104年 - [無官方正解]104 國立嘉義大學_轉學生招生考試試題：普通化學#145283

1. Express 1840000 in scientific notation. (A) 5.41x10⁸ (B) 1.84x10⁶ (C) 1.84x10⁶ (D) 184x10⁶ (E) 184x10⁴

2. Using the rules of significant figures, calculate the following:
70 + 4.461
(A) 70 (B) 75 (C) 74.46
(D) 74.461 (E)74

3. How many significant figures are in the number 4.00700×1013?
(A) 2 (B) 4 (C) 5
(D) 6 (E) none of these

4. Convert: –12.2°C = _____________ °F.
(A) –54.0°F (B) 10.0°F (C) 25.2°F
(D) –38.8°F (E) –22.0°F

5. The state of matter for an object that has a definite volume but not a definite shape is
(A) solid (B) liquid (C) gaseous
(D) elemental (E) mixed

6. Which of the following is an element?
(A) brass (B) salt (C) water
(D) earth (E)oxygen

7. The symbol Fe stands for the element
(A) francium (B) fluorine (C) fermium
(D) tin (E) iron

8. The symbol for the element mercury is
(A) Hg (B) Mg (C) He
(D) Mn (E) none of these

9. How many protons, electrons, and neutrons, respectively, does 31P have?
(A) 15, 15, 16 (B) 15, 16, 15 (C) 16, 15, 31
(D) 15, 15, 31 (E) 15, 31, 16

10. The correct name for LiCl is
(A) lithium monochloride (B) lithium(I) chloride (C) monolithium chloride
(D) lithium chloride (E) monolithium monochloride

11. The correct name for P₂O₅ is (A) phosphorus(II) oxide (B) phosphorus(V) oxide (C) diphosphorus oxide (D) diphosphorus pentoxide (E) phosphorus pentoxide

12. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? \[ \text{Na}_2\text{S}_2\text{O}_3 + \text{I}_2 \rightarrow \text{NaI} + \text{Na}_2\text{S}_4\text{O}_6 \] (A) 1 (B) 2 (C) 3 (D) 4 (E) 6

13. An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of barium nitrate. Identify the solid in the balanced equation. (A) BaSO₄ (B) (NH₄)₂SO₄ (C) Ba(NO₃)₂ (D) NH₄NO₃ (E) There is no solid formed when the two solutions are mixed.

14. 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 (E) 8

15. 2 moles of oxygen atoms represent (A) \( 0.7 \times 10^{24} \) atoms (B) 0.4 g (C) \( 1.0 \times 10^{2} \) g (D) \( 1.9 \times 10^{1} \) atoms (E) none of these

16. 4.04 moles of water weighs (A) 72.8 g (B) 2.24 x10^-1 g (C) 4.46 g (D) 22.1 g (E) 78.5 g

17. A hydrocarbon has the formula C₅H₁₂. What is the percent by mass of carbon in the compound? (A) 83.2 % (B) 41.6 % (C) 16.8 % (D) 29.4 % (E) 15.7 %

18. A certain compound has an empirical formula of NH₂O. Its molar mass is between 55 and 65 g/mol. Its molecular formula is (A) NH₂O (B) N₂H₄O₂ (C) N₃H₆O₃ (D) not calculable

19. The balanced equation 2Cu(s) + O₂(g) → 2CuO(s) tells us that 4.0 mol of Cu (A) reacts with 4.0 mol of O₂ (B) produces 4.0 mol of CuO (C) must react with 128 g of O₂ (D) cannot react with oxygen (E) produces 8.0 mol of CuO

20. Refer to the following equation: \[ 4\text{NH}_3(g) + 7\text{O}_2(g) \rightarrow 4\text{NO}_2(g) + 6\text{H}_2\text{O}(g) \] How many molecules of NO₂ are produced when 5.38 mol of ammonia is completely reacted? (A) 21.52 (B) 6.48 × 10²⁴ (C) 3.24 × 10²⁴ (D) 247 (E) none of these

21. Methane, CH₄, the major component of natural gas, burns in air to form CO₂ and H₂O. What mass of water is formed in the complete combustion of 7.07 x 10³ g of CH₄? (A) 2.55 x 10³ g (B) 7.94 x 10³ g (C) 2.38 x 10⁴ g (D) 1.59 x 10⁴ g (E) none of these

22. Consider that calcium metal reacts with oxygen gas in the air to form calcium oxide. Suppose we react 6.02 mol calcium with 4.00 mol oxygen gas. Determine the number of moles of calcium oxide produced after the reaction is complete.
(A) 6.02 mol CaO (B) 3.01 mol CaO (C) 4.01 mol CaO
(D) 8.00 mol CaO (E) none of these

23. A 6.75-g sample of gold (specific heat capacity = 0.130 J/g °C) is heated using 55.8 J of energy. If
the original temperature of the gold is 25.0°C, what is its final temperature?
(A) 88.6 °C (B) 38.6 °C (C) 76.9 °C (D)73.6 °C (E) 63.6 °C

24. For the reaction \[ \text{H}_2(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{H}_2\text{O}(l) \quad \Delta H = -286 \text{ kJ/mol} \] Calculate the enthalpy change when 2.80 g of water is produced. (A) 102 kJ (B) 801 kJ (C) -801 kJ (D) 44.4 kJ (E) -44.4 kJ

25. ____ is the ability to do work or produce heat.
(A) Gravity (B) Temperature (C) Radiation (D) Matter (E) Energy

26. ____ is a measure of disorder or randomness.
(A) Entropy (B) Enthalpy (C) Calorimetry (D) Internal energy (E)Hess's law

27. The probability map for an electron is called
(A) an orbit (B) a photon (C) an orbital
(D) an electron configuration (E) none of these

28. A d sublevel can hold a maximum of
(A) 5 electrons (B) 10 electrons (C) 14 electrons
(D) 32 electrons (E) none of these

29. The electron configuration for the sulfur atom is (A) \( 1s^22s^22p^63s^23p^4 \) (B) \( 1s^22s^22p^63s^23p^6 \) (C) \( 1s^22s^22p^63s^23p^2 \) (D) \( 1s^22s^22p^63s^6 \) (E) none of these

30. Which element has the fewest electrons in its valence shell?
(A) Cs (B) Mg (C) P (D) O (E) Br

31. What element has the electron configuration 1s²2s²2p⁶3s²3p⁶? (A) Ar (B) Cl (C) Kr (D) S (E) none of these

32. Which of the following atoms has the highest ionization energy?
(A) F (B) Be (C) N (D) C (E) Li

33. One of the most important characteristics of the water molecule is its __________, which allows it to surround and attract both positive and negative ions.
(A) polarity (B) strength (C) magnetism (D) fluidity (E) stability

34. Magnesium reacts with oxygen to form (A) MgO (B) Mg₂O (C) Mg₂O (D) Mg₂O₃ (E) none of these

35. How many of the following will have Lewis structures with multiple bonds? CO, CO₂, CO₃^2-, N₂, O₂ (A) 1 (B) 2 (C) 3 (D) 4 (E) 5

36. You are playing with a helium balloon on a typically warm California day. Suddenly, the Celsius
temperature doubles. Which of the following is true?
(A) The volume of the balloon will double.
(B) The volume of the balloon will slightly increase.
(C) The pressure inside the balloon will double.
(D) The volume of the balloon will decrease.
(E) The actual temperatures are needed to answer this question.

37. What is the volume of a helium balloon that contains 1.95 mol helium at 27°C and 1.10 atm?
(A) 3.93 L (B) 39.7 L (C) 48.0 L (D) 43.6 L (E) 4.32 L

38. Which conditions of P and T are most ideal for a gas?
(A) high P, high T (B) high P, low T (C) low P, high T
(D) low P, low T (E) depends on the gas

39. Which of the following has the lowest vapor pressure? (A) H₂O (B) NaCl (C) NH₃ (D) O₂ (E) CH₄

40. The total mass of a solution is 184.8 g. The solvent mass is 125.2 g. What is the mass percent of
the solute?
(A) 32.3 % (B) Not enough information is given. (C) 43.3 %
(D) 21.6 % (E) 67.7 %

41. You have 25.00 mL of a 0.1000 M sugar solution. How much water must be added to make a
0.01809M solution?
(A) 138.2 mL (B) 4.52 mL (C) 20.5 mL (D) 113.2 mL (E) 45.2 mL

42. How many grams of NaCl are contained in 350. mL of a 0.238 M solution of sodium chloride?
(A) 83.3 g (B) 4.87 g (C) 13.9 g (D) 1.43 g (E) none of these

43. What volume of 18.0 M sulfuric acid is required to prepare 26.2 L of 0.126 M H₂SO₄? (A) 5.45 mL. (B) 0.183 L. (C) 472 mL. (D) 3.30 L. (E) 208 mL.

44. Choose the case that is not a Bronsted conjugate acid-base pair. (A) CH₃NH₃⁺, CH₃NH₂ (B) HCN, CN^- (C) HClO₂, ClO₂^- (D) HCO₂H, HCO₂^- (E) H₃BO₃, H₂BO₃^-

45. A solution has [OH^-] = 3.0x10^-7 M. The [H⁺] in this solution is (A) 1.0 M (B) 3.0 x 10^-7 M (C) 1.0 x 10^-7 M (D) 3.3 x 10^-8 M (E) none of these

46. What is the pH of a 2.1 M solution of HNO3?
(A) –0.32 (B) 0.32 (C) 14.32 (D) 13.68 (E) none of these

47. Given the reaction \( A(g) + B(g) \rightleftharpoons C(g) + D(g) \). You have the gases A, B, C, and D at equilibrium. Upon adding gas A, the value of K (A) increases because when A is added, more products are made, increasing the product-to-reactant ratio (B) decreases because A is a reactant, so the product-to-reactant ratio decreases (C) does not change because A does not figure into the product-to-reactant ratio (D) does not change as long as the temperature is constant (E) depends on whether the reaction is endothermic or exothermic

48. Given the equation A(g) $\rightleftharpoons$ B(g) + 2C(g). At a particular temperature, $K = 1.3 \times 10^5$. If you mixed 1.4 mol B, 0.050 mol C, and 0.0050 mol A in a 1-liter container, in which direction would the reaction initially proceed? (A) The reaction will proceed to the right. (B) The reaction will proceed to the left. (C) The mixture is at equilibrium. (D) More information is needed to answer the question.

49. The solubility of Mg(OH)₂(s) in water at a certain temperature is 1.1x10^-4 mol/L. Calculate the value of K_sp for Mg(OH)₂(s) at this temperature. (A) 1.1 x 10^-4 (B) 1.3 x 10^-12 (C) 1.2 x 10^-8 (D) 5.3 x 10^-12 (E) none of these

50. The oxidation state of phosphorus in Mg₃(PO₄)₂ is (A) 0 (B) +2 (C) +4 (D) +5 (E) +6