112年 - 112 台北市立陽明高級中學教師甄試化學科試題#119137

7. Which shows the number of subatomic particles in ³¹P³⁻ ?  (A)(B)(C)(D) 

12. Two 100 cm³ aqueous solutions, one containing 0.010 mol NaOH and the other 0.010 mol HCl, are at the same temperature. When the two solutions are mixed the temperature rises by y °C. Assume the density of the final solution is 1.00 g cm⁻³. Specific heat capacity of water = 4.18 J g⁻¹ K⁻¹ What is the enthalpy change of neutralization in kJ mol−1? (A) (B) (C) (D)

16. Activity series of selected elements: least activity
 Which react with dilute sulfuric acid?

I. Cu
II. CuO
III. CuCO₃ (A) I and II only (B) I and III only (C) II and III only (D) I, II and III

19. Which increase across a period from left to right? (A)(B)(C)(D)

15. The potential energy profile for the reversible reaction, X + Y ⇌ Z is shown.

Which arrow represents the activation energy for the reverse reaction, Z → X + Y, with a catalyst?

21a. Calculate the percentage by mass of nitrogen in urea to two decimal places using the data in the appendix. [1 marks]

21b. The structural formula of urea is shown. 

Predict the electron domain and molecular geometries at the nitrogen and carbon atoms, applying the VSEPR theory. [3 marks]

21d. Sketch two different hydrogen bonding interactions between ammonia and water. [2 marks]

21e. The combustion of urea produces water, carbon dioxide and nitrogen. Formulate a balanced equation for the reaction. [2 marks]

21f. The IR spectrum of urea is shown below. Identify the bonds causing the absorptions at 3450 cm^–1 and 1700 cm^–1 using the data in the appendix. [2 marks]

21g. The mass spectrum of urea is shown below. Identify the species responsible for the peaks at the mass/charge ratio (m/z) equal to 60 and 44. [2 marks]

21h. Predict the number of signals in the H NMR 1 spectrum of urea. [1 marks]

22a. Outline two ways in which the progress of the reaction can be monitored. No practical details are required. [2 marks]

22b. The results of a series of experiments in which the concentration of HCl was varied are shown below. Suggest why point D is so far out of line assuming human error is not the cause. [1 mark]

22c. Suggest the relationship that points A, B and C (in 22b) show between the concentration of the acid and the rate of reaction. [1 mark]

23a. The antacid tablet was added to 50.00 cm³ of 0.100 mol dm⁻³ sulfuric acid, which was in excess. Calculate the amount, in mol, of H₂SO₄. [1 mark]

23b. The excess sulfuric acid required 20.80 cm3 of 0.1133 mol dm⁻³ NaOH for neutralization. Calculate the amount of excess acid present. [1 mark]

23c. Calculate the amount of H₂SO₄ that reacted with Mg(OH)₂. [1 mark]

23d. Determine the mass of Mg(OH)₂ in the antacid tablet. [1 marks]

23e. Calculate the percentage by mass of magnesium hydroxide in the 1.24 g antacid tablet to three significant figures. [1 mark]

24b. Deduce the half-equations for the reaction at each electrode when current flows. [2 marks]

25a. Ethyne, like ethene, undergoes hydrogenation to form ethane. State the conditions required. [2 marks]

25b. Outline the formation of polyethene from ethene by drawing three repeating units of the polymer. [1 mark

25d. Determine the standard enthalpy change, ΔH^Θ , for the following similar reaction, using ΔHf values in the appendix. [2 marks] 

3C₂H₂(g) → C₆H₆(l)

25e. Explain, giving two reasons, the difference in the values for 25c and 25d. If you did not obtain answers, use −475 kJ for 25c and −600 kJ for 25d. [1 marks]

25f. One possible Lewis structure for benzene is shown. 

State one piece of physical evidence that this structure is incorrect. [1 mark]

26a. Sketch a Maxwell–Boltzmann distribution curve for a chemical reaction showing the activation energies with and without a catalyst. [3 marks]

26b. Excess hydrochloric acid is added to lumps of calcium carbonate. The graph shows the volume of carbon dioxide gas produced over time.

Sketch a curve on the graph to show the volume of gas produced over time if the same mass of crushed calcium carbonate is used instead of lumps. All other conditions remain constant. [1 mark]

26c. State and explain the effect on the rate of reaction if ethanoic acid of the same concentration is used in place of hydrochloric acid. [2 marks]

26d. Outline why pH is more widely used than [H+ ] for measuring relative acidity. [1 mark]

27a. Draw the first four energy levels of a hydrogen atom on the axis, labelling n = 1, 2, 3 and 4. Draw the arrows, on your diagram, that represent the electron transitions to n = 2 in the emission spectrum. [2 marks]

27b. Elements show trends in their physical properties across the periodic table. Outline why atomic radius decreases across period 3, sodium to chlorine. [1 mark]

27c. Outline why the ionic radius of K+ is smaller than that of Cl⁻ . [2 marks]

27d. Copper is widely used as an electrical conductor. Draw arrows in the boxes to represent the electronic configuration of copper in the 4s and 3d orbitals. [1 mark]

27e. Impure copper can be purified by electrolysis. In the electrolytic cell, impure copper is the anode (positive electrode), pure copper is the cathode (negative electrode) and the electrolyte is copper(II) sulfate solution. Formulate the half-equation at each electrode. [2 marks]

28a. Distinguish between the terms reaction quotient, Q, and equilibrium constant, KC.[1 mark]

28b. The equilibrium constant, K_C, is 0.282 at temperature T. Deduce, showing your work, the direction of the initial reaction. [2 marks]

29a. Explain why the hydrides of group 16 elements (H₂O, H₂S, H₂Se and H₂Te) are polar molecules. [2 marks]

29b. The graph shows the boiling points of the hydrides of group 16 elements. Explain the increase in the boiling point from H₂S to H₂Te. [2 marks]

30a. According to the data of No.2 in table 1, determine the mass of CO₂, i.e. (IV), in g. [1 mark]

30b. According to the data of No.2 in table 1, determine the molecular mass, in g mol⁻¹ , using the ideal gas equation. [2 marks]

30c. The molecular mass determined by the ideal gas equation is quite different from the molecular mass of CO₂, 44 g mol⁻¹ . Explain the reason that causes the difference. [1 marks]

31b. Assume the reaction in (a) is the only one occurring and it goes to completion, but some product has been lost from the crucible. Deduce the percentage yield of magnesium oxide in the crucible. [1 mark]