62. Given the electron configuration of an element X is [Ar]3d¹⁰4s² 4p³ . What is the formula for the chloride of X most likely to be?
(A) XCl
(B) XCl₂
(C) XCl₃
(D) XCl₄
(E) XCl₆

63. How much energy is needed to convert 100 g of ice at 0℃ to water at 50℃?  specific heat capacity (ice) = 2.10 J/g· ℃；  specific heat capacity (water) = 4.18 J/g· ℃；  heat of fusion = 333 J/g；heat of vaporization = 2258 J/g (A) 10.1 kJ (B) 20.7 kJ (C) 31.4 kJ (D) 54.2 kJ (E) 65.8 kJ

64. What concentration of glucose in water is needed to produce an aqueous solution isotomic with blood? Give the osmotic pressure of blood at 25℃ is 7.70 atm. (R = 0.082 atm·L/mol·K) (A) 0.158 M (B) 0.315 M (C) 0.630 M (D) 1.580 M (E) 3.15 M

65. Which of the followings is not necessary for protein synthesis at the stage of peptide bonds formation? (A) amino acids (B) mRNA (C) DNA (D) tRNA (E) ribosomes

66. Give the effusion time of 250 mL of methane through a small hole is 48 s. How long will it require for same volume of helium to pass through the same hole? (CH4=16 g/mol； He=4 g/mol) (A) 12 s (B) 24 s (C) 48 s (D) 96 s (E) 192 s

67. Given the second half-life for a second order reaction is 60 seconds. How much time is required for 87.5% reactant to be consumed in this reaction? (A) 30 seconds (B) 60 seconds (C) 90 seconds (D) 120 seconds (E) 210 seconds

68. Which of the following trends is incorrect? (A) atom size: Li ＜ Na ＜ K ＜ Cs (B) ion size: Ca2+ ＜ K+ ＜ Cl– ＜ S2– (C) electronegativity: I ＜ Br ＜ Cl ＜ F (D) boiling point: H2O ＜ H2S ＜ H2Se ＜ H2Te (E) bond angle: SbF3 ＜ AsF3 ＜ PF3 ＜ NF3

69. At 27℃, an ideal gas with a mass of 0.4 g in 100 mL has a pressure of 0.3 atm. What is the molecular weight of this gas molecule? (R = 0.082 atm·L/mol·K) (A) 328 (B) 246 (C) 133 (D) 120 (E) 30

70. The rate constant for a reaction increases from 10.0 s-1 to 100.0 s-1 when the temperature is increased from 300 K to 400 K. What is the activation energy for this reaction in kJ/mol?(R = 8.31 J/mol·K； ln10 = 2.30) (A) 45.6 (B) 23.0 (C) 18.3 (D) 12.7 (E) 5.0

71. Below reaction was studied at –10℃ and the following results were obtained. Considering the rate law of this reaction, what’s the unit of the rate constant? (A) (mol/L)2 ·min-1 (B) (mol/L)1 ·min-1 (C) (mol/L)0 ·min-1 (D) (mol/L)-1 ·min-1 (E) (mol/L)-2 ·min-1

72. Which of the following statements is correct? (A) Arrhenius postulated that an acid is a proton (H+) donor, and a base is a proton acceptor. (B) A buffer with a large capacity contains large volumes of the buffering components. (C) For the titrations of weak acids with strong bases, the greater pH value at the equivalence point is obtained when the stronger acid is used. (D) For a particular buffering system, all solutions that have the same ratio of [A– ]/[HA] have the same pH value. (E) An acid-base indicator can be used to determine the equivalence point of an acid-base titration because of its ability to mark the half-equivalence point of a titration by changing color.

115年 - 115 國立中山大學_學士後醫學系招生考試試題：物理與化學#138404

115年 - 115 學士後醫學系招生考試試題：物理及化學#138377

115年 - 115 國立清華大學_學士後醫學系招生考試試題_學士後醫學系：化學與物理#138209

114年 - 114 學士後醫學系招生考試試題：物理及化學#126679

114年 - 114 國立清華大學_學士後醫學系_自然科學組﹕物理化學#126266

114年 - 114 國立中山大學_學士後醫學系招生考試試題：物理與化學#126239

113年 - 113 國立清華大學_學士後醫學系單招試題_學士後醫學系自然科學組：化學與物理#119930

113年 - 113 學士後醫學系招生考試:物理及化學#119747

113年 - 113 國立中山大學_學士後醫學系招生考試：物理及化學#119273

112年 - 112 學士後醫學系招生考試:物理及化學#114227