CLEP Chemistry: Study Guide & Test Prep Final Exam

Exam Instructions:

Choose your answers to the questions and click 'Next' to see the next set of questions. You can skip questions if you would like and come back to them later with the yellow "Go To First Skipped Question" button. When you have completed the practice exam, a green submit button will appear. Click it to see your results. Good luck!

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Question 1 1. Ammonia is made by the Haber Process according to the following chemical reaction: N2 (g) + 3H3 (g) ↔ 2NH3 (g). If ΔH = -92.4 kJ/mol, what affect will lowering the temperature have on the reaction at equilibrium?

Question 2 2. Which of the elements forms monoatomic ions with +1 charge in solutions?

Question 3 3. Which of the following contains the strongest polar covalent bond?

Question 4 4. What type of intermolecular force can affect noble gases?

Question 5 5. What is the oxidation number of iodine in Zn(IO3)2?

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Question 6 6. The pH of 0.1 M nitric acid is approximately

Question 7 7. A precipitate is formed when Na2SO4 is added to an aqueous solution. Which of the following ions is likely in the solution?

Question 8 8. What is the molar mass of a gas that has a density of 5.00 g/L at 2.00 atm of pressure and 100.°C? (R = 0.0821 L*atm/mol*K).

Question 9 9. The reaction A + 2B → C has the following experimental rate law at 25°C: rate = k[A][B]2. What effect will a two-fold increase in the rate of B have on the rate of the reaction?

Question 10 10. The electron configuration of an element, X, is 1s2 2s2 2p6 3s2 3p1. The most likely compound for form with S is

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Question 11 11. A student wants to make 5.00 L of 0.450 M Na2SO4. To do this, the student should weigh out

Question 12 12. At what point on a phase diagram do solid, liquid, and gas states of of a substance exist in equilibrium?

Question 13 13. For an exothermic reaction, which of the following always results in a spontaneous reaction?

Question 14 14. A student mixes 100. mL of 0.100 M NaOH with 100. mL of 0.200 M MgCl2. Following the reaction, what concentration of magnesium ions will be in solution?

Question 15 15. Which of the following best describes the molecular geometry of XeF4?

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Question 16 16. What does a positive cell potential tell you?

Question 17 17. When working with free energy, standard conditions are defined as which of the following?

Question 18 18. When writing electron configurations, electrons are represented in their lowest possible energy state, called their _____.

Question 19 19. What is the correct electron configuration for an atom of sodium (Na)?

Question 20 20. Which of the following is NOT a common property of acids?

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Question 21 21. According to Bronsted and Lowry, what is a base?

Question 22 22. Why are there plateaus on a heating curve?

Question 23 23. Which of the following statements is true about a heating curve?

Question 24 24. When neptunium-238 decays, it emits two alpha particles, a beta particle, and a gamma particle. The resulting isotope is:

Question 25 25. Becky was recently diagnosed with an aggressive brain tumor. Her oncologist recommended treating the tumor with cobalt-60 due to its precision with treating this type of cancer. This substance is being used for _____.

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Question 26 26. Which of the following elements has the same number of valence electrons as aluminum?

Question 27 27. Which of the elements below has the highest ionization energy?

Question 28 28. Identify the requirement for a dipole-dipole force to exist.

Question 29 29. Why are metals malleable?

Question 30 30. The ability of a solid to be dissolved in a given volume of a solvent at a given temperature is known as _____.

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Question 31 31. In general, what do Ksp values tell us about the solubility of a compound under the designated conditions?

Question 32 32. What is the density of a solid that has a mass of 9.2 grams and a volume of 12.3 cm^3? Would this object float or sink in water?

Question 33 33. How many millimeters (mm) are there in 5 meters (m)?

Question 34 34. What is the equation used to determine the mass percent of a solute in a solution?

Question 35 35. Which of the following is true about Raoult's Law?

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Question 36 36. The rate of a given chemical reaction is the

Question 37 37. The minimum amount of energy required to convert reactants to products is called

Question 38 38. Convert 20 degrees Celsius to degree Fahrenheit.

Question 39 39. What is the original form of the ideal gas equation?

Question 40 40. 3.9g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. Calculate the mass of potassium hydroxide produced.

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Question 41 41. Which of the following could be an empirical formula?

Question 42 42. A reaction will release heat when:

Question 43 43. A piece of copper wire contains 5 moles of copper atoms. What is its mass?

Question 44 44. Which of the following equations is exothermic?

Question 45 45. What is NOT something that a phase equilibrium line shows?

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Question 46 46. A 6.95 gram sample of radioactive nobelium-259 has a half-life of 58 min. How much is left after 2 hours and 54 minutes?

Question 47 47. As you move from top to bottom on the periodic table, what happens to the atomic radius?

Question 48 48. How many dots would you put around carbon, a group IVA element?

Question 49 49. What is the net effect of the common ion?

Question 50 50. _____ properties of matter can be determined without changing composition, while _____ properties of matter must change the composition of matter.

CLEP Chemistry: Study Guide & Test Prep Final Exam Instructions

Choose your answers to the questions and click 'Next' to see the next question. You can skip questions if you would like and come back to them later with the "Go To First Skipped Question" button. When you have completed the practice exam, a green submit button will appear. Click it to see your results. You will lose your work if you close or refresh this page. Good luck!

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