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Physical Chemistry Quiz

Physical Chemistry Quiz. Please be aware that some questions may require more than one answer without warning. Thermodynamics: The Second and Third Laws. A. A change that tends to occur without needing to be driven by an external influence.

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Physical Chemistry Quiz

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  1. Physical Chemistry Quiz Please be aware that somequestions may requiremore than one answer without warning

  2. Thermodynamics: The Second and Third Laws

  3. A A change that tends to occur without needing to be driven by an external influence A change that tends to occur with needing to be driven by an external influence A change that tends to occur without needing to be driven by an internal influence A change that tends to occur with needing to be driven by an internal influence What is the definition of a spontaneous change? B C D

  4. A A change that tends to occur without needing to be driven by an external influence A change that tends to occur with needing to be driven by an external influence A change that tends to occur without needing to be driven by an internal influence A change that tends to occur with needing to be driven by an internal influence What is the definition of a spontaneous change? B C D

  5. A Given constant temperature the entropy change is given by? B C D

  6. A Given constant temperature the entropy change is given by? B C D

  7. A Irreversible Naturally decreasing over the universe Given the sign E A State function Entropy is B C D

  8. A Irreversible Naturally decreasing over the universe Given the sign E A State function Entropy is B C D

  9. A + 0.308 JK-1 + 17.31 JK-1 + 0.710 JK-1 - 0.710 JK-1 A sample of N2 gas of volume 20 L at 5.00 kPa is heated from 20 °C to 400 °C at constant volume. What is the change in entropy of the nitrogen? B C D

  10. A + 0.308 JK-1 + 17.31 JK-1 + 0.710 JK-1 - 0.710 JK-1 A sample of N2 gas of volume 20 L at 5.00 kPa is heated from 20 °C to 400 °C at constant volume. What is the change in entropy of the nitrogen? B C D

  11. A The entropy of the universe is naturally progressing from high to low disorder The entropy of an isolated system increases in the course of a spontaneous change The entropy of an isothermal system increases in the course of a spontaneous change The entropy of an isolated system decreases in the course of a spontaneous change What is the second law of thermodynamics? B C D

  12. A The entropy of the universe is naturally progressing from high to low disorder The entropy of an isolated system increases in the course of a spontaneous change The entropy of an isothermal system increases in the course of a spontaneous change The entropy of an isolated system decreases in the course of a spontaneous change What is the second law of thermodynamics? B C D

  13. A The emissivity of a body is equal to its absorbance at the same temperature When a system at equilibrium is disturbed, the equilibrium conditions shift to counteract the disturbance The internal energy of an isolated system is constant For every action there is an equal and opposite reaction Which of the following is a concise statement about the First Law of Thermodynamics? B C D

  14. A The emissivity of a body is equal to its absorbance at the same temperature When a system at equilibrium is disturbed, the equilibrium conditions shift to counteract the disturbance The internal energy of an isolated system is constant For every action there is an equal and opposite reaction Which of the following is a concise statement about the First Law of Thermodynamics? B C D

  15. A The symbol used to represent internal energy is U The symbol used to represent enthalpy is H The symbol used to represent enthalpy is E The symbol used to represent enthalpy is U Which of the following is correct B C D

  16. A The symbol used to represent internal energy is U The symbol used to represent enthalpy is H The symbol used to represent enthalpy is E The symbol used to represent enthalpy is U Which of the following is correct B C D

  17. A A reversible process may easily be made to proceed in the reverse direction A reversible process may be undone completely The symbol used to represent internal energy is H The symbol used to represent internal energy is E Which of the following is correct B C D

  18. A A reversible process may easily be made to proceed in the reverse direction A reversible process may be undone completely The symbol used to represent internal energy is H The symbol used to represent internal energy is E Which of the following is correct B C D

  19. A A reversible process produces the maximum possible entropy A reversible process produces the maximum possible heat A reversible process produces the maximum possible work A reversible process is always in equilibrium Which of the following is correct B C D

  20. A A reversible process produces the maximum possible entropy A reversible process produces the maximum possible heat A reversible process produces the maximum possible work A reversible process is always in equilibrium Which of the following is correct B C D

  21. A - 2.50 JK-1 + 2.50 JK-1 - 5.76 JK-1 + 5.76 JK-1 What is the change in entropy of the gas then 1.00 mol N2(g) expands isothermally from 22 L to 44 L? B C D

  22. A - 2.50 JK-1 + 2.50 JK-1 - 5.76 JK-1 + 5.76 JK-1 What is the change in entropy of the gas then 1.00 mol N2(g) expands isothermally from 22 L to 44 L? B C D

  23. A - 4.27 JK-1 + 4.27 JK-1 - 9.85 JK-1 + 9.85 JK-1 Calculate the change in entropy when the pressure of 0.321 mol O2(g) is increased from 0.300 atm to 12.00 atm at constant temperature? B C D

  24. A - 4.27 JK-1 + 4.27 JK-1 - 9.85 JK-1 + 9.85 JK-1 Calculate the change in entropy when the pressure of 0.321 mol O2(g) is increased from 0.300 atm to 12.00 atm at constant temperature? B C D

  25. A Entropy changes with state The phase transition takes place at constant P so the heat supplied is equal to the enthalpy of the phase change At the phase transition temperature the transfer of heat is reversible At the transition temperature the temperature remains constant as heat is supplied Which of the following statements are correct? B C D

  26. A Entropy changes with state The phase transition takes place at constant P so the heat supplied is equal to the enthalpy of the phase change At the phase transition temperature the transfer of heat is reversible At the transition temperature the temperature remains constant as heat is supplied Which of the following statements are correct? B C D

  27. A - 0.01 JK-1mol-1 +0.01JK-1mol-1 + 88.4 JK-1mol-1 - 88.4 JK-1mol-1 What is the entropy of vaporisation of acetone at its normal boiling point of 56.2 °C? 29.1kJmol-1 B C D

  28. A - 0.01 JK-1mol-1 +0.01JK-1mol-1 + 88.4 JK-1mol-1 - 88.4 JK-1mol-1 What is the entropy of vaporisation of acetone at its normal boiling point of 56.2 °C? 29.1kJmol-1 B C D

  29. A + 85 JK-1 + 28 kJmol-1 + 28 JK-1 - 28 kJmol-1 Use Trouton’s rule to estimate the enthalpy of vaporisation of liquid bromine which boils at 59 °C? B C D

  30. A + 85 JK-1 + 28 kJmol-1 + 28 JK-1 - 28 kJmol-1 Use Trouton’s rule to estimate the enthalpy of vaporisation of liquid bromine which boils at 59 °C? B C D

  31. A The entropy of an isolated system increases in the course of a spontaneous change S  0 as T  0 The enthalpies of all perfect crystals approach zero as the absolute temperature approaches zero What is the third law of thermodynamics? B C D

  32. A The entropy of an isolated system increases in the course of a spontaneous change S  0 as T  0 The enthalpies of all perfect crystals approach zero as the absolute temperature approaches zero What is the third law of thermodynamics? B C D

  33. A + 1 JK-1 - 4 JK-1 0 JK-1 + 3.82 JK-1 Calculate the statistical entropy of a solid made of four CO molecules at T = 0 when all molecules are perfectly alligned. B C D

  34. A + 1 JK-1 - 4 JK-1 0 JK-1 + 3.82 JK-1 Calculate the statistical entropy of a solid made of four CO molecules at T = 0 when all molecules are perfectly alligned. B C D

  35. A 0 JK-1 + 1.81 x 10-23 JK-1 + 3.82 x 10-23 JK-1 + 3.82 JK-1 Calculate the statistical entropy of a solid made of four CO molecules at T = 0 the four molecules lie in random orientations. B C D

  36. A 0 JK-1 + 1.81 x 10-23 JK-1 + 3.82 x 10-23 JK-1 + 3.82 JK-1 Calculate the statistical entropy of a solid made of four CO molecules at T = 0 the four molecules lie in random orientations. B C D

  37. A This is extremely incorrect according to Boltzmann Law There are a possible 16 microstates This is approximately correct according to Boltzmann Law The entropy of 1.00 mol of FClO3 at T=0 is 10.1 JK-1. Suggest an interpretation. The predicted entropy is 11.5 kJ-1mol-1 B C D

  38. A This is extremely incorrect according to Boltzmann Law There are a possible 16 microstates This is approximately correct according to Boltzmann Law The entropy of 1.00 mol of FClO3 at T=0 is 10.1 JK-1. Suggest an interpretation. The predicted entropy is 11.5 kJ-1mol-1 B C D

  39. A More overall energy is gained More energy levels are available More microstates are available If we regard gas as lots of ‘particles in a box’, what happens as we increase the length of the box? Entropy Increases B C D

  40. A More overall energy is gained More energy levels are available More microstates are available If we regard gas as lots of ‘particles in a box’, what happens as we increase the length of the box? Entropy Increases B C D

  41. A More overall energy is gained More energy levels are available More microstates are available If we regard gas as lots of ‘particles in a box’, what happens as we increase the temperature of the box? Entropy Increases B C D

  42. A More overall energy is gained More energy levels are available More microstates are available If we regard gas as lots of ‘particles in a box’, what happens as we increase the temperature of the box? Entropy Increases B C D

  43. A More overall energy is gained More energy levels are available More microstates are available If we regard gas as lots of ‘particles in a box’, what happens as we increase mass of individual gas molecules? Microstates are more closely spaced B C D

  44. A More overall energy is gained More energy levels are available More microstates are available If we regard gas as lots of ‘particles in a box’, what happens as we increase mass of individual gas molecules? Microstates are more closely spaced B C D

  45. 4 3 2 1 5 A 5: △S , 4: △Stot , 3: Ssurr, 1: System of interest, 2: Isolated system 2: △S , 1: △Stot , 3: △Ssurr , 5: System of interest, 4: Isolated system 1: △S , 2: △Stot , 3: △Ssurr , 4: System of interest, 5: Isolated system 1: △S , 5: △Stot , 3: △Ssurr , 2: System of interest, 4: Isolated system What is the correct labelling of the beside representation? B C D

  46. 4 3 2 1 5 A 5: △S , 4: △Stot , 3: Ssurr, 1: System of interest, 2: Isolated system 2: △S , 1: △Stot , 3: △Ssurr , 5: System of interest, 4: Isolated system 1: △S , 2: △Stot , 3: △Ssurr , 4: System of interest, 5: Isolated system 1: △S , 5: △Stot , 3: △Ssurr , 2: System of interest, 4: Isolated system What is the correct labelling of the beside representation? B C D

  47. A + 309 JK-1 - 309 JK-1 0 JK-1 Calculate the change in entropy of the surroundings when the following reaction goes to completion at 298 K. N2(g) + 3H2(g) NH3(g)△H = - 92.22 kJ at 298 K + 323 JK-1 B C D

  48. A + 309 JK-1 - 309 JK-1 0 JK-1 Calculate the change in entropy of the surroundings when the following reaction goes to completion at 298 K. N2(g) + 3H2(g) NH3(g)△H = - 92.22 kJ at 298 K + 323 JK-1 B C D

  49. A + 3.81 x 103 JK-1 - 3.81 JK-1 + 3.81 JK-1 Assess whether the combustion of magnesium is spontaneous at 25 °C. 2Mg(s) + O2(g) 2MgO (g) △S = - 217 JK-1 △H = - 1202 kJ - 3.81 x 103 JK-1 B C D

  50. A + 3.81 x 103 JK-1 - 3.81 JK-1 + 3.81 JK-1 Assess whether the combustion of magnesium is spontaneous at 25 °C. 2Mg(s) + O2(g) 2MgO (g) △S = - 217 JK-1 △H = - 1202 kJ - 3.81 x 103 JK-1 B C D

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