7. Calculate the work associated with the expansion of a gas from 42.0 L to 79.0 L at a constant pressure of 14.0 atm.
(A) 518 L·atm
(B) –518 L·atm
(C) –1.11 × 103 L·atm
(D) 588 L·atm e. 1.11 × 103 L·atm

8. What is the specific heat capacity of a metal if it requires 169.6 J to change the temperature of 15.0 g of the metal from 25.00°C to 32.00°C? (A) 0.619 J/g°C (B) 11.3 J/g°C (C) 24.2 J/g°C (D) 1.62 J/g°C e. 275 J/g°C

9. Choose the correct equation for the standard enthalpy of formation of CO(g), where ΔHf° for CO = –110.5 kJ/mol (gr indicates graphite).  (A) 2C(gr) + O2(g) → 2CO(g), ΔH° = –110.5 kJ (B) C(gr) + O(g) → CO(g), ΔH° = –110.5 kJ (C) C(gr) + O2(g) → CO(g), ΔH° = –110.5 kJ (D) C(gr) + CO2(g) → 2CO(g), ΔH° = –110.5 kJ e. CO(g) → C(gr) + O(g), ΔH° = –110.5 kJ

10. Which of the following statements best describes the Heisenberg uncertainty principle? (A) The exact position of an electron is always uncertain. (B) The velocity of a particle can only be estimated. (C) It is impossible to accurately know both the exact location and momentum of a particle. (D) The location and momentum of a macroscopic object are not known with certainty. e. The location and momentum of a particle can be determined accurately, but not the identity of the particle.

11. Which of the following best describes an orbital? (A) space where electrons are unlikely to be found in an atom (B) space which may contain electrons, protons, and/or neutrons (C) the space in an atom where an electron is most likely to be found (D) small, walled spheres that contain electrons e. a single space within an atom that contains all electrons of that atom

12. If n = 2, how many orbitals are possible? (A) 3 (B) 4 (C) 2 (D) 8 e. 6

13. How many electrons can be described by the quantum numbers n = 2, l = 2, ml = 2? (A) 0 (B) 2 (C) 6 (D) 10 e. 14

14. Which of the following combinations of quantum numbers is not allowed? (A) n = 1, l = 1, ml = 0, ms = (B) n = 3, l = 0, ml = 0, ms = - (C) n = 2, l = 1, ml = -1, ms = (D) n = 4, l = 3, ml = -2, ms = - e. n = 4, l = 2, ml = 0, ms =

15. Which of the following processes represents the ionization energy of bromine? (A) Br(s) Br+(g) + e– (B) Br(l) Br+(g) + e– (C) Br(g) Br+(g) + e– (D) Br(s) Br+(s) + e– e. Br2(g) Br2+(g) + e–

16. Which of the following groups contains no ionic compounds? (A) HCN, NO2, Ca(NO3)2 (B) PCl5, LiBr, Zn(OH)2 (C) KOH, CCl4, SF4 (D) NaH, CaF2, NaNH2 (E) CH2O, H2S, NH3

17. In which pair do both compounds exhibit predominantly ionic bonding? (A) SCl4 and HF (B) Na2SO3 and NH3 (C) KI and O3  (D) BaF and H2O (E) RbCl and MgS

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