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 Visual Chemistry Encyclopedia 6 files - 711 sheets
One picture says more than a thousand words
 
File 4. Thermodynamics, Acids and Bases
 
6x Kinetics
5x Reaction rate measurement
7x Reaction rate diagrams
5x Influence of temperature
8x Heat
8x Enthalpy and entropy
7x Enthalpy diagrams
6x Enthalpy calculations
8x Equilibria
7x Influence of pressure and temperature
8x Acids and bases: indicators
9x Strong acids and bases
8x Strong vs. weak acids and bases
7x Titrations
7x Titration and indicators
5x Titration equipment

4.33
 Kinetics
4.33.1
 The relationships among K, ETH G°and E°cell (fig. 19.7 Eb)
4.33.2
 A representation of two types of free energy profiles (Zu 173)
4.33.3
 The dependence of free energy on partial pressure (Zu 174)
4.33.4
 Free energy and equilibrium (Zu 175)
4.33.5
 Interplay of ETH Ssys and ETH Ssurr in determining the sign of ETH Suniv (Zu 171)
4.33.6
 Various possible combinations of ETH H and ETH S for a process and the resulting dependence of spontaneity on temperature (Zu 172)
   
4.34 Reaction rate measurement
4.34.1 Collection of gas over water (fig. 5.17 Eb)
4.34.2 2NO2(g)_N2O4(g) (Zu 147)
4.34.3 Calculation of the average rate (fig. 13.5 Eb)
4.34.4 Following the concentration of N2O5 during decomposition (fig. 13.6 Eb)
4.34.5 A graph illustrating the half-life of a first-order reaction (fig. 13.8 Eb)
   
4.35 Reaction rate diagrams
4.35.1 Representation of the reaction 2NO2(g) 2 NO(g) + O2(g) (Zu 140)
4.35.2 The definition of rate (Zu 139)
4.35.3 Rate varies with concentration for N2O5 (Zu 141)
4.35.4 Constant half-life first-order process (Zu 142)
4.35.5 (a) A plot of In[C4H6] versus t. (b) A plot of 1/[C4H6] versus t. (Zu 143)
4.35.6 Plotting the data for the decomposition of nitrogen
dioxide part 1 (fig. 13.10 Eb)
4.35.7 Plotting the data for the decomposition of nitrogen
dioxide part 2 (fig. 13.10 Eb)
   
4.36 Influence of temperature
4.36.1 Representation of the mechanism of decomposition of N2O5 (fig. 13.16 Eb)
4.36.2 Plot of log [N2O5] versus time (fig. 13.9 Eb)
4.36.3 Collision variation with temperature (Zu 144)
4.36.4 Catalyzed and uncatalyzed reaction profiles (Zu 145)
4.36.5 Collision energy distribution versus activation energy for
catalyzed and uncatalyzed reactions (Zu 146)
   
4.37 Heat
4.37.1 Coffee-cup calorimeter (Zu 48)
4.37.2 Illustration of a thermodynamic system (fig. 6.4 Eb)
4.37.3 Bomb calorimeter (Zu 49)
4.37.4 A simple coffee-cup calorimeter (fig. 6.11 Eb)
4.37.5 A bomb calorimeter (fig. 6.12 Eb)
4.37.6 A kinetic-theory explanation of heat (fig. 6.5 Eb)
4.37.7 Pressure-volume work (fig. 6.9 Eb)
4.37.8 PV work (Zu 47)
   
4.38 Enthalpy and entropy
4.38.1 Reaction of Zn with HCl (illustrating expansion work) (fig. 18.3 Eb)
4.38.2 Standard entropy of methyl chloride at various temperatures (fig. 18.8 Eb)
4.38.3 Arrangements of balls in two containers (fig. 18.7 Eb)
4.38.4 Standard entropies - at 25°C part 1 (table 18.1 Eb)
4.38.5 Standard entropies - at 25°C part 2 (table 18.1 Eb)
4.38.6 Standard free energies of formation - at 25°C part 1 (table 18.2 Eb)
4.38.7 Standard free energies of formation - at 25°C part 2 (table 18.2 Eb)
4.38.8 Vapour pressure of water at various temperatures
(table 5.6 Eb)
   
4.39 Enthalpy diagrams
4.39.1 An analogy to illustrate a state function (fig. 6.7 Eb)
4.39.2 An enthalpy diagram (fig. 6.8 Eb)
4.39.3 Enthalpy diagram illustrating Hess’s law (fig. 6.13 Eb)
4.39.4 Energy of formation of MgO(s) versus NaF(s) (Zu 81)
4.39.5 Energetics of ionic bonding (fig. 9.2 Eb)
4.39.6 Standard enthalpies of formation - at 25°C part 1 (table 6.2 Eb)
4.39.7 Standard enthalpies of formation - at 25°C part 2 (table 6.2 Eb)
   
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4.40 Enthalpy calculations
4.40.1 The domains of kinetics and thermodynamics (Zu 169)
4.40.2 Pathway for combustion of ammonia (Zu 52)
4.40.3 Pathway for combustion of methane (Zu 50)
4.40.4 Born-Haber cycle for NaCl (fig. 9.3 Eb)
4.40.5 Molecular orientation in the reaction of NO and Cl2 (fig. 13.12 Eb)
4.40.6 Keep in mind the following concepts (Zu 51)
   
4.41 Equilibriums
4.41.1 Effect on chemical equilibrium of changing temperature (fig. 14.10 Eb)
4.41.2 Effect on chemical equilibrium of changing the pressure (fig. 14.9 Eb)
4.41.3 H2O and CO begin to react and reach equilibrium (Zu 148)
4.41.4 Activation energies in the decomposition of ozone (fig. 13.17 Eb)
4.41.5 Catalytic methanation reaction approaches equilibrium (fig. 14.2A Eb)
4.41.6 Catalytic methanation reaction approaches equilibrium (fig. 14.2B Eb)
4.41.7 Solubility product constants, Ksp, at 25°C part 1 (table 17.1 Eb)
4.41.8 Solubility product constants, Ksp, at 25°C part 2 (table 17.1 Eb)
   
   
   
4.42 Influence of pressure and temperature
4.42.1 The effect of decreased volume on the ammonia synthesis equilibrium (Zu 152)
4.42.2 The ammonia synthesis equilibrium (Zu 149)
4.42.3 CaCO3(s)_CaO(s) + CO2(g) (Zu 150)
4.42.4 Solubility equilibrium (fig. 12.2 Eb)
4.42.5 The steps in the dissolving process (Zu 134)
4.42.6 The temperature dependence of solubility for various solids (Zu 135)
4.42.7 Procedures for solving equilibrium problems (Zu 151)
   
 

4.43 Acids and bases: indicators
4.43.1 Colour changes of some acid-base indicators (fig. 15.8 Eb)
4.43.2 Red cabbage juice as an acid-base indicator (fig. 4.8right Eb)
4.43.3 The pH ranges of various common indicators (Zu 167)
4.43.4 Choosing an indicator for the titration of a strong acid and a weak acid (Zu 168)
4.43.5 The pH scale (fig. 15.6 Eb)
4.43.6 The acid and base forms of phenolphthalein (Zu 166)
4.43.7 The pH values of some common substances (Zu 157)
4.43.8 Relative strengths of acids and bases (table 15.2 Eb)
   
4.44 Strong acids and bases
4.44.1 HCl (aq) is completely ionized (Zu 26)
4.44.2 Reaction of nitric acid with water - model representation (fig. 4.9 Eb)
4.44.3 The hydronium ion, H3O+ (fig. 15.2 Eb)
4.44.4 An aqueous solution of sodium hydroxide (Zu 27)
4.44.5 Acid strength versus conjugated base strength (Zu 154)
4.44.6 Structures of the chlorine oxoacids (fig. 22.41 Eb)
4.44.7 The effect of the number of attached oxygens on the O-H bond in a series of chlorine oxyacids (Zu 159)
4.44.8 The oxychloro anions (Zu 198)
4.44.9 Flow chart of naming acids (Zu 17)
   
4.45 Strong vs. weak acids and bases
4.45.1 The pH curve for the titration of NH3 (Zu 165)
4.45.2 The titration curve for a weak acid (Zu 162)
4.45.3 A strong acid (a) and a weak acid (b) in water (Zu 156)
4.45.4 Acetic acid in water (Zu 28)
4.45.5 Graphical representations of strong and weak acid equilibria (Zu 153)
4.45.6 Reaction of hydronium ion with ammonia (fig. 15.3 Eb)
4.45.7 The effect of dilution on the percent dissociation and [H+] of a weak acid solution (Zu 158)
4.45.8 The structure of phosphoric acid (Zu 195)
 
 
4.46 Titrations
4.46.1 A glass electrode (fig. 19.8right Eb)
4.46.2 Titration of HCl with NaOH (fig. 4.19 center Eb)
4.46.3 Comparison of strong and weak acid titration curves (Zu 163)
4.46.4 The shape of the titration curve as a function of Ka (Zu 164)
4.46.5 The pH curves for the titration of a strong acid and a strong base (Zu 161)
4.46.6 Values of Ka for some common monoprotic acids (Zu 155)
4.46.7 Solving acid-based problems (Zu 160)
   
4.47 Titration and indicators
4.47.1 Titration of a strong acid by a strong base (fig. 16.11 Eb)
4.47.2 Effect of added acid or base on a buffer solution (fig. 16.10 Eb)
4.47.3 Titration of a weak base by a strong acid (fig. 16.13 Eb)
4.47.4 Titration of a weak acid by a strong base (fig. 16.12 Eb)
4.47.5 Base-ionization constants at 25°C (table 16.2 Eb)
4.47.6 Acid-ionization constants at 25°C (table 16.1 Eb)
4.47.7 Common strong acids and bases (table 4.3 Eb)
   
4.48 Titration equipment
4.48.1 A glass electrode for measuring pH (Zu 181)
4.48.2 Equipment measuring liquid volume (Zu 3)
4.48.3 Measuring liquid volume with a buret (Zu 4)
4.48.4 The difference between precision and accuracy (Zu 5)
4.48.5 Preparation of a standard solution (Zu 29)
4.48.6 Dilution procedures (Zu 30)
4.48.7 Stoichiometry steps for reactions in solution (Zu 31)
 
 
 
 
 
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