42. For an electron in a one-dimensional box, what is the minimum energy to excite the electron from the ground state?
(A)\( \frac{h^2}{8mL^2} \)
(B)\( \frac{2h^2}{8mL^2} \)
(C)\( \frac{3h^2}{8mL^2} \)
(D)\( \frac{4h^2}{8mL^2} \)
(E)\( \frac{5h^2}{8mL^2} \)

1. An element's most stable ion forms an ionic compound with chlorine having the formula \( \text{XCl}_2 \). If the mass number of the ion is 40 and it has 18 electrons, what is the element and how many neutrons does it have? (A)Ar, 22 neutrons (B)Ar, 24 neutrons (C)S, 24 neutrons (D)Ca, 20 neutrons (E)K, 19 neutrons

2. A material is made from Al, Ga, and As. The mole fractions of these elements are 0.25, 0.26, and 0.49, respectively. This material would be (A)a metallic conductor because Al is present. (B)an insulator. (C)a \( p \)-type semiconductor. (D)an \( n \)-type semiconductor. (E)superconductor.

3. How many protons, neutrons, and electrons does the atom \( ^{33}\text{S} \) have? (A)16 protons, 16 neutrons, 33 electrons (B)17 protons, 17 neutrons, 16 electrons (C)16 protons, 16 neutrons, 16 electrons (D)17 protons, 16 neutrons, 17 electrons (E)16 protons, 17 neutrons, 16 electrons

4. A certain substance, X, has a triple-point temperature of \( 20^\circ\text{C} \) at a pressure of 2.0 atm. Which one of the following statements cannot possibly be true? (A)X can exist as a liquid above \( 20^\circ\text{C} \). (B)X can exist as a solid above \( 20^\circ\text{C} \). (C)Liquid X can exist as a stable phase at \( 25^\circ\text{C} \), 1 atm. (D)Both liquid and solid X have the same vapor pressure at \( 20^\circ\text{C} \). (E)All of these statements could be true.

5. Iron is biologically important in the transport of oxygen by red blood cells from the lungs to the various organs of the body. In the blood of an adult human, there are approximately \( 2.60 \times 10^{13} \) red blood cells with a total of 2.90 g of iron. On the average, how many iron atoms are present in each red blood cell? (molar mass for Fe = 55.85 g) (A)\( 8.33 \times 10^{-10} \) (B)\( 1.20 \times 10^9 \) (C)\( 3.12 \times 10^{22} \) (D)\( 2.60 \times 10^{13} \) (E)\( 5.19 \times 10^{-2} \)

6. A liquid-liquid solution is called an ideal solution if I. it obeys \( PV = nRT \). II. it obeys Raoult's law. III. solute-solute, solvent-solvent, and solute-solvent interactions are very similar. IV. solute-solute, solvent-solvent, and solute-solvent interactions are quite different. (A)I, II, III (B)I, II, IV (C)II, III (D)II, IV (E)I, II

7. To calculate the concentration in molarity of a salt solution, you need to know (A)the mass of the salt added to the solution and the volume of water added to the solution. (B)the mass of the salt added to the solution and the total volume of the solution. (C)the mass of the salt added, the molar mass of the salt, and the total volume of the solution. (D)the molar mass of the salt and the total volume of the solution. (E)the mass of the salt added, the molar mass of the salt, the volume of water added, and the total volume of the solution.

8. Which pair of ions would not be expected to form a precipitate when dilute solutions of each are mixed? (A)\( \text{Cu}^{2+}, \text{S}^{2-} \) (B)\( \text{Ag}^+, \text{Cl}^- \) (C)\( \text{Ca}^{2+}, \text{PO}_4^{3-} \) (D)\( \text{Mn}^{2+}, \text{OH}^- \) (E)\( \text{Mg}^{2+}, \text{SO}_4^{2-} \)

9. The molar mass of a solid as determined by freezing-point depression is 10% higher than the true molar mass. Which of the following experimental errors could not account for this discrepancy? (A)Not all the solid was dissolved. (B)More than the recorded amount of solvent was pipetted into the solution. (C)The solid dissociated slightly into two particles when it dissolved. (D)Some solid was left on the weighing paper. (E)Before the solution was prepared, the container was rinsed with solvent and not dried.

10. The mass of 1.12 L of gas Y is found to be 6.23 g. The density of gas Y is (A)10.6 g/L. (B)5.56 g/L. (C)15.6 g/L. (D)0.200 g/L. (E)0.180 g/L.

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