Chemistry quiz easy, homework help

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Name _________________________________ I.D. Number _______________________ Unit 2 Evaluation Evaluation 02 Chemistry 2 (SCIH 032 062) This evaluation will cover the lessons in this unit. It is open book, meaning you can use your textbook, syllabus, and other course materials. You will need to understand, analyze, and apply the information you have learned in order to answer the questions correctly. To submit the evaluation, follow the directions provided. Matching Match each of the following terms to its correct definition. a. calorimeter b. calorie c. joule d. enthalpy e. specific heat _____ 1. quantity of heat needed to raise the temperature of 1 g of water by 1°C _____ 2. SI unit of energy _____ 3. quantity of heat needed to change the temperature of 1 g of a substance by 1°C _____ 4. device used to measure the heat absorbed or released during a chemical or physical process _____ 5. heat content of a system a. heat of reaction b. heat of formation c. Hess’s law of heat summation d. heat of fusion e. heat of solution _____ 6. the enthalpy change for a chemical reaction Unit 2 Evaluation 73 SCIH 032 _____ 7. the enthalpy change caused by dissolving a substance _____ 8. the energy required to melt a solid at its melting point _____ 9. the change in enthalpy that accompanies making a compound from its elements _____ 10. if you add two or more thermochemical equations to give a final equation, you can also add the heats of reaction to give the final heat of reaction Multiple-Choice Select the response that best completes the statement or answers the question. _____ 11. _________ is the quantity of heat needed to change the temperature of an object by 1°C. a. b. c. d. _____ 12. Specific heat Heat capacity Enthalpy Calorimetry During an endothermic chemical reaction, what is the source of energy that causes the reaction to continue? a. b. c. d. _____ 13. How do calories and joules differ from one another? a. b. c. d. _____ 14. materials that are part of the system reactants involved in the reaction chemical bonds of the reaction products materials in the surroundings of the system They are two different measures of amounts of energy. Calories measure energy and joules measure heat flow. Joules are used in chemistry and calories are used in biology. Joule and calorie are two different names for the same unit of energy. Which statement correctly describes the energy of the chemical bonds of the reactants in an exothermic reaction? a. b. c. d. Unit 2 Evaluation equal to the energy stored in the bonds of the products greater than the energy stored in the bonds of the products less than the energy stored in the bonds of the products independent of the energy stored in the bonds of the products 74 SCIH 032 _____ 15. What is the amount of heat required to raise the temperature of 200.0 g of aluminum by 10°C? (specific heat of aluminum = 0.21 cal/(g x °C) a. b. c. d. _____ 16. 420 cal 4200 cal 42,000 cal 420,000 cal A 100-gram piece of heated iron cools from 50° to 20°C. How much heat is released to the surroundings? a. b. c. d. _____ 17. 300 J of heat are released to the surroundings. 300 cal of heat are released to the surroundings. The amount of heat cannot be calculated because the heat capacity is not known. The amount of heat cannot be calculated because there is no closed system. How much ice at 0°C could be melted by the addition of 15 kJ of heat? (Hfus = 6.01kJ/mol) a. b. c. d. _____ 18. Which of the following substances has the highest specific heat? a. b. c. d. _____ 19. steel liquid water mercury ice What are the standard conditions for determining heat of formation? a. b. c. d. _____ 20. 0.4 g 2.5 g 7.2 g 45 g 0°C and 101 kPa 25°C and 101 kPa 0°C and 0 kPa 25°C and 22.4 kPa How much water at 100°C could be vaporized by the addition of 120 kJ of heat? (Hvap = 40.7 kJ/mol) a. b. c. d. Unit 2 Evaluation 2.9 g 6.1 g 53 g 87 g 75 SCIH 032 _____ 21. Calculate the energy released when 24.8 g Na2O reacts in the following reaction. Na2O(s) + 2HI(g)  2NaI(s) + H2O(l) ΔH = –120.00 kcal a. b. c. d. _____ 22. 0.207 kcal 2.42 kcal 48.0 kcal 3.0010 kcal The amount of heat needed to melt one mole of a solid at a constant temperature is called _________. a. b. c. d. _____ 23. What is the heat of solution? a. b. c. d. _____ 24. It is always negative. It is always positive. It can be positive or negative. It is always equal to zero. The symbol ΔHf° represents _________. a. b. c. d. _____ 26. The amount of heat required to change a solid into a liquid. The amount of heat absorbed or released when a solid dissolves. The amount of heat required to change a vapor into a liquid. The amount of heat released when a vapor changes into a liquid. By definitions which of the following is true of ΔH? a. b. c. d. _____ 25. molar heat of fusion molar heat of solidification heat of reaction enthalpy of fusion specific heat of a substance heat capacity of a substance heat of reaction for a chemical reaction standard heat of formation for a compound ΔH for the formation of rust (Fe2O3) is -826 kJ/mol. How much energy is released in the formation of 5 grams of rust? a. b. c. d. Unit 2 Evaluation -25.9 kJ 25.9 J -66 kJ 66 J 76 SCIH 032 Matching Match each of the following terms to its correct definition. a. activated complex b. reaction rate c. inhibitor d. activation energy e. free energy _____ 27. the minimum energy colliding particles must have in order to react _____ 28. arrangement of atoms at the peak of an energy barrier _____ 29. the number of atoms, ions, or molecules that react in a given time to form products _____ 30. a substance that interferes with a catalyst _____ 31. energy available to do work a. spontaneous reaction b. entropy c. chemical equilibrium d. reaction mechanism e. elementary reaction _____ 32. when the forward and reverse reactions take place at the same rate _____ 33. a reaction that releases free energy _____ 34. the measure of disorder _____ 35. reactants are converted to products in a single step _____ 36. includes all elementary reactions of a complex reaction Unit 2 Evaluation 77 SCIH 032 Multiple-Choice Select the response that best completes the statement or answers the question. _____ 37. Why does a higher temperature cause a reaction to go faster? a. b. c. d. _____ 38. Why does a higher concentration make a reaction faster? a. b. c. d. _____ 39. Collisions between molecules occur more slowly so there is more time to react. Collisions are not as frequent but each collision has more energy. Collisions occur more frequently and they occur with greater energy. Collisions have less energy so molecules are less likely to bounce away from one another. Higher concentration increases the frequency of collisions. Higher concentration increases the total energy of collisions. Higher concentration decreases the activation energy of the overall reaction. Higher concentration decreases the energy needed for a collision to be effective. Which expression shows the solubility product constant for silver (I) sulfide, Ag2S, which is very slightly soluble in water? a. b. c. d. _____ 40. Ksp = [Ag+][S2-] Ksp = 2[Ag+][S2-] Ksp = [Ag+]2[S2-] Ksp = [Ag2S] If sulfur dioxide and oxygen can be made into sulfur trioxide, what is the reverse reaction? a. b. c. d. _____ 41. 2SO3  2SO2 + O2 SO2 + O2  SO3 2SO2 + O2  2SO3 SO2 + 2SO3  3S + 4O2 Consider the reaction N2(g) + 3H2(g)  2NH3(g). What is the effect of decreasing the volume on the contained gases? a. b. c. d. _____ 42. The reaction shifts toward the product gas. The system reacts by increasing the number of gas molecules. The pressure on the gases decreases momentarily. Ammonia is consumed in the reaction. If a reaction has an equilibrium constant just greater than 1, what type of reaction is it? a. b. c. d. Unit 2 Evaluation irreversible spontaneous reversible, favoring products reversible, favoring reactants 78 SCIH 032 _____ 43. The Ksp of nickel sulfide (NiS) is 4.0 x 10-20. What is the concentration of sulfide ion in a saturated solution of nickel sulfide to which 0.040 mol of nickel nitrate (NiNO3) is added? a. b. c. d. _____ 44. Which reaction results in the greatest increase in entropy? a. b. c. d. _____ 45. 2.0 x10-10 M 1.0 x10-18 M 1.0 x 10-22 M 1.6 x 10-22 M AB A  2B 2A  B 3A  B When a student in a chemistry lab combines two clear solutions a precipitate forms. What conclusion can the student make about the combined solution? a. The value of Ksp for the compound formed by the combination of two ions is less than 1. b. The value of Ksp for the compound formed by the combination of two ions is greater than 1. c. The concentration of one of the ions in solution exceeded the Ksp for that ion in water. d. The product of the concentrations of two ions exceeded the Ksp for the compound formed by the ions. _____ 46. The two factors that determine whether a reaction is spontaneous or nonspontaneous are _________. a. b. c. d. _____ 47. entropy and disorder entropy and energy electron configuration and ionic charge energy and heat of reaction In a first-order reaction, how does the rate change if the concentration of the reactant decreases to one-third its original value? a. b. c. d. Unit 2 Evaluation The rate decreases by a factor of one-ninth. The rate decreases by a factor of one-third. The rate decreases by a factor of one-half. The rate stays the same. 79 SCIH 032 _____ 48. When nitrous oxide is converted to nitrogen and oxygen, what is the term used to describe the oxygen atoms formed? a. b. c. d. _____ 49. At what stage of a chemical reaction is chemical energy at its highest level? a. b. c. d. _____ 50. reactants products activated complexes intermediates when only reactants are present when only products are present when an activated complex exists when the activated complex becomes a product Which of these conditions describes a situation in which a reaction must be nonspontaneous? a. b. c. d. enthalpy decreases and entropy decreases enthalpy decreases and entropy increases enthalpy increases and entropy decreases enthalpy increases and entropy increases Carefully check your answers on this evaluation and make any corrections you feel are necessary. When you are satisfied that you have answered the questions to the best of your ability, transfer your answers to an answer sheet. Please refer to the information sheet that came with your course materials. Unit 2 Evaluation 80 SCIH 032
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Explanation & Answer

Here are the answers, please tell me if you have any problem.

1.
2.
3.
4.
5.

b.
c.
e.
a.
d.

calorie
joule
specific heat
calorimeter
enthalpy

6. a. heat of reaction
7. e. heat of solution
8. d. heat of fusion
9. b. heat of formation
10. c. Hess’s law of heat summation

11. b. Heat capacity
12. d. materials in the surroundings of the system
13. a. They are two different measures of amounts of energy.
14. b. greater than the energy stored in the bonds of the products
15. a. 420 cal
16. c. The amount of heat cannot be calculated because the heat capacity is
not known.
17. d. 45 g
18. b. liquid water
19. b. 25°C and 101 kPa
20. c. 53 g
21. c. 48.0 kcal
22. a. mo...


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