R = 0.08206 L.atm/mol.K   1 atm = 760 torr   R = 8.314 J/mol.K
VcMc = VdMd         naMaVa = nbMbVb   PV = nRT
q = mCsDT         DH = -qsurr      Pi = ciPT   
Molar Mass (MM)      MM = m/n      ci = ni/nT   
urms = (3RT/MM)1/2       tA/tB = (MMA/MMB)1/2   
DH° = S nDHf°(products) - S mDHf°(reactants)   




1. Which compound listed below is soluble in water?
A.BaSO4
B.AgCl
C.MgCO3
D.Na2CO3
E.none of these


2. Which equation is the net ionic equation for the reaction in water of BaCl2 and Na2SO4.
A.BaCl2(aq) + Na2SO4(aq) ® BaSO4(s) + 2NaCl(aq)
B.BaCl2(s) ® Ba2+(aq) + 2Cl-(aq)
C.Ba2+(aq) + SO42-(aq) ® BaSO4(s)
D.Na+(aq) + Cl-(aq) ® NaCl(s)
E.none of these


3. What mass of NaOH is needed to make 450 mL of a 2.0 molar solution?
A.18 g
B.42 g
C.36 g
D.24 g
E.12 g


4. What volume of 1.1 M HCl is needed to prepare 100 mL of a 0.20 M HCl solution?
A.9.0 mL
B.18 mL
C.32 mL
D.36 mL
E.48 mL


5. What mass of Al(OH)3 is formed from mixing 1.24 L of 0.332 molar AlCl3 with excess NaOH?
A.12.1 g
B.40.3 g
C.24.1 g
D.32.1 g
E.17.6 g


6. How many mL of 1.0 M HCl will be needed to react with 5.0 mL of 2.0 M Ca(OH)2?
A.10 mL
B.20 mL
C.5.0 mL
D.1.0 mL
E.none of these


7. What is the concentration of a HCl solution if experiment shows that 33.2 mL of the solution neutralizes the base in 0.223 g of NaOH?
A.0.168 molar
B.0.223 molar
C.0.332 molar
D.0.442 molar
E.0.536 molar


8. What is the molarity of a NaCl solution if the addition of excess AgNO3 to a 40 mL sample of the solution yields 0.123 g of AgCl?
A.0.011 molar
B.1.4 molar
C.0.021 molar
D.0.11 molar
E.2.3 molar


9. Given the three statements below, which answer is correct?
(a) A thermochemical equation must include the physical state of all substances.
(b) The coefficients in a thermochemical equation are interpretted as moles.
(c) The sign of DH is negative for an endothermic reaction.
A.a and b are true, c is false
B.a and c are true, b is false
C.a, b, and c are all true
D.a, b, and c are all false
E.b and c are true, a is false


10. Given the equation below, what is DH for burning 8.0 g of C2H2(g) in excess O2(g)?
2C2H2(g) + 5O2(g) ® 4CO2(g) + 2H2O(l)   DH = -2600 kJ
A.-200 kJ
B.-400 kJ
C.-800 kJ
D.-1600 kJ
E.-600 kJ


11. A chemical reaction releases enough heat to raise the temperature of 35.2 g of water from 25.60°C to 34.80°C. Given that the specific heat of water is 4.184 J/g·K, what is the heat evolved?
A.6.22 kJ
B.2.55 kJ
C.9.15 kJ
D.1.35 kJ
E.2.77 kJ


12. In the reaction of 8.00 g of SO2(g) with excess oxygen, 9.85 kJ of heat are released. What is DH for the thermochemical equation: 2SO2(g) + O2(g) ® 2SO3(g) ?
A.-1.58 x 102 kJ
B.-78.8 kJ
C.-39.4 kJ
D.+78.8 kJ
E.+33 kJ


13. Given the following thermochemical equations:
2C2H2(g) + 5O2(g) ® 4CO2(g) + 2H2O      DH = -2601 kJ   
C8H8(l) + 10O2(g) ® 8CO2(g) + 4H2O(l)   DH = -4393 kJ
Calculate the enthalpy change for the reaction
   4C2H2(g) ® C8H8(l)             DH = ?
A.1792 kJ
B.-809 kJ
C.-6994 kJ
D.-9595 kJ
E.703 kJ


14. Given the data below, what is DH° for 2H2S(g) + 3O2(g) ® 2H2O(l) + 2SO2(g)?
[H2S(g)] = -21 kJ/mol    [H2O(l)] = -286 kJ/mol
[SO2(g)] = -297 kJ/mol
A.-562 kJ
B.832 kJ
C.-1124 kJ
D.-1420 kJ
E.782 kJ


15. "Condensed phase" refers to:
A.gases only
B.gases and liquids
C.liquids only
D.liquids and solids
E.solids only


16. Given the three statements below, pick the correct answer.
(a) Pressure is directly proportional to temperature in kelvins.
(b) Volume is directly proportional to pressure.
(c) Volume is directly proportional to the number of moles of the gas sample.
A.a and b are true, c is false
B.a and c are true, b is false
C.b and c are true, a is false
D.all three are true
E.only c is true


17. What pressure will a given sample of gas have at 27°C if at 100°C this gas exerts a pressure of 4.0 atm, all measurements at constant volume?
A.5.0 atm
B.3.2 atm
C.1.1 atm
D.15 atm
E.12 atm


18. What is the final pressure of a gas if a given sample at 300°C, 2.2 atm and 2.4 L is changed to 0°C and 1.0 L?
A.6.4 atm
B.9.1 atm
C.2.5 atm
D.5.3 atm
E.3.7 atm


19. How many moles are present in a 2.00 L sample of gas at 30°C and 0.821 atm?
A.18.5 mol
B.1.50 mol
C.0.667 mol
D.6.60 x 10-2 mol
E.none of these


20. What is the molar mass of a gas if 16 g occupy 3.0 L at 2.2 atm and 27°C?
A.30 g/mol
B.45 g/mol
C.60 g/mol
D.90 g/mol
E.100 g/mol


21. What volume of H2 gas will be produced at 1.0 atm and 28°C if 10 g of Na are mixed with 100 g of H2O? The other product of the reaction is NaOH.
A.0.48 L
B.5.4 L
C.11 L
D.2.7 L
E.3.3 L


22. A sample of gas is prepared by mixing 0.10 mol Ar, 0.10 mol N2, and 0.30 mol He. If the entire vessel is at a pressure of 2.1 atm, what is the partial pressure of He?
A.1.5 atm
B.1.3 atm
C.1.0 atm
D.1.8 atm
E.0.77 atm


23. Which statement listed below is not part of the kinetic model for gases?
A.An ideal gas consists of molecules (or atoms) in constant, random motion.
B.Gas molecules do not exert forces on one another except when they collide.
C.The volume of the molecules is negligible compared to the space between them.
D.The molecules of an ideal gas collide with the walls of their container and with each other.
E.All four of the above statements are part of the kinetic model.


24. For which of the samples listed below will the average molecular speed be greatest?
A.N2 at 400 K
B.N2 at 300 K
C.SO2 at 400 K
D.SO2 at 300 K
E.All of them have the same average speed.


25. Under which of the following conditions would you expect a sample of N2 (boiling point = -196°C) to behave most nearly as an ideal gas?
A.0.05 atm, -160°C
B.0.05 atm, 300°C
C.2000 atm, -160°C
D.2000 atm, 300°C
E.behaves ideally under all these conditions



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