Chemistry I SOL Practice Test — Set 3 of 6
Set 3 of 6 — 50 more free Chemistry I SOL practice questions from official VDOE released tests.
1. 2Al(C₂H₃O₂)₃ + 3BaSO₄ → Al₂(SO₄)₃ + 3Ba(C₂H₃O₂)₂ Which type of chemical reaction does this equation represent?
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Answer: D — Double-replacement
2. What is the molarity of a solution with 0.2 moles of potassium permanganate (KMnO₄) dissolved in enough water to make a 500.0 mL solution?
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Answer: C — 0.4 M
3. When 92.0 g of ethanol (C₂H₅OH) are vaporized at its boiling point of 78.3°C, it requires 78.6 kJ of energy. What is the approximate molar heat of vaporization of ethanol in kJ/mol?
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Answer: C — 39.3
4. Which element has 16 neutrons, 15 protons, and 15 electrons?
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Answer: B — Phosphorus (P)
5. Al(s) + 3AgNO₃(aq) → Al(NO₃)₃(aq) + 3Ag(s) This equation represents which type of chemical reaction?
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Answer: A — Single-replacement
6. In the formula for barium chloride (BaCl₂), barium (Ba) is written first because it is —
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Answer: C — the positive ion
7. Which laboratory technique is best to separate a solid from a liquid in order to recover the liquid?
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Answer: C — Filtering
8. Which of these is NOT required to ensure that stock solutions are free of contamination?
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Answer: A — Store all solutions in brown bottles
9. Which value is most responsible for changing the boiling and freezing points of a solvent?
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Answer: D — Number of the solute particles
10. What is the name of the compound with the formula NH₄NO₃?
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Answer: A — Ammonium nitrate
11. N₂(g) + 3F₂(g) ⇌ 2NF₃(g) Equilibrium has been reached for the reaction shown. Which conclusion is correct?
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Answer: B — The partial pressures of N₂, F₂, and NF₃ will stay constant.
12. If 89.6 joules of heat are needed to heat 20.0 g of iron from 30.0°C to 40.0°C, what is the specific heat of iron in J/(g·°C)?
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Answer: A — 0.448
13. A pH scale shows the following substances at these approximate pH values: Calcium hydroxide: pH 12–13 Human blood: pH 7–8 Whole milk: pH 6 Lemon juice: pH 2 Which of these substances is slightly basic?
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Answer: B — Human blood
14. Which element will most likely form covalent bonds with fluorine?
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Answer: A — Carbon
15. The physical process of evaporation involves —
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Answer: D — overcoming intermolecular forces
16. __C₂H₆ + __O₂ → __CO₂ + __H₂O How many moles of O₂ are required when this equation is balanced using the lowest whole-number coefficients?
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Answer: C — 7
17. While English physicist J. J. Thomson was carrying out experiments on cathode rays, he determined that the rays consisted of particles he called “corpuscles.” These particles were later named —
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Answer: B — electrons
18. In the Haber process, nitrogen (N₂) and hydrogen (H₂) react to form ammonia (NH₃). The balanced equation is: N₂ + 3H₂ → 2NH₃ Which set of reactant particles represents the correct stoichiometric ratio for this reaction?
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Answer: B — 1 molecule of N₂ and 3 molecules of H₂
19. A beaker of water is placed in a sealed container connected to a vacuum pump. As air is removed from the container, the water begins to boil. This occurs because —
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Answer: C — the air pressure is lowered until it equals the vapor pressure of the water
20. According to the periodic table, which elements belong to the same period?
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Answer: B — Gallium, Germanium, Arsenic
21. How many moles are in 2.04 × 10²⁴ molecules of H₂O?
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Answer: B — 3.39 mol
22. What is the correct IUPAC name for FeCl₃?
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Answer: D — Iron(III) chloride
23. Which statement correctly describes how organic catalysts operate in biological reactions?
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Answer: C — They lower the activation energy of the reactions.
24. What volume will 35.9 g of hydrogen gas (H₂) occupy at STP?
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Answer: A — 399 L
25. __Ca(NO₃)₂ + __H₃PO₄ → __Ca₃(PO₄)₂ + __HNO₃ When this equation is balanced, what is the coefficient in front of H₃PO₄?
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Answer: B — 2
26. Increasing the volume of a sealed container will cause the gas particles inside to —
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Answer: D — exert lower pressure
27. Consider any set of three adjacent elements in the same period of the periodic table. For which characteristic is the average of the three elements always equal to the value of the middle element?
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Answer: A — Atomic number
28. A substance has a molecular formula of C₆H₁₂N₂O₂. What is its empirical formula?
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Answer: B — C₃H₆NO
29. What is the correct name for AlI₃?
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Answer: D — Aluminum iodide
30. 2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O How many moles of carbon dioxide are produced when 6.00 moles of butane react with excess oxygen?
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Answer: B — 24.0 mol
31. Using only one trial to collect data in an experiment —
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Answer: C — causes the conclusion to be less reliable
32. A common product of acid–base neutralization reactions is —
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Answer: B — water
33. A data table compares the brightness of a light bulb when connected to different aqueous solutions. Which solution is a base and a weak electrolyte?
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Answer: D — CH₃NH₂
34. A graph shows the beta decay of Americium-242. The y-axis represents mass remaining, and the x-axis represents time in hours. The mass decreases by half every 16 hours. What is the half-life of Americium-242?
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Answer: B — 16 hours
35. In a Lewis structure of Br₂, two electrons are shared equally between the two bromine atoms. What type of bond exists between the bromine atoms?
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Answer: A — Nonpolar covalent bond
36. A student studies how different solutions affect the browning of apple slices. The student varies the pH of the solutions, immerses three apple slices in equal volumes of each solution, and observes the color change. What is the independent variable?
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Answer: A — pH of the solution
37. An experiment produced 0.10 g of CO₂ with a volume of 0.056 L at STP. If the accepted density of CO₂ at STP is 1.96 g/L, what is the approximate percent error?
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Answer: D — 8.2%
38. The following data are obtained in the laboratory: (a) The mass of a clean, dry 250 mL beaker (b) The mass of the same beaker containing an unknown quantity of magnesium sulfate The mass of the magnesium sulfate is obtained by subtracting (a) from (b). Which of the following will provide the most accurate results?
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Answer: A — Measurements should be taken using the same balance.
39. Many reactions are taken to completion by heating the reaction mixture in a test tube. Each of the following would be a safe practice except—
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Answer: H — placing a stopper in the test tube to prevent gas from escaping
40. A student recorded the following data while studying the effect of volume on gas pressure. Temperature remained constant at 298 K. Trial 1: Volume 100 mL, Pressure 250 mmHg Trial 2: Volume 300 mL, Pressure 83 mmHg Trial 3: Volume 500 mL, Pressure 50 mmHg How could the student now study the effects of temperature on gas pressure?
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Answer: A — Vary the temperature but keep the gas volume constant.
41. A graph shows the solubility of four salts in water (measured in grams of solute per 100 grams of water) over a temperature range from 0 °C to 120 °C. • Sodium chloride (NaCl) shows very little change in solubility across the temperature range. • Potassium nitrate (KNO₃), potassium bromide (KBr), and sodium chlorate (NaClO₃) all show significant increases in solubility as temperature increases. Which salt’s solubility in water is least affected by temperature?
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Answer: J — NaCl
42. A student studied the effect of temperature on the reaction A + B → AB using a catalyst. Experimental conditions were: Trial 1: 17 °C, 1 mg catalyst, 5 g A, 7 g B, reaction time 10 min Trial 2: 18 °C, 2 mg catalyst, 5 g A, 7 g B, reaction time 8 min Trial 3: 20 °C, 3 mg catalyst, 5 g A, 7 g B, reaction time 5 min Trial 4: 16 °C, 4 mg catalyst, 5 g A, 7 g B, reaction time 3 min Which of the following would improve the student’s experimental design?
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Answer: A — Use the same amount of catalyst in all trials.
43. A student massed a piece of iron on a balance marked in 0.1 g intervals and reported the mass as 12.34 g. Which digit in this measurement is estimated?
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Answer: J — 4
44. A student measured the temperature of a boiling solution and found it to be 56.0 °C at standard pressure. The theoretical boiling temperature is 55.0 °C. What is the percent error?
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Answer: B — 1.8%
45. How many significant digits are in 0.003450?
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Answer: G — 4
46. A 0.500 L solution of 6 M HCl is to be prepared. How much 12 M HCl is required?
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Answer: A — 0.250 L
47. Two substances have the following compositions: Substance A: 8 protons, 8 neutrons, 8 electrons Substance B: 8 protons, 9 neutrons, 8 electrons The data indicate that—
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Answer: A — A and B are isotopes of the same element.
48. A neutral atom of calcium has 20 electrons. Calcium forms a 2+ ion. How many electrons does a calcium ion have?
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Answer: G — 18
49. According to their placement on the periodic table, which elements would have the most similar atomic structures?
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Answer: C — Sodium and potassium
50. Oxygen and sulfur are in the same group (Group 16) in the periodic table. This means that, in general, oxygen and sulfur—
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Answer: G — undergo similar reactions with other elements
Chemistry I SOL practice test — FAQ
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How many Chemistry I SOL practice questions are there?
Across all sets, there are 278 Chemistry I practice questions drawn from official Virginia Department of Education released SOL tests. This set has 50.
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The questions are adapted from official VDOE released SOL tests for Chemistry I. SOL Prep is an independent study aid and is not affiliated with or endorsed by the Virginia Department of Education.
Practice items adapted from Virginia Department of Education released SOL tests. Practice items are provided for study purposes and are not affiliated with or endorsed by the Virginia Department of Education.