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Comprehensive Review of Thermodynamics Concepts and Calculations

This review game covers essential topics in thermodynamics, including the heat of fusion, Gibbs energy, entropy, molar heat capacity, and enthalpy. Questions explore the calculations involved in determining heat absorbed or released during chemical reactions, the spontaneous nature of reactions, and the relationships between different thermodynamic variables. Players will engage with various scenarios and equations to deepen their understanding of energy changes in physical and chemical processes. Perfect for students preparing for exams in physical chemistry.

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Comprehensive Review of Thermodynamics Concepts and Calculations

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  1. Unit 7 Review Game Board

  2. 1 What is the heat of fusion in kJ/g of a substance if it takes 65980 J of heat to melt a 55 g sample of the substance? 1.2 kJ/g Back

  3. 2 A reaction occurs spontaneously when G is: negative Back

  4. 3 605 K equals how many degrees Celsius? 332 C Back

  5. 4 A measure of the average kinetic energy of the particles in a sample of matter? Temperature Back

  6. 5 What letter corresponds to the melting of a solid? b Back

  7. 6 In the equation, q = nCT, what does q stand for? heat Back

  8. 7 What is a measure of the disorder in a system? entropy Back

  9. 8 What is the formula that defines the change in Gibbs energy? G = H – TS Back

  10. 9 The study of all energy changes is called Thermodynamics Back

  11. 10 In the equation, q=nCT, what does C stand for? Molar heat capacity Back

  12. 11 According to ____________________, the overall enthalpy change in a reaction is equal to the sum of the enthalpy changes of individual steps. Hess’s Law Back

  13. 12 A positive S means the process was ____________. More disorderly Back

  14. 13 Entropy plays a larger role in determining the Gibbs energy of reactions that take place at _____________ temperatures. Higher Back

  15. 14 This is the energy of a system at constant pressure. Enthalpy Back

  16. 15 In the Gibb’s energy equation, ___________ is the symbol for entropy. S Back

  17. 16 The standard enthalpy of formation of a(n) ____________ is equal to zero. element Back

  18. 17 In the expression q = nCT, what does n represent? moles Back

  19. 18 A negative G means the process was ____________. spontaneous Back

  20. 19 The term ____________________ refers to the amount of energy as heat required to raise the temperature of 1 mole of a substance by 1 K. Molar heat capacity Back

  21. 20 A negative H means the process was ____________. exothermic Back

  22. 21 A device used to measure the heat absorbed or released in a chemical or physical change calorimeter Back

  23. 22 This equation is used to calculate heat. q=nCT Back

  24. 23 What letter represents the range where the liquid is being warmed? c Back

  25. 24 In the Gibb’s energy equation, __________ is the symbol for enthalpy. H Back

  26. 25 What is 52 Joules in calories? 12.4 calories Back

  27. 26 A 58.2 g sample was heated from 300 K to 350 K. It absorbed 1523 J of energy. What is the specific heat of iron? 0.53 J/gK Back

  28. 27 The total entropy of the products in a reaction is 732 J/K, and the total entropy of the reactants is 524 J/K. What is S for the reaction? 208 J/K Back

  29. 28 452 ºF to ºC 233 C Back

  30. 29 How much energy as heat does an iron (MM = 55.8 g/mol) sample gain if its molar heat capacity is 25.1 J/K mol, its mass is 33.01 g, and it is heated from 15.0°C to 42.0°C? 400.9 J Back

  31. 30 If 1484 J of energy as heat is released from a 800 g block of aluminum (MM = 27.0). What temperature change occurred if the molar heat capacity of aluminum is 24.2 J/K.mol? 2.07 K Back

  32. 31 What is the boiling point of the substance (number)? 450 K Back

  33. 32 A 426.3 g sample of Gold (MW = 197) was heated from 0°C to 20°C. It absorbed 1108 J of energy. What is the molar heat capacity of iron? 25.6 J/mol.°C Back

  34. 33 341 K equals how many degrees Fahrenheit? 154 C Back

  35. 34 What is the value of G at 330 K for a reaction in which H = –103 kJ/mol and S = +23.00 J/mol K? -110590 J/mol Or -110.59 kJ/mol Back

  36. 35 For a process in which H is –98 kJ and S is 132 J/K, calculate the change in the free energy at 0°C. -134036 J/mol Or -134 kJ/mol Back

  37. 36 When calculating the change in enthalpy of a reaction, this is the equation that is used. H reaction = H products - H reactants Back

  38. 37 Water has a specific heat of 4.18 J/gK. What is its molar heat capacity? 75.24 J/molK Back

  39. 38 How much heat would be needed to evaporate 100 g of water if the heat of vaporization of water is 2.26 kJ/g? 226 kJ Back

  40. 39 How much energy as heat does a 9 mol titanium sample gain if its molar heat capacity is 27.8 J/K mol and it is heated from 15°C to 55.0°C? 10008 J Back

  41. 40 What is the standard thermodynamic temperature? 25 C (or 298 K) Back

  42. 41 The English measurement for measuring energy is the ___________ calorie Back

  43. 42 What is the melting point of this substance? 300 K A B Back

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