106年 - 106 高雄醫學大學學生轉系考試：普通化學#99839

1. Which of the following statement in regard to unit conversions is correct? (A) One kilogram is equal to teragrams. (B) Twenty-five femtograms are equal to kilograms. (C) Eight liters are equal to 80 cubic decimeters. (D) 294.5 nm are equal to centimeters. (E) One microliter is equal to milliliters.

3. Which one of the following statements is correct? (A) The systematic name for is tellurate ion. (B) The systematic name for Hg₂Cl₂ is mercury chloride. (C) The systematic name for Mg3(SbO₄)₂ is magnesium antimonate. (D) The systematic name for GaAs is gallium arsenate. (E) The systematic name for Na₂O₂ is sodium oxide.

4. A spherical glass container of unknown volume contains helium gas at 25°C and 1.960 atm. When a portion of the helium is withdrawn and adjusted to 1.00 atm at 25°C, it is found to have a volume of 1.75 cm³ . The gas remaining in the first container shows a pressure of 1.710 atm. The volume of the spherical container is _________ L. (A) (B) (C) (D) 0.7 (E) 7

6. The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves the following steps:
4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(g)
2NO(g) + O₂(g) → 2NO₂(g)
3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g). The values of for some chemicals are the following: NO(g), 90 kJ/mol；H₂O(g), -242 kJ/mol； NH₃(g), -46 kJ/mol； NO₂(g), 34 kJ/mol； HNO₃(aq), -207 kJ/mol； H₂O(l), -286 kJ/mol. Use the provided values of to calculate the value of for the last reaction, 3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g) to be ______.
(A) -908 kJ (B) -112 kJ (C) -140 kJ (D) -826 kJ (E) -220 kJ

7. Using the Heisenberg uncertainty principle, please calculate the ∆x for a baseball (mass = 145 g) with ∆v = 0.100 m/s to be . (A)m (B)m (C)m (D)m (E)m

8. Which of the following statements is correct? (A) Argon has ionization energy higher than bromine. (B) Among has the smallest radius. (C) For Rb, Na, and Be, the order of increasing atomic size is Rb ＜ Na ＜ Be. (D) In the ground state of mercury, Hg, its electron configuration is . (E) In the ground state of element 115, Uup, it has 24 electrons occupying atomic orbitals with l = 3.

9. Please use the following data to estimate for potassium chloride to be _________ kJ/mol.
K(s) + (1/2)Cl₂(g) → KCl(s)； lattice energy, -690. kJ/mol； ionization energy for K, 419 kJ/mol； electron affinity of Cl, -349 kJ/mol； bond energy of Cl₂, 239 kJ/mol； ethalpy of sublimation for K, 90. kJ/mol. (A) -161 (B) -1085 (C) 161 (D) 1085 (E) -411

10. Which of the following statements is correct? (A) F2 + has its bond order of 1.5. (B) CN- is paramagnetic. (C) Between would most likely gain an electron. (D) The predicted molecular structure and expected hybrid orbitals on the central atom of TeF4 are see-saw and d² sp ³ , respectively. (E) The predicted molecular structure and expected hybrid orbitals on the central atom of IF₄ is trigonal bipyramid and d² sp ³ , respectively.

14. Consider the reaction 3A + B + C⇌D + E where the rate law is defined as –(∆[A]/∆t) = k[A]² [B][C]. An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 1.00 × M. We also know that after 3.00 min of the reaction, [A] is 3.26 × M. What will be the concentration of A after 10.0 min? (A)M (B)M (C) 1.00 M (D)M (E)M

16. Consider the decomposition equation of a compound: C₅H₆O₃(g)⇌C₂H₆(g) + 3CO(g). When a 5.63-g sample of pure C₅H₆O₃(g) was sealed into an otherwise empty 2.50-L flask and heated to 200℃, the pressure in the flask gradually rose to 1.63 atm and remained at that value. The K value for this reaction is _____ . (A) (B) (C) (D) (E)

18. A 0.15 M solution of a weak acid is 3.0% dissociated. The Ka of the acid is calculated to be _______ . (A) (B) (C) (D)(E)

19. Two drops of indicator HIn (Ka = ), where HIn is yellow and In- is blue, are placed in 100.0 mL of 0.10 M HCl. The solution is titrated with 0.10 M NaOH. At what pH will the color change (yellow to greenish yellow) occur? (A) 7.0 (B) 8.5 (C) 9.0 (D) 7.5 (E) 8.0

20. The solubility of Fe(OH)₃ () in a solution buffered at pH = 5.0 is _________ mol/L (A) (B)(C) (D) (E)

21. Which of the following statements is correct? (A)(B)(C) One mol H₂ (at STP) has more positional probability than 1 mol H₂ at 100 K, 0.5 atm. (D)(E) At constant T and P, the change with ∆Η = +25 kJ, ∆S = +100 J/K, T = 300. K is not a spontaneous process.

22. Consider the following reaction at 25°C: 2NO₂(g)⇌N₂O₄(g). The values of ∆Η^ο and ∆S^ο are -58.03 kJ/mol and -176.6 J/K•mol, respectively. Assuming ∆Η^ο and ∆S^ο are temperature independent, estimate the value of K at 100.0°C. (A) 3.00 × 10⁶ (B)(C) 8.72 (D) (E)

24. The atomic mass of ¹ H is 1.00782 amu and the mass of a neutron is 1.00866 amu. The binding energy for uranium-235 (atomic mass 235.0439 u) is calculated to be ________ J/nucleon. (A)(B) (C)(D) (E)