Chapter 11: Thermodynamics

System

part of universe what you are studying

surroundings

anything and everything not under study

open system

transfer energy and matter to surroundings

closed system

transfer only energy to surroundings

isolated system

transfers nothing to surroundings

state functions

describes an aspect of a chemical system (such as pressure, volume)

extensive properties

the matter changes as the initial sample change

standard state

1 atm, 25 celsius, 1 mol of compound present

exothermic

energy lost to surroundings

ΔH sign for exothermic

negative

endothermic

energy gained from surroundings

ΔH symbol for endothermic

positive

law of conservation of energy

energy cannot be created or destroyed

kinetic energy

energy in motion

potential energy

stored and released under certain conditions

specific heat

amount of energy needed to cause 1 g of substance to increase in 1 degree celsius (or kelvin)

first law of thermodynamics

energy is always conserved

work

force applied to an object as it moved a certain distance

enthalpy

H

formation reactions

only one mole of products and reactants in standard states

entropy

S

Gibbs Free Energy

G