reaction that releases energy in the form of light or heat.

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19
Q

Collision Theory

A

Molecules have to collide in a certain way with a certain amount of activation energy in order to form a new product.

20
Q

Activation Energy

A

The minimum energy required to start a chemical reaction

21
Q

How to speed up the Rate of a Reaction

A
  1. Shrink the container or increase concentration. 2. Increase the number of particles. 3. Speed up the particles by adding heat. 4. Break up clumps into individual particles. 5. Use a catalyst.
22
Q

Catalyst

A

A substance that causes a chemical reaction to happen more quickly.

23
Q

Heating Curve

A

A plot of the temperature versus time.

24
Q

What do the symbols in the following equation represent:

Q=mC(Delta T)

A
25
Q

Solid

A

Solid is one of the four fundamental states of matter. It is characterized by structural rigidity and resistance to changes of shape or volume.

26
Q

Liquid

A

Liquid is one of the four fundamental states of matter, and is the only state with a definite volume but no fixed shape. A liquid is made up of tiny vibrating particles of matter, such as atoms, held together by intermolecular bonds.

27
Q

Gas

A

One of four main states of matter, composed of molecules in constant random motion. Unlike a solid, a gas has no fixed shape and will take on the shape of the space available. Unlike a liquid, the intermolecular forces are very small; it has no fixed volume and will expand to fill the space available.

28
Q

Boiling

A

Boiling is the rapid vaporization of a liquid, which occurs when a liquid is heated to its boiling point.

29
Q

Boiling Point

A

The temperature at which the vapor pressure of the liquid is equal to the pressure exerted on the liquid by the surrounding environmental pressure. At the boiling point the gas and liquid phase exist in equilibrium.

30
Q

Melting Point

A

The melting point of a solid is the temperature at which it changes state from solid to liquid at atmospheric pressure. At the melting point the solid and liquid phase exist in equilibrium.

31
Q

Phase Changes

A
32
Q

Law of Conservation of Energy

A

Energy can not be created nor destroyed during a chemical reaction

33
Q

Heat Capacity

A

Heat capacity is the amount of heat energy required to change the temperature of a substance

34
Q

Specific Heat

A

the amount of energy in the form of heat, calories or joules, required to raise the temperature of 1 gram of a substance 1°C

35
Q

Evaporation versus Boiling

A
36
Q

thermochemical equation

A

thermochemical equation

  • balanced chemical equations with heat changes taken into account
  • think of it as (and treat it as) a reactant or a product
37
Q

Enthalpy (H)

A

-the heat content of a system (or chemical reaction)

38
Q

CaO (s) + H₂O (l) → Ca(OH)₂(s) + 65.2 kJ
Change in H = - 65.2 kJ
Endo or Exo?

A

Exo
heat is a product and change in H is negative

39
Q

2 NaHCO₃ (s) + 129 kJ → Na₂O (s) + H₂O (g) + CO₂(g)
Change in H = +129 kJ
Endo or Exo ? How to tell?

A

Endo
heat is a reactant and change in H is positive

40
Q

Endo or Exothermic?

A

Exothermic reaction graph

41
Q

five ways to tell if a reaction is exothermic

A

graph slopes down
heat is given off (to the surroundings)
change in H is negative
temperature of “surroundings” increases
heat is written as a product

42
Q

five ways tell if a reaction is endothermic

A

graph slopes up
heat is absorbed (from the surroundings)
change in H is positive
temperature of “surroundings” decreases
heat is written as a reactant

43
Q

Phase Diagram most substances (e.g. CO2)

A

slight positive slope; more dens in (l) phase;
triple point: s, l, g in equilib.
critical point: T and P above which there is no distinction between l and g

44
Q

Phase Diagram H2O

A

negative slope bc H2O has lower density in (s) than (l); increase in P favors more dense version.

45
Q

Which phase changes are endothermic? Which are Exothermic? Is bond breaking Endothermic or Exothermic?

A
46
Q

Phase Diagram Questions

A
47
Q

Heating Curve Questions

A

Perryland Chemistry Honors (12 decks)

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