2. 100.0 mL of 2.50 M H2SO4 are added to 150.0 mL of 4.00 M H2SO4. Assuming that the volumes are additive, the final concentration of H2SO4 is A. 3.00 M B. 3.25 M C. 3.40 M D. 3.50 M
3. How much water should be added to 205 mL of a 1.15 M HCl solution to produce a 0.810 M HCl solution ? Assume volumes are additive. A. 291 mL B. 144 mL C. 86 mL D. 125 mL
4. What volume of 0.50 M HCl is required to neutralize 5.0 mL of 2.0 M Ca(OH)2 ? A. 5.0 mL B. 10. mL C. 20. mL D. 40. mL
5. Which of the following solutions will yield a precipitate when mixed ? 1. CuCl2(aq) + NaOH(aq) 4. NaNO3(aq) + KOH(aq) 2. BaCl2(aq) + H2SO4(aq) 5. AgNO3(aq) + NaCl(aq) 3. NH4Cl(aq) + HCl(aq) 6. CaCl2(aq) + Na2CO3(aq) A. 1, 2, 3, 6 B. 2, 3, 4, 5 C. 3, 4, 5, 6 D. 1, 2, 5, 6
6. For the reaction Co(s) + Cl2(g) = CoCl2(s) H = -312.5 kJ What is the enthalpy change when 5.00 g of cobalt reacts with an excess of chlorine gas ? A. -26.5 kJ B. +312.5 kJ C. -312.5 kJ D. -1.56 x 103 kJ
7. Given the following information, C(graphite) + O2(g) = CO2(g) H = -393.5 kJ C(diamond) + O2(g) = CO2(g) H = -395.2 kJ What is the enthalpy change for the transformation from graphite to diamond ? C(graphite) = C(diamond) A. 0 kJ B. 1.7 kJ C. -1.7 kJ D. -788.7 kJ
8. A one gram sample of aluminum (specific heat of Al = 0.900 J/g-K) is heated to 100 deg C and dropped into 10 g of water at 0oC (specific heat of water = 4.18 J/g-K). What is the final water temp- erature ? (Assume the aluminum loses all of the heat to the water.) A. 2oC B. 0.1oC C. 98oC D. 54oC
9. The reaction of magnesium metal and hydrochloric acid produces hydrogen gas and magnesium chloride. What volume (in L) of hydrogen may be formed at 738 torr and 24oC from 1.31 g of magnesium ? A. 2.70 L B. 0.676 L C. 5.41 L D. 1.35 L
10. In a 1.00 L flask, 20.0 g of H2 is mixed with 20.0 g of O2 at 0oC. What is is the pressure inside the container ? A. 222 atm B. 14.0 atm C. 236 atm D. 208 atm
11. How many liters of H2(g) and O2(g) are required to form 7 L of H2O(g), all volumes being measured at STP ? 2 H2(g) + O2(g) = 2 H2O(g) A. 14 L H2, 7 L O2 B. 7 L H2, 3.5 L O2 C. 2 L H2, 1 L O2 D. 22.4 L H2, 11.2 L O2
12. A gas is most likely to behave as an ideal gas at A. high temperatures and low pressures. B. low temperatures and low pressures. C. high temperatures and high pressures. D. low temperatures and high pressures.
13. Which one of the following statements is not consistent with the kinetic molecular theory of gases ? A. Collisions of gas particles are elastic. B. There are attractive and repulsive forces between gas particles. C. The average kinetic energy is proportional to temperature on the Kelvin scale. D. Gases are made up of small particles that are in constant and random motion.
14. At 27oC and 1.00 atm, the density of a gaseous compound is 1.79 g/L. The compound is A. C2H4 B. C2H6 C. C3H8 D. C4H8
15. At constant volume, an increase in the temperature of a gas would cause an increase in the pressure of the gas, because A. Boyle's law says so. B. the collisions of gas particles will exert a greater force on the walls of the container due to higher rms speed of the gas particles on the walls. C. the number of collisions on the walls per unit area per unit time will increase. D. both B and C.
16. If the temperature of a gas sample is changed from 200 K to 400 K and its pressure changes from 2 atm to 1 atm. What must happen to the volume if no gas is lost ? A. The volume stays the same. B. The volume is twice the original volume. C. The volume is one half of the original volume. D. The volume is four times greater than the original volume.
17. A mixture of helium (He) gas and an unknown gas effuses through a small hole. The helium effuses 2.24 times faster than the unknown. What is the unknown gas ? A. Ne B. H2 C. Ar D. Kr
18. WEKU broadcasts at a frequency of 88.9 MHz. What is the wave- length of the radiation from this FM station ? A. 3.00 mm B. 3.37 m C. 10.4 m D. 3.00 km
19. What is the wavelength of an electron that is moving at a velocity of 2.20 x 106 m/s ? (me = 9.11 x 10-31 kg) A. 454 nm B. 0.331 nm C. 3.02 x 109 nm D. 302 nm
20. The notation for the subshell with n = 2 and l = 2 is A. 2 p B. 2 d C. 3 d D. This combination is not allowed.
21. What is the maximum number of electrons that can occupy an f orbital ? A. 2 B. 3 C. 7 D. 14
22. What is the energy of one mole of photons with a wavelength of 750 nm ? A. 4.00 x 105 J B. 4.00 x 10-14 J C. 2.65 x 10-19 J D. 160 kJ
23. Which one of the following equations properly relates the energy (E) of a photon to the wavelength (lambda), the frequency (nu), the speed of light (c), or Planck's constant (h) ? A. E = h lambda B. E = h c / lambda C. E = h c / nu D. E = lambda / h c
24. The orbital diagram for a nitrogen atom in its ground state is
25. The possible values of the magnetic quantum number of a 3d electron are A. +1, +2, +3 B. 0, +1, +2 C. -2, -1, 0, +1, +2 D. -1, 0, +1