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energy (1)
capacity to do work
work (1)
process of moving against an opposing force
thermodynamics (1)
study of heat, work, and energy changes during processes
open system (1)
exchange matter and energy
closed system (1)
exchange energy only
isolated system (1)
no exchange of matter or energy
standard enthalpy of formation (2)
the enthalpy change when forming 1 mol of substance in its standard state from its elements
standard reaction enthalpy (2)
the enthalpy change when 1 mol of substance reacts under standard conditions
standard enthalpy of combustion (2)
the enthalpy change for the complete combustion of a substance with oxygen, typically hydrocarbons
Hess’ law (2)
the net enthalpy change for a reaction equals the sum of enthalpy changes of individual steps
entropy (3)
a fundamental concept in thermodynamics relating to a disorder, often symbolized as S and associated with the number of microstates (disorder) corresponding to a thermodynamic system.
heat (3)
represents energy due to the random motion of molecules
reversibility (3)
a system can return to its original state with small changes in conditions without any net change in the surroundings.
stoichiometry (5)
study of the numbers of reactants and product molecules
rate of reaction (5)
number of moles of reaction per unit time
order of reaction (5)
the power to which the concentration is raised in the rate law
zero order (5)
rate is independent of concentration
pre-exponential factor (A) (6)
represents how frequently molecules collide in the proper orientation to react
activation energy (Ea) (6)
the minimum energy required for molecular collisions to result in a reaction
arrhenius law (6)
a formula that relates the rate constant of a reaction to the temperature and activation energy.
transition state theory (6)
the maximum energy required corresponds to the formation of an activated complex of the original reactants
catalyst (6)
accelerates reactions without being consumed in the process
half life (7)
time for concentration to decrease to half its initial value
equilibrium (8)
the rate of formation of products equals the rate of decomposition of reactants
dynamic chemical equilibrium (8)
a state where the concentrations of reactants and products remain constant over time as they are continuously formed and decomposed
chemical standard state (8)
typically defined as 1 mol dm^-3 concentrations
biological standard state (8)
maintains 1 mol dm^-3 & ph7 (with [H+] = 10^-7 mol dm^-3) and a temperature of 25°C.
reaction quotient (Q) (8)
provides a measure of the relative amounts of products and reactants at any point
monoprotic acid (10a)
acid containing one proton
diprotic acid (10a)
acid containing two protons
triprotic acid (10a)
acid containing three protons
Ka (10a)
acid dissociation constant, measures the strength of an acid
Kd (10a)
measure propensity (tendency) to dissociate reversibly, reciprocal of Ka. describes binding affinity of a ligand to a protein
acid (10b)
donates protons (H+)
base (10b)
accepts protons
strong acid (10b)
an ** that completely dissociates in solution, releasing all its protons. ionizes fully.
buffer (10b)
solution that maintain a constant pH when diluted or when acid/base
latent heat for melting (q) (11)
heat required to convert 1 mol of solid to liquid at melting point
latent heat for boiling (q) (11)
heat required to convert 1 mol of liquid to gas at boiling point
enthalpy of fusion (11)
energy required to convert 1 mol of solid (ice) to liquid at the melting point (0 C) = 6.01 kj mol-1enth
enthalpy of vaporization (11)
energy required to convert 1 mol of liquid (water) to gas (steam) at boiling point (100 C) = 40.7 kj mol-1
oxidation (12)
loss of electrons
reduction (12)
gain of electrons
redox reaction (12)
involves loss of electrons from one species and gain by another
reducing agent (12)
acts as an electron donor and is itself oxidized
oxidizing agent (12)
acts as an electron acceptor and is itself reduced
electrochemistry (12)
study of chemical processes that cause electrons to move
voltaic (galvanic) cell (12)
generates current spontaneously
electrolytic cell (12)
requires external voltage to drive a reaction
metal electrode (13)
composed of metal in contact with an ionic solution
redox electrode (13)
involves an inert metal in contact with a solution containing a species in two oxidation states
gas electrode (13)
consists of a gas in equilibrium with its ionic solution in the presence of an inert metal
insoluble salt electrode (13)
involves a metal (M) coated with an insoluble salt (MX) immersed in a solution containing X- ions
vertical bar I (13)
denotes a barrier (eg. Ag l AgCl )
double vertical bars ll (13)
represents connection, such as a salt bridge
anode (13)
left hand half cell
cathode (13)
right hand half cell
cell potential (E) (13)
the difference between the electrode potentials of the cathode and anode
zero current potential (13)
the maximum amount of non-expansion work (Wmax= deltaG)