4Liquids and solutions - TEP-TEPE, Faculty of … hydrogen electrode Figure 3 Half standard hydrogen...
Transcript of 4Liquids and solutions - TEP-TEPE, Faculty of … hydrogen electrode Figure 3 Half standard hydrogen...
![Page 1: 4Liquids and solutions - TEP-TEPE, Faculty of … hydrogen electrode Figure 3 Half standard hydrogen cell ... =159 kJ, (C-F) =489 kJ, (H-F) =567 kJ . SC123 Fundamental Chemistry Asst.](https://reader031.fdocuments.net/reader031/viewer/2022030418/5aa430e37f8b9ac8748b976d/html5/thumbnails/1.jpg)
SC 123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 1
Solution
Figure 10 Solutions.
Solubility
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Figure 11 Hexane, water, and CCl4
Temperature and solubility of solid
Figure 12 Temperature and solubility of solid
Temperature and solubility of gas
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SC 123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 3
Figure 13 Temperature and solubility of gas
Pressure and solubility of gas
Figure 14 Pressure and solubility of gas
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Figure 15 kH of gases
Energy of solution
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Figure 16 Energy of solution
Solution of ionic compounds
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SC 123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 6
Table 1 Enthalpy of hydration of ions
Enthalpy of Hydration (KJ/mol)
Cations Anions
H+ -1130 F- -483
Li+ -580 Cl- -340
Na+ -444 Br- -309
Mg2+ -2003
Ca2+ -1557
Al3+ -2537
Practice
1. Calculate the energy of solution of MgCl2 with a lattice energy of 3250 kJ/mol
Types of solution
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SC 123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 7
Units of solubility (concentration)
Practice
1. Calculate the concentrations of methanol (CH3OH) 50 g in water 1000 g in mass
fraction, mole fraction, molal, molar, and ppm
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Colligative properties
1. Depression of vapor pressure
Figure 17 Depression of vapor pressure of solution
2. Boiling-point elevation
3. Freezing-point depression
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SC 123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 9
Figure 18 Kb and Kf of some liquids
Figure 19 Red blood cells in normal solution (left), salt solution (middle), and pure water
(right)
4. Osmotic pressure
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SC 123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 10
Figure 20 ความดันออสโมติก
Practice
1. Calculate the boiling point, freezing point, and osmotic pressure of a solution of
methanol (CH3OH) 50 g in water 1000 g
Colloid
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SC 123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 11
Practice
1. Calculate the concentrations of glucose (molecular weight =180 g/mol) 90 g in water
1000 g in mass fraction, mole fraction, molal, molar, and ppt
2. Calculate the volume of 0.1 M HCl in human stomach to digest magnesium
hydroxide 500 mg. Molecular weight of magnesium hydroxide is 58.3 g/mol.
3. Calculate the freezing point, boiling point, and osmotic pressure of a solution of
ethylene glycol 478 g in water 3202 g. Molecular weight of ethylene glycol is 62.01 g
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4. For a 5.86 M ethanol solution (C2H5OH) with a density of 0.927 g/mL, calculate the
concentration of this solution in molal.
5. A unknown solution with 18 g of unknown and 150 g of water has a boiling point of
100.34 ˚C. Calculate the molecular weight of the unknown.
6. A solution of protein 1.00x10-3 g and water 1.00 mL has an osmotic pressure of 1.12
torr at temperature of 25.0 ˚C. Calculate the molecular weight of this protein
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SC123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 1
Electrochemistry
Electrochemical reactions
Figure 1 Redox reaction between Zn and Cu2+
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SC123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 2
Oxidation number
Balance redox equations
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SC123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 3
Practice
1. Balance redox reactions
a. H2O2 + Fe2+ Fe3+ + H2O (in acidic solution)
b. CN- + MnO4- CNO- + MnO2 (in basic solution)
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Electrochemical cell
Table 1 Comparison between galvanic cell and electrolyte cell
Galvanic cell Electrolyte cell
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Figure 2 Comparison between galvanic cell and electrolyte cell
Cell diagram
Standard hydrogen electrode
Figure 3 Half standard hydrogen cell
Standard half cell potential, E0
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SC123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 6
Figure 4 Measurement of standard half cell potential
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Figure 5 Reduction potential
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SC123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 8
Cell potential, Ecell
Practice
1. Calculate cell potential of
a. Zn and Cu2+
b. MnO2 and Cu
c. Fe2+ and Cl-
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SC123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 9
Nernst equation
Thermodynamics and electrochemistry
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SC123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 10
Figure 6 Relationship between ΔG0 and E0cell
Practice
1. Calculate the equilibrium constant of 2H2O(l) 2H2(g) + O2(g) with Gibbs
free energy = -237.2 kJ/mol
2. Determine whether or not the following reaction is spontaneous at 298 K
Co(s) + Fe2+(aq) Co2+(aq) + Fe(s) when [Co2+]=0.15 M and [Fe2+] =0.68 M
Faraday law
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SC123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 11
Practice
1. Calculate the amount of zinc generated at cathode for current of 2.0 A passing
through ZnSO4 solution for 20 minutes.
Examples of electrochemical cells in daily life
1. Battery
Figure 7 Batteries
2. Rust protection
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SC123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 12
Figure 8 Rust protection of metal pipeline
3. Metal coating
Figure 9 Metal coating
Practice
1. Balance the redox equations
a. CH3CH2OH + Cr2O72- CH3COOH + Cr3+ (in basic solution)
b. Mg + O2 Mg2+ + H2O (in acidic solution)
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SC123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 13
2. Calculate E0 for the reaction between mercury and (a) 1 M HCl and (b) 1 M HNO3.
Which acid oxidize Hg to Hg22+ under standard condition
3. Calculate equilibrium constant of Sn(s) + 2Cu2+(aq) Sn2+(aq) + 2Cu+(aq)
4. Calculate the change of Gibbs free energy of
2Au(s) + 3Ca2+(aq, 1 M) 2Au3+(aq, 1 M) + 3Ca(s)
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5. A galvanic cell with cell potential of 0.54 V at 25 ˚C ถ้า [Zn2+]=1.0 M and PH2 = 1.0
atm. Calculate the concentration of H+
6. Is this reaction spontaneous at 25 0C when [Fe2+] = 0.60 M and [Cd2+] = 0.010 M?
Fe2+ (aq) + Cd (s) Fe (s) + Cd2+ (aq)
7. Calculate equilibrium constant at 25 0C
Fe2+ (aq) + 2Ag (s) Fe (s) + 2Ag+ (aq)
8. For an electrochemical reaction of Na2SO4, there is oxygen gas and hydrogen gas
generated at anode and cathode, respectively. Write the corresponding redox
equations.
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SC123 Fundamental Chemistry Asst. Prof. Peerasak Paoprasert 15
9. What is the cell potential of an electrochemical cell with Cd electrode and 1.0 M
Cd(NO3)2 solution and Cr electrode and 1.0 M Cr(NO3)3?
Cd2+ (aq) + 2e- Cd (s) E0 = -0.40 V
Cr3+ (aq) + 3e- Cr (s) E0 = -0.74 V
10. Calculate the current required to make 3 g of gold from AuCl3 solution in 20 minutes.
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SC123 Fundamental Chemistry Asst. Prof. Dr. Peerasak Paoprasert 1
Chemical thermodynamics
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SC123 Fundamental Chemistry Asst. Prof. Dr. Peerasak Paoprasert 2
Heat, q
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SC123 Fundamental Chemistry Asst. Prof. Dr. Peerasak Paoprasert 3
Practice
1. Calculate heat capacity of 10 g of water at room temperature
2. Calculate heat required to boil 10 g of water from 30 degree Celsius
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SC123 Fundamental Chemistry Asst. Prof. Dr. Peerasak Paoprasert 4
The First Law of Thermodynamics
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SC123 Fundamental Chemistry Asst. Prof. Dr. Peerasak Paoprasert 5
Practice
1. Calculate ∆U of the following reaction at 25 C: N2(g) + 3H2(g) → 2NH3(g)
∆H° = −350 kJ
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SC123 Fundamental Chemistry Asst. Prof. Dr. Peerasak Paoprasert 6
Practice
1. Calculate the enthalpy of the following reaction
CH4(g) + 4F2(g) → CF4(g) + 4HF(g)
Given (C-H) = 413 kJ, (F-F) =159 kJ, (C-F) =489 kJ, (H-F) =567 kJ
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SC123 Fundamental Chemistry Asst. Prof. Dr. Peerasak Paoprasert 7
Practice
1. Calculate enthalpy C(gr) + 1/2O2(g) → CO(g) when
CO(g) + 1/2O2(g) → CO2 (g) ∆H2 = -283kJ
C(gr) + O2(g) → CO2 (g) ∆H3 = -393kJ
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SC123 Fundamental Chemistry Asst. Prof. Dr. Peerasak Paoprasert 8
Practice
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SC123 Fundamental Chemistry Asst. Prof. Dr. Peerasak Paoprasert 9
1. Calculate ∆H°rxn at 25°C of CaCO3(s) → CaO(s) + CO2(g) when ΔH°f, of
CaO(s)=-50.6 kJ/mol, ΔH°f of CO2(g)= -393.5 kJ/mol, and ΔH°f of CaCO3 = -120
kJ/mol
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SC123 Fundamental Chemistry Asst. Prof. Dr. Peerasak Paoprasert 10
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SC123 Fundamental Chemistry Asst. Prof. Dr. Peerasak Paoprasert 11
Practice
1. Calculate ∆S°rxn at 25°C of CaCO3(s) → CaO(s) + CO2(g) when ∆S°CaO(s)=39.8
J/K, ∆S°CO2(g)=213.6 J/K, ∆S°CaCO3 = 92.9 J/K
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SC123 Fundamental Chemistry Asst. Prof. Dr. Peerasak Paoprasert 12
Practice
1. Predict whether or not this reaction is spontaneous if its enthalpy and entropy are
100 kJ/mol and 550 J/K, respectively.
Practice
1. Calculate ∆U at 25 C of 2CO(g) + O2(g) → 2CO2(g) at 25 oC ∆H° =
−566 kJ
2. Calculate w, q, ∆U when 1 mol of liquid water is turned into gas at 100 oC and 1
atm. Density of water at100 oC = 9.583 × 10-3 kg.m-3 and latent heat of water vapor=
40.63 kJ mol-1
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SC123 Fundamental Chemistry Asst. Prof. Dr. Peerasak Paoprasert 13
3. What is the heat capacity of 60 g of water?
4. When 500 g of water is heated from 10 C to 90 C, how much heat is involved? Is this
an endothermic or exothermic process?
5. Calculate ΔH° of C(s) + 2H2(g) → CH4(g).
Given
C(s) + O2(g) → CO2(g) ΔH° = -393 kJ
H2(g) + 1/2O2(g) → H2O(l) ΔH° = -285 kJ
CH4(g) + 2O2(g) → CO2(g) +2H2O(l) ΔH° = -890 kJ
6. Predict the sign of ∆S°rxn of the following reactions
a. Ag+(aq) + Cl¯(aq) → AgCl(s)
b. NH4Cl(s) → NH3(g) + HCl(g)
c. H2(g) + Br2(g) → 2HBr(g)
7. Calculate entropy of the following reactions
a. N2(g) + 3H2(g) → 2NH3(g)
b. H2(g) + Cl2(g) → 2HCl(g)