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Newest Thermodynamics Questions

1. Which event is an example of an exothermic reaction?(1 point)Responses combustion combustion evaporation evaporation melting ice
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   2. asked by nuh uhhhhhhhh
   3. 32 views
2. Use the table to answer the question.Reaction Bonds Present Energy of Bonds Broken and Formed (kJ/mol) C + O2→CO2 O=O 2 C=O
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   2. asked by nuh uhhhhhhhh
   3. 27 views
3. When producing hydrogen iodide, the energy of the reactants is 581 kJ/mol, and the energy of the products is 590 kJ/mol. The
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   2. asked by nuh uhhhhhhhh
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4. Use the table below to calculate the change in enthalpy (bond energy) for the reaction above.Bond Type Bond Energy kJ/mol
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5. Determine if the following scenarios are part of an open or closed system, in terms of Chemistry.1. During combustion, fuel and
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   2. asked by 1131207
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6. 25 (s) * 30, (g) - 250g (a) Дн = -790 kJ5 (s) + O2 (9) - 50,(0) 4н = 297 kJ the enthalpy of the reaction in which sufur
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7. Which fact must be true if a relationship is endothermic?(1 point)The bond energy released by breaking the bonds in the
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8. Given the following reaction:2NH₃ → N₂ + 3 H₂ If the total bond energy absorbed by the reactant , NH₃, is 2316 KJ/mol
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9. What is the enthalpy change for the forward reaction 4 (8N₂O + 4CS₂ → S₈ + 4CO₂ + 8N₂), and is it endothermic or
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   2. asked by 124u821498142942
   3. 16 views
10. When producing hydrogen iodide, the energy of the reactants is 581 kJ/mol, and the energy of the products is 590 kJ/mol. The
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11. Which event is an example of an exothermic reaction?a melting ice b decomposition c combustion d evaporation
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12. Use the table to answer the question.Reaction CH4 + 4Cl2 → CCl4 + 4HCl Reactants Products Bonds Present 4 H–C 4 Cl–Cl 4
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13. Use the information in the table to answer the question.Bond Bond Energy ( kJ/mol ) H-I 297 H-H 435 I-I 151 Hydrogen and iodine
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14. When producing hydrogen iodide, the energy of the reactants is 581 kJ/mol, and the energy of the products is 590 kJ/mol. The
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15. H2 + I2 ------> 2HIWhat is the total energy of the reaction? Is this an endothermic or exothermic reaction? 9 KJ/mol endothermic
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16. Hydrogen bromide breaks down into diatomic hydrogen and bromine in the reaction shown.2HBr → H2 + Br2 The energy of the
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17. Hydrogen bromide breaks down into diatomic hydrogen and bromine in the reaction shown. 2HBr → H2 + Br2 The energy of the
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18. Which result occurs during an exothermic reaction?(1 point) Responses Light or heat are released into the environment. Light or
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19. Use the table to answer the question.%0D%0A%0D%0AReaction%09Bonds Present%09Energy of Bonds Broken and Formed (kJ/mol)%0D%0AC +
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20. Use the table to answer the question.Reaction Bonds Present Energy of Bonds Broken and Formed (kJ/mol) C + O2→CO2 O=O 2 C=O
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    2. asked by d
    3. 16 views
21. When producing hydrogen iodide, the energy of the reactants is 581 kJ/mol, and the energy of the products is 590 kJ/mol. The
    1. 1 answer
    2. asked by d
    3. 16 views
22. When producing hydrogen iodide, the energy of the reactants is 581 kJ/mol, and the energy of the products is 590 kJ/mol. The
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    2. 18 views
23. Given the enthalpy of reactants is 100 and enthalpy of product is 300.What is the enthalpy change of the energy profile graph
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    2. asked by JESSY
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24. If this reaction was too difficult to conduct in a calorimeter, the following known reactions would be usedto determine
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25. . In the Solvay process for the production of sodium carbonate (or washing soda), one step is thedecomposition of sodium
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26. 1 mol of an ideal gas with Cp=20J/K/mol is maintained at 400k in a volume of 50dm^3. Determine the initial pressure of the
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27. Suggest a physical interperation of the dependence of the Gibbs energy on the temperature.
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    2. asked by Davepee
    3. 31 views
28. Calculate the molar entropy of a constant-volume sample of argon at 250K given that it is 154.84 J/K/mol at 298K.
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    2. asked by Davepee
    3. 35 views
29. Calculate the standard Gibbs energy of the reaction CO (g) + CH3OH (l) ----> CH3COOH (l) at 298K, from the standard entropies
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    2. asked by Davepee
    3. 41 views
30. Calculate the molar entropy of a constant-volume sample of argon at 250K given that it is 154.84J/K/mol at 298K.
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    2. asked by Davepee
    3. 32 views
31. Calculate delta rH° and delta rU° at at 298K and delta rH° at 348K for the hydrogenation of ethyne to ethene from the
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    2. asked by Davepee
    3. 47 views
32. Calculate ΔH for the process: Hg₂Cl₂(s) ⟶ 2Hg(l) + Cl₂(g) from the following information:Hg(l) + Cl₂(g)⟶HgCl₂(s)
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33. A sample consists of 2.00 mole He is expanded isothermally at 22 degree celsius from 22.8 dm³ to 31.7 dm³(a) reversibly, (b)
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    2. asked by Davepee
    3. 65 views
34. A sample consists of 2.0 mole He was expanded isothermally at 22 degree celsius from 22.8 dm³ (a) reversibly, (b) against a
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    2. asked by Davepee
    3. 44 views
35. Using the hess's law to calculats the enthalpy change for the synthesis of diborane from its element according to equation2B(s)
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36. In reaction below2Al(s) +Fe2O3(s) = Al2O3(s) +2Fe(l) Calculate the heat release in kilojoules per gram of Al reacted with Fe2O3
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37. A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities involved in the process
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38. Determine the pressure CHANGE when a constant volume of gas at 1.00 atm is heated from 20.0 °C to 30.0 °C.
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    2. asked by Will
    3. 29 views
39. determine the enthalpy change for the combustion of 1 mole of C2H6g with all reactants and product in their standard state.
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    2. asked by Yusuf S Yamma
    3. 21 views
40. The vapour pressure of pure ethanol at 20 deg C is 44 mm HG . Alcohol contains 45 % ethanol and 55% water by weight. What would
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41. A sample of 10.0 grams of carbon dioxide gas is contained in a tank with a volume of 6.0 L so that the pressure inside the tank
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42. A 10.0 l gas cylinder contains nitrogen gas at a pressure of 98.2 PSI at 24°C what will the pressure of the gas be if the
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    2. asked by Alicia
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43. Kpa
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44. Why do the molecules of this substance move so quickly?
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45. Which of the following reactions is an example of an endothermic reaction?A. H2O(l) + energy → 2H2(g) + O2(g) B. 2H2(g) +
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    2. asked by akarsha
    3. 42 views
46. Reaction B, The change in enthalpy for the forward reaction is -91kJ/mol. (Energy is a product, flowing from the chemical
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47. Which of the following describes a process that releases or produces energy to its surroundings?1 point endothermic equilibrium
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48. Which of the following describes a process that absorbs or uses energy from its surroundings?1 point endothermic equilibrium
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49. If the tempature of 34.4 g of ethanol increases from 25.0 C to 78.8 C, how much heat has been absorbed by the ethonal?
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50. Lab: Enthalpy
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    2. asked by babs
    3. 39 views
51. What’s the heat of this reaction: C2H4 (g) + H2O (g) —-> C2H5OH (l)
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52. Calculate the change in heat for the reaction 2C + H2 > C2H2 given the following chemical equations and their respective
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    2. 51 views
53. What is the enthalpy of reaction, ΔH, for the formation of tungsten carbide, WC, from itselements? W (s) + C (graphite) → WC
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54. You are given the melting point and boiling point of an unknown substance. You are to create a heating curve from the data
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    2. asked by LostCoward
    3. 88 views
55. Calculate q, change in U, change in H and change in S for the process of heating 4 mol of O2 adiabatically at a constant
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    2. asked by Wesley
    3. 65 views
56. If heat is removed from the equilibrium below, what will happen? a The system will move toward more freezing, with more solid
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57. Which of the following is an endothermic process?* 1 point combusting methane freezing acetone condensing water melting ice
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    2. 54 views
58. When ethanol burn in a container, the container is hot to touch. Which of the following statement is true regarding the
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    2. 52 views
59. Which of the following process is likely to be an endothermic process?* 1 point freezing of water to ice cooling of graphite
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    2. 54 views
60. Which of the following statement is true?* 1 point in an endothermic process, heat is transferred from the surrounding to the
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61. Not enough information provided to solve the questionThe enthalpy of reaction is negative and the entropy of reaction is
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    2. 51 views
62. Which one of the following has the highest standard molar entropy, S°, at 25°C?N2(g) F2(g) Cl2(g) O2(g) H2(g)
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63. Place the following in order of decreasing molar entropy at 298 K.Thermo3 H2 > Cl2 > F2 F2 > Cl2 > H2 H2 > F2 > Cl2 Cl2 > F2 >
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64. Predict the sign of ΔG0 and ΔSuniverse for water freezing at -10℃ and 1 atm. Note that the normal freezing point of water is
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65. Predict the sign of ΔG0 and ΔSuniverse for water freezing at -10℃ and 1 atm. Note that the normal freezing point of water is
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66. phase vs molecular complexity, which has more influence on entropy
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67. How do we qualitatively rank influences on entropy? A) Phase B) Molecular Complexity C) Molar Quantity D) They all influence
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68. The heat of vaporization of isopropanol (C3H8O) is 158.5 -. How much energy in calories is absorbed when 37. g of isopropanol is
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    2. 51 views
69. Is the process of water evaporating endothermic or exothermic?(1 point)Responses It is exothermic because heat from the
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70. Reaction B, The change in enthalpy for the forward reaction is -91kJ/mol. (Energy is a product, flowing from the chemical
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71. Which of the following is an example of an endothermic change?* 1 point burning boiling freezing cooling
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72. ΔΗ =- 55kcal mol Equilibrium favors the (Choose one)
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73. Part 3 of 3ΔΗ =- 100 kcal mol or ΔΗ=+100 kcal mol OAH =- 100 will proceed faster × Ο ΔΗ=+100 kcal mol cannot predict
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74. The question asks about the energy released during the reaction of 52.0 g of ethylene. To find the energy released, we’ll need
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75. The question asks about the energy released during the reaction of 52.0 g of ethylene. To find the energy released, we’ll need
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76. Reaction B (attached); The change in enthalpy for the forward reaction is -91kJ/mol. (Energy is a product, flowing from the
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    2. 63 views
77. The specific heat of liquid bromine is 0.226 J/(g•°C). How much heat (J) is required to raise the temperature of 31.2 g of
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78. In an endorthermic reaction, the reactants have a higher , total bond energy. This means the relative potential energy of the
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79. Sulfur trioxide, a precursor of sulfuric acid, is prepared industrially using the contact process by passing sulfur dioxide and
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80. Let’s calculate the specific heat of cadmium using the information provided.Known Quantities: Heat absorbed by cadmium metal,
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81. Consider the reaction, C2H4(g) + H2(g) → C2H6(g), where ΔH = –137 kJ. How many kilojoules are released when 3.5 mol of C2H4
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82. 9) Consider the reaction: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g), where ΔH = –531 kcal. Which statement concerning this
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83. Calorimetry, enthalpy, standard state, Hess's Law, and the second law of thermodynamics are all important concepts in the study
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84. Calorimetry is the science of using a calorimeter, a device used to measure the change in heat associated with a chemical
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85. Determine the value of the enthalpy change, AH an, for the following reaction using the information below.AP Chemistr 4 Al ( * 3
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86. The standard heat of vaporization, AH vap of SO, is + 24.3 kJ/mol and that of F,is +5.9 k//mol.a. Identify the types) of
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87. Calculate the heat of combustion of a compound if o.06 mole of burning raise the temperature of 40.0gm of water by 10k ( specfic
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    2. asked by Zubydon
    3. 58 views
88. SynopsisEnergy is one of the great subject matters of our time, but what is energy actually? In this simulation you will learn
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89. Which quantity will always have a negative valueA. The total bond energy of products during an exothermic reaction B.The total
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90. Choose the situation below that would result in an endothermic ΔHsolution.when the magnitude of ΔHsolute is less than
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91. What is activation energy?(1 point)Responses the kinetic energy of the reactants of a system after the reaction has begun the
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92. Add the energies on the reactant side- 1678 KJ/molAdd the energies on the product side-7828 KJ/mol This reaction is endothermic,
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93. A reaction (produces or absorbs) kJ when 2 moles of acetylene (C2H2) reacts.Does it produce or absorb?
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94. Using the data of 0.3 degrees Celsius freezing point of water-ice mixture, mass of solid unknown used 5.034g, freezing point of
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95. The reaction is exothermic because the total bond energy of the reactants is less than the total bond energy of the products.
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96. some nitrogen and hydrogen gases are pumped into an empty 5.00liter vessel at 500°c. when equilibrium was established, 3.00
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97. A student writes, “A reaction is endothermic because the temperature went up. The reaction feels cold.” Why is this student
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    2. asked by jack
    3. 77 views
98. What is the combined energy absorbed for the reactant side of the equation? (Hint: add up the energies needed to break the bonds
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99. Determine the standard molar enthalpy of combustion of octane using Hess's law
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100. C(s) + 2Cl2(g) -> CCl4(l) ∆= -106.4 kJ What is the molar enthalpy for chlorine?
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