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106年 - 106 高雄醫學大學_學生轉系考試：普通化學#86786

科目：轉學考-普通化學 | 年份：106年 | 選擇題數：25 | 申論題數：0

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所屬科目：轉學考-普通化學

選擇題 (25)

1. Which of the following statement in regard to unit conversions is correct? (A) One kilogram is equal to 10-9 teragrams. (B)Twenty-five femtograms are equal to 2.5 × 10-14 kilograms. (C) Eight liters are equal to 80 cubic decimeters. (D) 294.5 nm are equal to 2.945 × 107 centimeters. (E)One microliter is equal to 10-6 milliliters.
2. Which one of the following statements is correct? Assume the acids are dissolved in water. (A) The systematic name for H2SO4 is hydrosulfuric acid. (B)The systematic name for ICl is iodine chloride. (C) The systematic name for NH4NO3 is nitrogen tetrahydrogen nitrate. (D) The systematic name for Sr3N2 is tristrontium dinitrogen. (E)The systematic name for KClO3 is potassium chlorite.
3. Which one of the following statements is correct? (A) The systematic name for TeO32- 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 When a portion of the helium is withdrawn and adjusted to 1.00 atm at 25°C, it is found to have a volume of 1.75 cm3 .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) 7 × 10-4 (B)7 × 10-3 (C) 7 × 10-2 (D) 0.7 (E)7
5. Which one of the following statements is correct? (A) For a 1.0-L container of neon gas at STP, its frequency of collision with the container walls will increase when the temperature is decreased to -50°C. (B)Real gas behaves most ideally when a container volume is relatively small and the gas molecules are moving relatively slow. (C) For separate 1.0-L gaseous samples of H2, Xe, Cl2 and O2 all at STP, H2 has the highest average velocity. (D) For separate 1.0-L gaseous samples of H2 and O2 that all have the same average velocity, O2 has a lower temperature. (E)For separate 1.0-L gaseous samples of H2, Xe, Cl2 and O2 all at STP, Xe has the highest average kinetic energy.
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 ∆Hf o 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 ∆Hf o to calculate the value of ∆Ho 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) 3.64 × 10-4 m (B)5.79 × 10-4 m (C) 3.64 × 10-33 m (D) 5.79 × 10-33 m (E)3.64 × 10-18 m
8. Which of the following statements is correct? (A) Argon has ionization energy higher than bromine. (B)Among Na- , Na, and Na+ , Na- 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 1s2 2s2 2p6 3s2 3p6 4s2 3d104p6 5s2 4d10. (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 ∆Hfo 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 O22+ and N2 2+, O2 2+ 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.
11. Which of the following statements is correct? (A) CO2 has intermolecular forces greater than that of OCS. (B)LiF has its freezing point lower than those of F2 and HCl. (C) CaO has its enthalpy of fusion smaller than those of I2 and CsBr. (D) H2O2 has its viscosity greater than those of HF and H2S. (E)H2CO has intermolecular forces greater than that of CH3OH.
12. Calcium has a cubic closest packed structure as a solid. Assuming that calcium has an atomic radius of 197 pm, please calculate the density of solid calcium to be__________ g/cm3 (A) 11.6 (B)1.54 (C) 4.5 (D) 3.38 (E)22.68
13. In order to prepare a solution with a freezing point of -1.50°C, 200.0 g water has to be added glycerin (C3H8O3), a nonelectrolyte, with mass of__________ g to attain the desired aqueous solution. (A) 0.018 (B)36.46 (C) 18.1 (D) 26.0 (E)14.8

14. Consider the reaction 3A + B + C 5ee046d5c5919.jpgD + 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 × 10-4 M. We also know that after 3.00 min of the reaction, [A]is 3.26 × 10-5 M. What will be the concentration of A after 10.0 min? (A) 1.27 × 10-5 M (B)2.5 × 10-6 M (C) 1.00 M (D) 2.50 × 10-5 M (E)7.90 × 10-5

15. Ea for the uncatalyzed reaction O3(g) + O(g) → 2O2 is 14.0 kJ. Ea for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 25℃? Assume that the frequency factor A is the same for each reaction. (A) 215 (B)51 (C) 2.3 (D) 532 (E)0.25

16. Consider the decomposition equation of a compound: C5H6O3(g) 5ee04767b4b68.jpgC2H6(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) 3.89 × 10-1 (B)6.74 × 10-6 (C) 8.00 × 10-2 (D) 4.00 × 10-3 (E)1.20 × 10-9 
17. Which of the following 0.10 M solutions are correctly arranged in order of most acidic to most basic? (A) HCl > KCl > NH4Cl > KCN > KOH (B)NH4Cl .> HCl .> KCl > KCN > KOH (C) NH4Cl .> HCl .> KCN > KCl > KOH (D) HCl > NH4Cl > KCl > KCN > KOH (E)HCl > NH4Cl > KCN > KCl > KOH
18. A 0.15 M solution of a weak acid is 3.0% dissociated. The Ka of the acid is calculated to be . (A) 3.5 × 10-4 (B)4.2 × 10-3 (C) 1.4 × 10-4 (D) 2.4 × 10-2 (E)3.6 × 10-3
19. Two drops of indicator HIn (Ka = 1.0 × 10-9 ), 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 (Ksp = 4 × 10-38) in a solution buffered at pH = 5.0 is mol/L (A) 4.0 × 10-11 (B)2.5 × 10-10 (C) 2.5 × 10-4 (D) 4.0 × 10-29 (E)4.0 × 10-17
21. Which of the following statements is correct? (A) For HCl(g) → H+ (aq) + Cl- (aq), its ∆So is larger than 0 (> 0) (B)The So of Cgraphite(s) is larger than the So of Cdiamond(s) (C) One mol H2 (at STP) has more positional probability than 1 mol H2 at 100 K, 0.5 atm. (D) The sign of ∆Ssurr for the process of I2(g) → I2(s) is negative (-). (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)5ee0484f15962.jpg N2O4(g). The values of ∆Ηο and ∆Sο are -58.03 kJ/mol and -176.6 J/K•mol, respectively. Assuming ∆Η ο and ∆Sο are temperature independent, estimate the value of K at 100.0°C. (A) 3.00 × 106 (B)1.47 × 10-87 (C) 8.72 (D) 7.89× 10-2 (E)5.9 × 1015

23. An unknown metal M is electrolyzed. It took 74.1 s for a current of 2.00 A to plate out 0.107 g of the metal from a solution containing M(NO3)3. The metal is therefore identified as________ . (A) aluminum (B)cobalt (C) bismuth (D) lead (E)gallium
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) 1.22 × 10-11 (B)1.22 × 10-12 (C) 1.22 × 10-13 (D) 1.47 × 10-12 (E)1.47 × 10-11
25. When proteins in solution are heated, the hydrogen bonds in proteins may be broken to result in collapsing of protein secondary structures. What will be the effects of the heating process on ∆H and ∆S of the proteins? (A) ∆H and ∆S all will increase. (B)∆H and ∆S all will decrease. (C) ∆H will increase but ∆S will decrease. (D) ∆H will decrease but ∆S will increase (E)Both ∆H and ∆S will not change. 

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