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Chemistry 1100 > Chapter 6 Definitions > Flashcards

Chapter 6 Definitions Flashcards

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1
Q

Thermodynamics

A

The general study of energy and its conversions

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2
Q

Kinetic Energy

A

Energy associated with motion

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3
Q

Thermal Energy

A

Energy associated with temperature

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4
Q

Energy

A

The ability to do work

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5
Q

Work

A

Force acting through a distance

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6
Q

Heat

A

The flow of energy caused by temperature difference

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7
Q

Potential Energy

A

Energy associated with positions or composition

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8
Q

Chemical Energy

A

A form of potential energy associated with positions of electrons and nuclei in a system

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9
Q

Thermochemistry

A

The study of heat energy associated with chemical reactions and physical transformations

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10
Q

What is the Law of Conservation of Energy

A

Energy can neither be created nor destroyed, but it can be transferred from one object or system to another.

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11
Q

System

A

A specific area of interest

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12
Q

Surroundings

A

Everything else (i.e. the universe)

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13
Q

First Law of Thermodynamics

A

The total energy of the universe is constant

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14
Q

Internal energy (U)

A

The sum of the kinetic energy and potential energies of all of the particles in a system

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15
Q

The state of the system is defined by parameters like:

A

Temperature, Pressure, Concentration, and Physical State

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16
Q

Summarize Energy Flow for reactants with higher internal energy

A

If reactants have higher internal energy than the products, the ‘triangle’Usys is negative and energy flows out of the system into the surroundings. The surroundings is negative and energy is decreasing.

17
Q

Summarize Energy Flow for reactants with lower internal energy

A

If reactants have lower internal energy than the products, the ‘triangle’Usys is positive and energy flows into the system from the surroundings. The surroundings is positive and energy is increasing.

18
Q

Heat Capacity (C) of a system

A

The quantity of heat required to change its temperature by 1degreesC or 1K. Depends on mass

19
Q

Two types of calorimeters (Heat of reactions are measured in calorimeters)

A

Bomb Calorimeters: Constant Volume
Coffee Cup Calorimeters: Constant Pressure

20
Q

Two types of Heat Capacity

A

Specific Heat Capacity: Heat Capacity per gram of a material (does not depend on mass)
Molar Heat Capacity: Heat Capacity per mole of a material (depends on mass)

21
Q

Pressure-Volume Work

A

The force is caused by a volume change against an external pressure

22
Q

Heat is proportional/disproportional to temperature

A

Proportional

23
Q

List the state function.

A

Internal Energy (U), Pressure(P), Volume(V), and H(enthalpy). Its’ value depends only on the state of the system

24
Q

Heat and work are not path functions. True/False

A

False. Path functions depend on the path taken to reach one state from another

25
Q

Closed System

A

Pressure changes, and volume remains constant

26
Q

Open System

A

Volume remains constant, and pressure changes

27
Q

Enthalpy

A

The heat evolved in a chemical reaction at constant pressure

28
Q

If enthalpy is greater than 0. What is the reaction?

A

The reaction is endothermic

29
Q

If enthalpy is less than 0. What is the reaction?

A

The reaction is exothermic (it releases energy)

30
Q

Exothermic Reactions

A

Negative Enthalpy - Gives off heat heat from the surroundings

Weaker bonds break and stronger
bonds form
* Electrons reorganize
* Molecules reorganize
* Potential energy converts to thermal
energy
* Reaction gives off thermal energy
* System is more stable, lower in
potential energy

31
Q

Endothermic

A

Positive Enthalpy - Absorbs heat from the surroundings

Weaker bonds forms and stronger bonds break
* Electrons do not reorganize
* Molecules do not reorganize
* Potential energy converts to thermal
energy ???
* Reaction do not give off thermal energy
* System is unstable, higher in
potential energy

32
Q

Hess’s Law

A

The enthalpy changes of the reaction carried out in multiple steps is equal to the sum of the enthalpy changes for each individual step.

Chemistry 1100 (3 decks)

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