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Choose Your Category

Choose Your Category. Round Two. Potential Energy Graph - 100. Where is the location on the activated complex on this graph?. The Answer is the top of the hump. Back. Potential Energy Graph - 200. What is the energy of the products?. The Answer is 100 J. Back.

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Choose Your Category

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  1. Choose Your Category Round Two

  2. Potential Energy Graph - 100 Where is the location on the activated complex on this graph? The Answer is the top of the hump. Back

  3. Potential Energy Graph - 200 • What is the energy of the products? The Answer is 100 J. Back

  4. Potential Energy Graph - 300 • What is the energy needed to break the chemical bonds? The Answer is 100 J. Back

  5. Potential Energy Graph - 400 • What is the net energy of this reaction? The answer is -200 J Back

  6. Daily Double

  7. Reaction Rates - 100 • Calcium carbonate was placed in a flask on a balance, and dilute hydrochloric acid was added. Carbon dioxide that was produced escaped from the flask. The total mass of the flask and its contents was recorded every 10 seconds. The diagram to the right shows a plot of the results. Between which two times shown was the reaction the fastest? Back The Answer is 0-10 seconds.

  8. Reaction Rates - 200 At equilibrium, the forward reaction rate is _____________ to the reverse reaction rate. The Answer is equal Back

  9. Reaction Rates - 300 • The role of a catalyst is to affect ________________. • The Answer is activation energy. Back

  10. Daily Double

  11. Reaction Rates - 400 • Name three factors that can influence the rate of a reaction. The Answer is any three of the following: concentration of the reactants temperature surface area pressure catalysts Back

  12. Keq and Ksp – 100 • What is ksp for the dissociation of NaCl in water? NaCl (s) + H2O (l)  Na+ (aq) + Cl- (aq) The Answer is [Na+][Cl-] Back

  13. Keq and Ksp – 200 • What is the equilibrium expression (Keq) for the following reaction? CaCO3(s) + 2H3O+(aq) Ca2+(aq) + CO2(g) + 3H2O(l) The Answer is Keq=[Ca2+][CO2] [H3O+]2 Back

  14. Random Points 100 Points

  15. Keq and Ksp – 300 • A very low value of the equilibrium constant for a reaction can indicate that A) products are favored B) equilibrium is reached slowly C) Reactants are favored D) equilibrium is reached quickly The Answer is C. Back

  16. Keq and Ksp – 400 • What is the solubility in mol/L of silver iodide, AgI? Its Ksp value is 8.3 x 10-17 and the equation is AgI (s)  Ag+1(aq) + I-1(aq). The Answer is 9.11 x 10-9 Back

  17. Le Châtelier's Principle - 100 [Ni(H2O)6]+2 + 6NH3 [Ni(NH3)6]+2 + 6H2O (endothermic) green blue-violet • What color would you except the above solution to be if NH3 is added? (Green, blue-violet or no change) The Answer is blue-violet Back

  18. Le Châtelier's Principle - 200 [Ni(H2O)6]+2 + 6NH3 [Ni(NH3)6]+2 + 6H2O (endothermic) green blue-violet • What color would you except the above solution to be if water is removed? (Green, blue-violet or no change) The Answer is blue-violet. Back

  19. Random Points 300 Points

  20. Le Châtelier's Principle - 300 [Ni(H2O)6]+2 + 6NH3 [Ni(NH3)6]+2 + 6H2O (endothermic) green blue-violet • What color would you except the above solution to be if NaBr is added? (Green, blue-violet or no change) The Answer is no change. Back

  21. Le Châtelier's Principle - 400 [Ni(H2O)6]+2 + 6NH3 [Ni(NH3)6]+2 + 6H2O (endothermic) green blue-violet • What color would you except the above solution to be if the solution is heated? (Green, blue-violet or no change) The Answer is blue-violet Back

  22. Definitions – 100 • A chemical reaction in which the products re-form the original reactants The Answer is reversible reaction. Back

  23. Random Points 500 Points

  24. Definitions – 200 • A state of balance in which the rate of a forward reaction equals the rate of the reverse reaction and the concentrations of substances do not change The Answer is equilibrium. Back

  25. Definitions – 300 • A type of protein that speeds up metabolic reactions in plant and animals without being permanently changed or destroyed The Answer is an enzyme. Back

  26. Definitions – 400 • The minimum amount of energy required to start a chemical reaction. The Answer is activation energy. Back

  27. Choose Your Category The Final Question

  28. Properties - 100 • Acids taste __________________. The Answer is sour, or any word that means sour. Back

  29. Properties - 200 • If a base was touched, it would feel ____________________. The Answer is slippery. Back

  30. Properties - 300 • Strong acids are ______________ electrolytes. The Answer is strong. Back

  31. Properties - 400 • Strong acids ______________ ionize when added to water. The Answer is completely. Back

  32. Identify the Acid or Base - 100 Whose definition of acids and bases emphasizes the role of protons? The Answer is Brønsted-Lowry Back

  33. Random Points 300 Points

  34. Identify the Acid or Base - 200 • An Arrhenius Acid increases the _____________ concentration. The Answer is hydronium. Back

  35. Identify the Acid or Base - 300 • In the reaction H3PO4 + H2O  H3O+ + H2PO4-, the ion H2PO4- acts as a(n) ___________________. The Answer is base. Back

  36. Daily Double

  37. Identify the Acid or Base - 400 • Label the acid, base, conjugate acid, and conjugate base in the equation: • HCl(g) + H2O(l)  H3O+(aq) + Cl-(aq) acid base conj acid conj base Back

  38. pH - 100 • What is the pH of a neutral solution at 25°C? The Answer is 7. Back

  39. Random Points 500 Points

  40. pH - 200 The pH of a solution is 8. What is its H3O+ concentration? The Answer is 1x 10-8 Back

  41. pH - 300 • What is the pH of a 1 x 10-3 M KOH solution? • The Answer is 11. Back

  42. pH - 400 • What is the pH of a 0.00870 M KOH solution? The Answer is 11.9. Back

  43. Kw and Ka– 100 • What is the value of the self-ionization constant of water? The Answer is 1 x 10-14 Back

  44. Kw and Ka– 200 • What is the equilibrium expression (Kw) for the self-ionization of water? The Answer is Kw=[OH-][H3O+] Back

  45. Kw and Ka– 300 • What is the acid-ionization constant, Ka, for the ionization of acetic acid, shown in the reaction • CH3COOH(aq) + H2O(l)  H3O+(aq) + CH3COO–(aq)? The Answer is [H3O+][CH3COO-]/[CH3COOH] Back

  46. Daily Double

  47. Kw and Ka– 400 • A 0.845 M sample of carbonic acid, H2CO3, has a measured hydronium ion concentration of 5.36 x 10–3 M. Calculate the acid-ionization constant of carbonic acid. The equilibrium equation is • H2CO3(aq)_+ H2O (l)  H3O+ (aq) + HCO3-(aq) The Answer is 3.4 x 10-5 Back

  48. Titrations - 100 • During a titration the volume of the titrant is measured with a(n) ____________________. The Answer is buret or burette Back

  49. Titrations - 200 • What unknown quantity can be calculated after performing a titration? The Answer is concentration or volume. Back

  50. Titrations - 300 • During a titration, the indicator _________________________ is used to study neutralizations of weak acids with strong bases. The Answer is phenolphthalein. Back

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