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100. 100. 100. 100. 100. 200. 200. 200. 200. 200. 300. 300. 300. 300. 300. 400. 400. 400. 400. 400. 500. 500. 500. 500. 500. Energy, Heat, & Work 100. Convert 450 J to kJ. Next Question. Energy, Heat, & Work 200. Is the following reaction endothermic or exothermic?

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  1. 100 100 100 100 100 200 200 200 200 200 300 300 300 300 300 400 400 400 400 400 500 500 500 500 500

  2. Energy, Heat, & Work100 Convert 450 J to kJ Next Question

  3. Energy, Heat, & Work200 Is the following reaction endothermic or exothermic? 2 NH4Cl + Ba(OH)2 → 2 NH3 + 2 H2O + BaCl2 ΔHrxn = +54.8 kJ Next Question

  4. Energy, Heat, & Work300 What will determine the direction of heat flow in a chemical or physical process? Next Question

  5. Energy, Heat, & Work400 A hot air balloon is heated by a torch that provides 1,000,000 kJ of energy. As it expands, the balloon does 300,000 kJ of work on the surroundings. What is ΔEballoon? Next Question

  6. Energy, Heat, & Work500 A small pipe bomb explodes, releasing 50,000 kJ of heat and doing 25,000 kJ of work on the surroundings. What is ΔEsurroundings? Next Question

  7. Calorimetry100 You have 100 g of an unknown substance. What property of the substance will help you determine how much its temperature will increase when 250 kJ are added to it? Next Question

  8. Calorimetry200 You have 10 moles of liquid nitrogen. What property of the N2will help you determine how much energy it will absorb as it becomes a gas? Next Question

  9. Calorimetry300 A 2.0 gram sample of food is burned in a calorimeter, increasing the temperature of 100 g of water by 10 °C. What is the energy content of the food in Calories/g? Next Question

  10. Calorimetry400 An 36 g sample of water at 0 °C is frozen into steam at -10 °C. How much energy is removed from the water in the process? Next Question

  11. Calorimetry500 An 18 g sample of water at 90 °C is boiled into steam at 100 °C. How much energy is absorbed by the water in the process? Next Question

  12. Hess’s Law100 What is ΔHrx for: Cu (s) + CuO (s) → Cu2O (s) Next Question

  13. Hess’s Law200 What is ΔHrx for: 2 CuO(s) → Cu2O (s) + ½ O2 (g) Next Question

  14. Hess’s Law300 What is ΔHrx for: S (s) + O2 (g) → SO2 (g) Next Question

  15. Hess’s Law400 What is ΔHrx for: Cu (s) + ½ O2 (g) → CuO(s) Next Question

  16. Next Question Hess’s Law500 What is ΔHrx for: Mg (s) + O2(g) + H2(g) → Mg(OH)2(s) Next Question

  17. Enthalpies of Formation100 What is the ΔHf° for Cl2 (g) ? Next Question

  18. Enthalpies of Formation200 What is the reaction of formation for N2O (g) ? Next Question

  19. Enthalpies of Formation300 What is the reaction of formation for HNO3 (l) ? Next Question

  20. Enthalpies of Formation400 Using your thermodynamic table, determine the ΔH for the following reaction: CaO (s) + CO2 (g) → CaCO3 (s) Next Question

  21. Enthalpies of Formation500 Using your thermodynamic table, determine the ΔH for the following reaction: CH3OH (l)+ 3/2 O2(g) → CO2(g) + 2 H2O (g) Next Question

  22. Potpourri100 H2(g)+ ½ O2(g) → H2O (g) ∆H = -241.8 kJ Should ∆H be written with reactants or products? Next Question

  23. Potpourri 200 Which state of matter has the lowest amount of internal energy? Next Question

  24. Potpourri300 What property of a substance can be defined as the average kinetic energy of its particles? Next Question

  25. Potpourri400 What is the ∆T when water boils at normal atmospheric pressure? Next Question

  26. Potpourri500 H2 (g) + ½ O2 (g) → H2O (g) ∆H = -241.8 kJ How much heat will be absorbed/released when 6 g of H2 are consumed? Next Question

  27. Daily Double !!

  28. Daily Double !!

  29. Final Jeopardy None

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