CHEM 430 – Physical Chemistry I
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1. Properties of Gases
2. Thermodynamics
3. Changes of State
4. Chemical Reactions
5. Electrochemistry
6. Kinetic Theory of Gases
7. Chemical Kinetics
8. Changes of State
9. Transport Properties
Chapter 1
1. What is the error in calculating the pressure of 3.00 moles CO2 gas in a 0.250 m3 container at 500.0 K using the ideal gas law instead of van der Waals equation?
2. True or False. At the critical point the first and second derivatives of the pressure with respect to the molar volume are equal to zero.
3. True of False. Virial Equations of state assume that molecules have no volume, but do interact with one another.
4. What is a system called when neither mass or energy is exchanged with the surroundings.
5. When work is done on the system by the surroundings its’ sign is ( + or – ). (Circle one)
6. A mixture of H2 and O2 is 10.0% by mass H2, what are the mole fractions of H2 and O2?
Chapter 2
1. If heat is release by a reaction the reaction is said to be
2. 2.00 moles of an ideal monatomic gas is adiabatically expanded against a constant external pressure of 0.02704 MPa from 0.0500 m3 at 298.15 K to 0.0750 m3. What is the work (w), heat (q), the change internal energy (ΔU) and change in enthalpy (ΔH) of the system for this expansion?
3. What is the work (w), heat (q), the change internal energy (ΔU) and change in enthalpy (ΔH) of the system if the gas in Problem 3 is compressed back to it initial volume isothermally and reversibly?
4. 1.00 mole of an ideal monatomic gas is adiabatically and reversibly expanded from 0.0500 m3 at 300.0 K to 0.150 m3. What is the work (w), heat (q), the change internal energy (ΔU) and change in enthalpy (ΔH) of the system for this expansion?
5. What is the work (w), heat (q), the change internal energy (ΔU) and change in enthalpy (ΔH) of the system if the gas in Problem 4 is compressed back to it initial volume isothermally against a constant pressure of 24.0 kPa?.
6. Determine the change in enthalpy (ΔH) for the reaction,
C3H8(g) + 5 O2 –> 3 CO2(g) + 4 H2O(l)
using the heat of formation data in Table C.2 in your book.
7. When 0.3213 g of glucose was burned in a bomb calorimeter the temperature rose 7.793 K. What is the molar internal energy of combustion of glucose if the heat capacity of the calorimeter is 641J/K?
8. True or False. If an expansion is done isothermally the change in internal energy of the system will be negative.
9. If a variable is only dependent on the initial and final conditions and not the pathway it is referred to as a
10. One mole of an carbon dioxide a real gas is isothermally expanded from 0.0500 m3 at 298.15 K to 0.0750 m3. What is w for the process if you assume van der Waals equation.
11. Derive the expression for reversible work of a isothermal expansion for a virial equation in volume. (Truncate the equation after 3 terms, PVm= RT ( 1+ B/Vm + C/Vm2) )
12. Given that Cp – Cv = α2TV/κT, determine the equation for the difference between Cp and Cv for a real gas that obeys the viral equation given in Problem 2.
Chapter 3
1. One mole of an carbon dioxide a real gas is isothermally expanded from 0.0500 m3 at 298.15 K to 0.0750 m3. What is w for the process if you assume van der Waals equation.
2. Derive the expression for reversible work of a isothermal expansion for a virial equation in volume. (Truncate the equation after 3 terms, PVm= RT ( 1+ B/Vm + C/Vm2) )
3. Given that Cp – Cv = α2TV/κT, determine the equation for the difference between Cp and Cv for a real gas that obeys the viral equation given in Problem 2.
Chapter 3a
1. One mole of an ideal monatomic gas is isothermally expanded against a constant pressure of 0.03305 MPa from 0.0500 m3 at 298.15 K to 0.0750 m3. What are the DSSYS, DSSURR, and DSUNIV? (R= 8.314 Pa m3 T-1 mol-1)
2. One mole of an ideal monatomic gas is reversibly heated at constant volume from 300.0K to 400.0K. What are the DSSYS, DSSURR, and DSUNIV?
3. One mole of an ideal monatomic gas is adiabatically and reversibly expanded from 0.500 dm3 at 298.15 K to 0.750 dm3. What are the DSSYS, DSSURR, and DSUNIV?
4. If the efficiency of a Carnot Heat Engine is 0.80 and the lower temperature reservoir is at 77.32K, what is the temperature of the high temperature reservoir?
5. What are the DU, DH, DSSYS, DSSURR, and DSUNIV for one cycle of the Carnot Heat Engine in Problem 4?
6. What would you expect the sign of DSSYS to be for the irreversible process of converting water (liquid) to ice at -10oC?
7. What is the DS of mixing 4.00 mol of N2 with 1.00 mol of O2 at 300.0 K if both gases are acting ideal?
8. What is the DSRXN for the following reaction?(Use Table C.2 in the text)
2 H2(g) + O2(g) ® 2 H2O (l) : DSRXN=?
9. What is the S298 for HCl given the following data?
a=0.0009521 J K-4mol-1 Cp(16®98.36K)=16.24 J K-1mol-1
DHtrns(I®II)=1.190kJ/mol Cp(98.36®158.91K)=44.00 J K-1mol-1
DHfus(158.91)=1.992kJ/mol Cp(158.91®188.07K)=58.76 J K-1mol-1
DHvap(188.07)=1.190kJ/mol Cp(188.07®298.15K)=29.30 J K-1mol-1
10. A sample of an ideal gas occupies 0.0150 m3 at 250.0 K and 0.100 MPa. To what volume must the gas be compressed isothermally in order to reduce its entropy by 5.00J/K? What is the ΔG and ΔA for this process?
11. What is the molar Gibbs free energy of reaction (ΔGRXN) for the following reaction at 398.15 K and 100.0 bar?
2 NO (g) + O2 (g) —> 2 NO2 (g),
ΔHo298= -228.28 kJ, ΔSo298= 117.20 J/K
12. What if the difference between the CP and CV for 0.100 m3 benzene at 273K if the values for a and k are 12.4×10-4 K-1 and 9.10×10-10 Pa-1 respectively?
13. What is the fugacity coefficient for Ar at 1000. bar and 273 K if the B’ and C’ (virial coefficients) are -8.24×10-3 bar-1 and 2.33×10-6 bar-2, respectively?
Chapter 4
1. One mole of an ideal monatomic gas is isothermally expanded against a constant pressure of 0.03305 MPa from 0.0500 m3 at 298.15 K to 0.0750 m3. What are the ΔSSYS, ΔSSURR, and ΔSUNIV? (R= 8.314 Pa m3 T-1 mol-1)
2. One mole of an ideal monatomic gas is reversibly heated at constant volume from 300.0K to 400.0K. What are the ΔSSYS, ΔSSURR, and ΔSUNIV?
3. One mole of an ideal monatomic gas is adiabatically and reversibly expanded from 0.500 dm3 at 298.15 K to 0.750 dm3. What are the ΔSSYS, ΔSSURR, and ΔSUNIV?
4. If the efficiency of a Carnot Heat Engine is 0.80 and the lower temperature reservoir is at 77.32K, what is the temperature of the high temperature reservoir?
5. What are the ΔU, ΔH, ΔSSYS, ΔSSURR, and ΔSUNIV for one cycle of the Carnot Heat Engine in Problem 4?
6. What would you expect the sign of ΔSSYS to be for the irreversible process of converting water (liquid) to ice at -10oC?
7. What is the ΔSRXN for the following reaction?(Use Table C.2 in the text)
2 H2(g) + O2(g) → 2 H2O (l) : ΔRXN=?
8. What is the S298 for HCl given the following data?
a=0.0009521 J K-4mol-1 Cp(16→98.36K)=16.24 J K-1mol-1
ΔHtrns(I→II)=1.190kJ/mol Cp(98.36→158.91K)=44.00 J K-1mol-1
ΔHfus(158.91)=1.992kJ/mol Cp(158.91→188.07K)=58.76 J K-1mol-1
ΔHvap(188.07)=1.190kJ/mol Cp(188.07→298.15K)=29.30 J K-1mol-1
Chapter 4a
1. The molar volume of a certain solid is 161.0 cm3 mol-1 at 1.00 atm and 350.75 K, its melting temperature. The molar volume of the liquid at this temperature and pressure is 163.3 cm3 mol-1. At 100 atm the melting temperature changes to 351.26 K. Calculate the molar enthalpy and entropy of fusion of the solid.
2. What is the vapor pressure of water at 90.0oC if the standard boiling is 99.6oC? The enthalpy of vaporization of water is 40.656 kJ/mol?
3. What is the vapor pressure of a sample of water at 298 K when a pressure of 10.0 bar is applied externally? The vapor pressure of water at 298 without external pressure is 0.0315 bar and the molar volume of the liquid at 298 is 18.07 cm3 mol-1?
4. What is the mole fraction of water in the vapor over a solution of 2.00 moles of water and 2.00 moles of methanol at 50.0oC, if the vapor pressure of methanol and water at this temperature are 100.0 torr and 92.51 torr respectively? (Assume an ideal solution)
Chapter 5
1. A sample of an ideal gas occupies 0.0150 m3 at 250.0 K and 0.100 MPa. To what volume must the gas be compressed isothermally in order to reduce its entropy by 5.00J/K? What is the ΔG and ΔA for this process?
2. What is the molar Gibbs free energy of reaction (ΔGRXN) for the following reaction at 398.15 K and 100.0 bar?
2 NO (g) + O2 (g) —> 2 NO2 (g),
ΔHo298= -228.28 kJ, ΔSo298= 117.20 J/K
3. What if the difference between the CP and CV for 0.100 m3 benzene at 273K if the values for a and k are 12.4×10-4 K-1 and 9.10×10-10 Pa-1 respectively?
4. What is the fugacity coefficient for Ar at 1000. bar and 273 K if the B’ and C’ (virial coefficients) are -8.24×10-3 bar-1 and 2.33×10-6 bar-2, respectively?
Chapter 5a
1. What is the chemical potential of H2O2(g) at 298.15 K and 10.00 atm if it is -105.57 kJ/mol at 1.00 atm?
2. What is the ΔG, ΔH, and ΔS of mixing 4.00 mol of N2 with 2.00 mol of O2 at 300.0 K if both gases are acting ideal?
3. What is the temperature at which an 0.100 molal aqueous solution of isopropanol(C3H8O) will boil? (ΔHVAP=44.0 kJ/mol)
4. What is the molar mass of a compound if its osmotic pressure at 298K is 34.0 torr when 0.2 grams is added to 0.500 liters?
5. What is the mean concentration, inoic Strenght, mean activity coefficient and mean activity of a 0.0100 molal solution of CaCl 2 (aq) at 25 ° C? (Assume Debye Hückel Theory)
6. What is the activity coefficient of water in a mixture of 10.0 moles of water and 0.5 moles of ethanol at 50.0 oC if the partial pressure of water in this mixture at this temperature is 90.0 torr? The vapor pressure of pure water at this temperature is 92.51 torr.
Chapter 6
1. The molar volume of a certain solid is 161.0 cm3 mol-1 at 1.00 atm and 350.75…
