RUGG CHEM 100 Chapter 5 Exam

Potential energy (PE)

is energy stored in an object because of its relative position or orientation

Potential energy forms

- Nuclear energy

- Chemical energy

Chemical energy

results from the particular arrangement of atoms in a chemical compound

Nuclear energy

is released when particles in the nucleus of the atom are rearranged

Electrical Energy

results from the flow of electrically charged particles

Kinetic energy (KE)

is energy due to the motion of an object

Kinetic Energy Forms

- Thermal energy

- Radiant Energy

Thermal Energy

results from atomic and molecular motion; the faster the motion, the higher the thermal energy

Radiant Energy

is the energy in light, microwaves, and radio waves

Conservation of Energy

- The total amount of energy in the universe remains constant -Debated*

- "Energy can be neither created nor destroyed, but it can be converted from one form to another"-Einstein

Open System

Can exchange both matter and energy with its surroundings

Closed System

Can exchange energy but not matter with its surroundings

Isolated System

Can exchange neither energy nor matter with its surroundings

Energy

is the capacity to do work

Mechanical work

is energy required to move an object a distance d(meters) when opposed by a force F(newtons)

Work =

Force x Distance

Mass x acceleration x distance =

work

Heat (q)

is thermal energy that can be transformed from an object at one temperature to an object at another temperature

energy change =

heat + work

Joule (J)

The SI unit of energy

- 1J = 1 kg * m^2/s^2

Calorie (cal)

Non-SI unit of energy

- 1 cal = 4.184 J exactly

State (of a system)

A complete description of the system at a given time—its temperature, pressure, the amount of matter it contains, its chemical composition, and the physical state of the matter

State function

A property of a system whose magnitude depends on only the present state of the system, not its previous history

Exothermic

A process in which heat (q) is transferred from a system to its surroundings

q __ 0 for an exothermic reaction

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Endothermic

A process in which heat (q) is transferred to a system from its surroundings

q __ 0 for an endothermic reaction

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Internal energy (E)

The sum of the kinetic and potential energies of all of a system's components

Internal energy is

a state function

Internal energy equation

ΔE = q + w, where q is the heat produced by the system and w is the work performed by the system

Enthalpy (H)

The sum of a system's internal energy E and the product of its pressure P and volume V

Enthalpy equation

H = E + PV

Enthalpy

is the state fun.

Calorimeter

an instrument used to measure the change of heat due to chemical and physical processes

Specific heat (s)

the amount of heat needed to raise 1g of substance

- 1C unit= J/(g *C)

Heat capacity (C)

the amount of heat needed to raise an object

- 1C unit= J/(C)

A barometer is used to

find atmospheric pressure

A Manometer is used to

measure non atmospheric pressures

Heat of Fusion

The amount of heat required to convert a solid into a liquid at its melting point

Heat of Vaporization

The amount of heat required to convert a liquid into a gas at its boiling point

Adiabatic Process

A process in which no heat is exchanged with the surroundings

Standard Enthalpy of Formation

The enthalpy change when one mole of a compound is formed from its elements in their standard states

Hess's Law

The total enthalpy change for a reaction is the same regardless of the number of steps in the reaction or the pathway taken