Physical Chemistry

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59 Terms

1

energy (1)

capacity to do work

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2

work (1)

process of moving against an opposing force

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3

thermodynamics (1)

study of heat, work, and energy changes during processes

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4

open system (1)

exchange matter and energy

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5

closed system (1)

exchange energy only

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6

isolated system (1)

no exchange of matter or energy

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7

standard enthalpy of formation (2)

the enthalpy change when forming 1 mol of substance in its standard state from its elements

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8

standard reaction enthalpy (2)

the enthalpy change when 1 mol of substance reacts under standard conditions

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9

standard enthalpy of combustion (2)

the enthalpy change for the complete combustion of a substance with oxygen, typically hydrocarbons

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10

Hess’ law (2)

the net enthalpy change for a reaction equals the sum of enthalpy changes of individual steps

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11

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.

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12

heat (3)

represents energy due to the random motion of molecules

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13

reversibility (3)

a system can return to its original state with small changes in conditions without any net change in the surroundings.

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14

stoichiometry (5)

study of the numbers of reactants and product molecules

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15

rate of reaction (5)

number of moles of reaction per unit time

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16

order of reaction (5)

the power to which the concentration is raised in the rate law

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17

zero order (5)

rate is independent of concentration

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18

pre-exponential factor (A) (6)

represents how frequently molecules collide in the proper orientation to react

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19

activation energy (Ea) (6)

the minimum energy required for molecular collisions to result in a reaction

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20

arrhenius law (6)

a formula that relates the rate constant of a reaction to the temperature and activation energy.

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21

transition state theory (6)

the maximum energy required corresponds to the formation of an activated complex of the original reactants

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22

catalyst (6)

accelerates reactions without being consumed in the process

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23

half life (7)

time for concentration to decrease to half its initial value

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24

equilibrium (8)

the rate of formation of products equals the rate of decomposition of reactants

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25

dynamic chemical equilibrium (8)

a state where the concentrations of reactants and products remain constant over time as they are continuously formed and decomposed

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26

chemical standard state (8)

typically defined as 1 mol dm^-3 concentrations

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27

biological standard state (8)

maintains 1 mol dm^-3 & ph7 (with [H+] = 10^-7 mol dm^-3) and a temperature of 25°C.

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28

reaction quotient (Q) (8)

provides a measure of the relative amounts of products and reactants at any point

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29

monoprotic acid (10a)

acid containing one proton

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30

diprotic acid (10a)

acid containing two protons

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31

triprotic acid (10a)

acid containing three protons

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32

Ka (10a)

acid dissociation constant, measures the strength of an acid

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33

Kd (10a)

measure propensity (tendency) to dissociate reversibly, reciprocal of Ka. describes binding affinity of a ligand to a protein

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34

acid (10b)

donates protons (H+)

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35

base (10b)

accepts protons

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36

strong acid (10b)

an ** that completely dissociates in solution, releasing all its protons. ionizes fully.

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37

buffer (10b)

solution that maintain a constant pH when diluted or when acid/base

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38

latent heat for melting (q) (11)

heat required to convert 1 mol of solid to liquid at melting point

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39

latent heat for boiling (q) (11)

heat required to convert 1 mol of liquid to gas at boiling point

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40

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

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41

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

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42

oxidation (12)

loss of electrons

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43

reduction (12)

gain of electrons

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44

redox reaction (12)

involves loss of electrons from one species and gain by another

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45

reducing agent (12)

acts as an electron donor and is itself oxidized

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46

oxidizing agent (12)

acts as an electron acceptor and is itself reduced

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47

electrochemistry (12)

study of chemical processes that cause electrons to move

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48

voltaic (galvanic) cell (12)

generates current spontaneously

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49

electrolytic cell (12)

requires external voltage to drive a reaction

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50

metal electrode (13)

composed of metal in contact with an ionic solution

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51

redox electrode (13)

involves an inert metal in contact with a solution containing a species in two oxidation states

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52

gas electrode (13)

consists of a gas in equilibrium with its ionic solution in the presence of an inert metal

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53

insoluble salt electrode (13)

involves a metal (M) coated with an insoluble salt (MX) immersed in a solution containing X- ions

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54

vertical bar I (13)

denotes a barrier (eg. Ag l AgCl )

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55

double vertical bars ll (13)

represents connection, such as a salt bridge

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56

anode (13)

left hand half cell

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57

cathode (13)

right hand half cell

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58

cell potential (E) (13)

the difference between the electrode potentials of the cathode and anode

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59

zero current potential (13)

the maximum amount of non-expansion work (Wmax= deltaG)

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