109年 - [無官方正解]109 國立嘉義大學_轉學生招生考試試題_農學院、生命科學院：普通化學#144271

1. When the following equation is balanced, what is the coefficient for H₂O? Ca(OH)₂(aq) + H₃PO₄(aq) → Ca₃(PO₄)₂(s) + H₂O(l) (A)2 (B)3 (C)4 (D)6

2. A substance that, when dissolved in water, produces a solution that conducts electric current very efficiently is called (A) a strong electrolyte (B) a weak electrolyte (C) a strong ion (D) an electrical solute

3. Classify the reaction : \[ \text{Cu(NO}_3)_2\text{(}\textit{aq}\text{)} + 2\text{NaOH(}\textit{aq}\text{)} \rightarrow \text{Cu(OH)}_2\text{(s)} + 2\text{NaNO}_3\text{(}\textit{aq}\text{)} \] (A) formation of a solid (B) formation of a gas (C) formation of water (D) transfer of electrons

4. The equation 2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O is an oxidation-reduction reaction. Which statement is true? (A) the carbon is reduced, and the oxygen is oxidized (B) the carbon is oxidized, and the hydrogen is reduced (C) the carbon is oxidized, and the oxygen is reduced (D) it is a decomposition reaction

5. \( \text{Cu(NO}_3)_2\text{(aq)} + 2\text{NaOH(aq)} \rightarrow \text{Cu(OH)}_2\text{(s)} + 2\text{NaNO}_3\text{(aq)} \)
Which one is the net ionic equation?
(A) \( \text{Cu}^{2+}\text{(aq)} + 2\text{NO}_3^-\text{(aq)} \rightarrow \text{Cu(NO}_3)_2\text{(aq)} \)
(B) \( \text{Cu}^{2+}\text{(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{Cu(OH)}_2\text{(s)} \)
(C) \( 2\text{NO}_3^-\text{(aq)} + 2\text{Na}^+\text{(aq)} \rightarrow 2\text{NaNO}_3\text{(aq)} \)
(D) \( \text{Na}^+\text{(aq)} + \text{OH}^-\text{(aq)} \rightarrow \text{NaOH(s)} \)

6. How many electrons are transferred in the following redox reaction?

 Zn(s) + 2AgNO₃(aq) → Zn(NO₃)₂(aq) + 2Ag(s) (A)1 (B)2 (C)3 (D)4

7. Finish and balance the neutralization reaction: HClO₄ (aq) + Ba(OH)₂ (aq) → (A) H₂O (l) + BaCl₂ (aq) (B) H₂O (l) + Ba(ClO₄)₂ (s) (C) H₂O (l) + Ba(ClO₄)₂ (aq) (D) BaO (s) + Cl₂ (g) + H₂O (l)

8. Al(s) + I₂(g) → AlI₃(s). Which one is correct? (A) I₂ is oxidized (B) Al is reduced (C) Al is a reducing agent (D) I₂ is a reducing agent

9. Calculate the molar mass of a sample with a single molecule weighs \(9.31 \times 10^{-23}\) g.
(A) 56.1 g/mol
(B) \(6.47 \times 10^{45}\) g/mol
(C) \(6.02 \times 10^{23}\) g/mol
(D) \(9.31 \times 10^{-23}\) g/mol

10. What percentage of nitrogen contained in (NH₄)₂CO₃ by mass? (A) 58.3% (B) 14.6% (C) 29.2% (D) 18.8% 

11. The molar mass of a compound is 100 g/mol with the percent composition (by mass) of C : H : O = 65.45% : 5.45% : 29.09%. Determine the empirical formula and the molecular formula. (A) CHO and C₆H₆O₆ (B) C₃H₃O and C₆H₆O₂ (C) C₃HO and C₆H₂O₂ (D) CH₂O and C₄H₈O₄

12. There is 100.0 g samples of the following compounds: NH₃, N₂O, HCN, N₂H₄, and HNO₃. Which sample has the least mass percent of nitrogen? (A)NH₃ (B)N₂O (C)HCN (D)HNO₃

13. How many milliliters of 18.2 M H₂SO₄ are needed to prepare 600.0 mL of 0.10 M H₂SO₄? (A)0.30 mL (B)109 mL (C)3.3 mL (D)1.6 mL

14. Which of the following concentration measures will change in value as the temperature of a solution changes? (A)mass percent (B)mole fraction (C)molality (D)molarity

15. Consider the reaction \(^{2}\text{H}_{2} + \text{O}_{2} \rightarrow ^{2}\text{H}_{2}\text{O}\)
What is the ratio of the initial rate of the appearance of water to the initial rate of disappearance of oxygen?
(A)1:1
(B)2:1
(C)1:2
(D)3:2

16. Consider the reaction X → Y + Z

 Which of the following is a possible rate law? (A)Rate = k[X] (B)Rate = k[Y] (C)Rate = k[Y][Z] (D)Rate = k[Z]

17. Which of the following is true about a system at equilibrium? (A)The concentration(s) of the reactant(s) is equal to the concentration(s) of the product(s). (B) No new product molecules are formed. (C) The concentration(s) of reactant(s) is constant over time. (D)The rate of the reverse reaction is equal to the rate of the forward reaction and both rates are equal to zero.

18. For the reaction given below, 2.00 moles of A and 3.00 moles of B are placed in a 6.00-L container. \[ \text{A(g)} + 2\text{B(g)} \rightleftharpoons \text{C(g)} \] At equilibrium, the concentration of A is 0.261 mol/L. What is the concentration of B at equilibrium? (A) 0.261 mol/L (B) 0.355 mol/L (C) 0.500 mol/L (D) 0.522 mol/L

19. For the equilibrium that exists in an aqueous solution of nitrous acid (HNO₂, a weak acid), the equilibrium constant expression is: (A) \( K = \frac{[\text{H}^+][\text{NO}_2^-]}{[\text{HNO}_2]} \) (B) \( K = \frac{[\text{H}^+][\text{N}^{3+}][\text{O}^{2-}]^2}{[\text{HNO}_2]} \) (C) \( K = [\text{H}^+][\text{NO}_2^-] \) (D) \( K = \frac{[\text{H}^+]^2[\text{NO}_2^-]}{[\text{HNO}_2]} \)

20. Identify the strongest base. (A)CH₃O^- (B)CH₃OH (C)CN^- (D)H₂O

21. The correct mathematical expression for finding the molar solubility (s) of Sn(OH)₂ is: (A) \(2s^2 = K_{sp}\) (B) \(4s^2 = K_{sp}\) (C) \(108s^5 = K_{sp}\) (D) \(4s^3 = K_{sp}\)

22. For which process is \(\Delta S\) negative? (A) evaporation of 1 mol of \(CCl_4(l)\) (B) mixing 5 mL ethanol with 25 mL water (C) compressing 1 mol Ne at constant temperature from 1.5 L to 0.5 L (D) raising the temperature of 100 g Cu from 275 K to 295 K

23. Which metal ion has a d⁵ electron configuration? (A)Pd²⁺ (B)Ag⁺ (C)Fe³⁺ (D)V²⁺

24. What is the electron configuration of the Sc(I) ion? (A)[Ar] 4s¹4d¹ (B)[Ar] 3d² (C)[Ar] 3d¹3a¹ (D)[Ar] 4s²

25. Which is a possible product of the chlorination of butane in the presence of light? (A)C₄H₉Cl (B)C₄H₇Cl (C)C₄H₁₀Cl₂ (D)C₄H₆Cl₂