Kinetics and Equilibrium Extra Credit

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1 1. The potential energy diagram below represents the reaction 2 KClO3 2 KCl + 3 O2. 4. When AgNO3(aq) is mixed with NaCl(aq), a reaction occurs which tends to go to completion and not reach equilibrium because A) a gas is formed B) water is formed C) a weak acid is formed D) a precipitate is formed 5. Which equation represents a change that results in an increase in disorder? A) I2(s) I2(g) B) CO2(g) CO2(s) C) 2Na(s) + Cl2(g) 2NaCl(s) D) 2H2(g) + O2(g) 2H2O( ) 6. Given the system at Which numbered interval on the diagram would change when a catalyst is added? A) 1 B) 2 C) 3 D) 4 2. Given the balanced equation: Which statement best describes this process? A) It is endothermic and entropy increases. B) It is endothermic and entropy decreases. C) It is exothermic and entropy increases. D) It is exothermic and entropy decreases. 3. When ammonium chloride crystals are dissolved in water, the temperature of the water decreases. What does this temperature change indicate about the dissolving of ammonium chloride in water? A) It is an endothermic reaction because it absorbs heat. B) It is an endothermic reaction because it releases heat. C) It is an exothermic reaction because it absorbs heat. D) It is an exothermic reaction because it releases heat. N2O4(g) kj 2 NO2(g) What will be the result of an increase in temperature at constant pressure? A) The equilibrium will shift to the left, and the NO2(g) will decrease. B) The equilibrium will shift to the left, and the NO2(g) will increase. C) The equilibrium will shift to the right, and the NO2(g) will decrease. D) The equilibrium will shift to the right, and the NO2(g) will increase. 7. The net energy released or absorbed during a reversible chemical reaction is equal to A) the activation energy of the endothermic reaction B) the activation energy of the exothermic reaction C) the difference between the potential energy of the products and the potential energy of the reactants D) the sum of the potential energy of the products and the potential energy of the reactants 8. Which 1-mole sample has the least entropy? A) Br2(s) at 266 K B) Br2( ) at 266 K C) Br2( ) at 332 K D) Br2(g) at 332 K Page 1

2 9. According to Table I, which potential energy diagram best represents the reaction that forms H2O( ) from its elements? A) B) C) D) 13.Based on Reference Table G, which amount of a compound dissolved in 100 grams of water at the stated temperature represents a system at equilibrium? A) 20 g KClO3 at 80ºC B) 40 g KNO3 at 25ºC C) 40 g KCl at 60ºC D) 60 g NaNO3 at 40ºC 14. Each of four test tubes contains a different HCI(aq) at 25 C. A 1-gram cube of Zn is added to each test tube. In which test tube is the reaction occurring at the fastest rate? A) B) 10.Which statement must be true when solution equilibrium occurs? C) D) A) The solution is at STP. B) The solution is supersaturated. C) The the solution remains constant. D) The masses of the dissolved solute and the undissolved solute are equal. 11. Given the system at 15. Base your answer to the following question on Given the potential energy diagram of a chemical reaction: Which changes occur when system? is added to this A) The equilibrium shifts to the right and the increases. B) The equilibrium shifts to the right and the decreases. C) The equilibrium shifts to the left and the increases. D) The equilibrium shifts to the left and the decreases. 12. In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is equal to the A) activation energy B) kinetic energy C) heat of reaction D) rate of reaction Which arrow represents the potential energy of the reactants? A) A B) B C) C D) D 16. A solution that is at equilibrium must be A) concentrated B) dilute C) saturated D) unsaturated Page 2

3 17. Base your answer to the following question on In each of the four beakers shown below, a 2.0-centimeter strip of magnesium ribbon reacts with 100 milliliters of HCl(aq) under the conditions shown. In which beaker will the reaction occur at the fastest rate? A) A B) B C) C D) D Base your answers to questions 18 and 19 on the table below, which represents the production of 50 milliliters of CO2 in the reaction of HCl with NaHCO3. Five trials were performed under different conditions as shown. (The same mass of NaHCO3 was used in each trial.) 21. Which will occur if a catalyst is added to a reaction mixture? A) The activation energy will be changed. B) Only the rate of the forward reaction will be increased. C) Only the rate of the reverse reaction will be increased. D) The energy change (DH) of the reaction will be decreased. 22. Given the equation representing a system at 2SO2(g) + O2(g) 2SO3(g) At equilibrium, the 18. Which two trials could be used to measure the effect of surface area? A) trials A and B B) trials A and C C) trials A and D D) trials B and D 19. Which trial would produce the fastest reaction? A) trial A B) trial B C) trial C D) trial D 20. Which balanced equation represents a phase equilibrium? A) B) C) A) SO2(g) must equal the SO3(g) B) SO2(g) must be constant C) O2(g) must equal the SO2(g) D) O2(g) must be decreasing 23. The activation energy required for a chemical reaction can be decreased by A) increasing the surface area of the reactant B) increasing the temperature of the reactant C) adding a catalyst to the reaction D) adding more reactant D) Page 3

4 24. Given the equation representing a system at H2O (s) «H20 (l) At which temperature does this equilibrium exist at kilopascals? A) 0 K B) 0 C C) 32 K D) 273 C 25. Given the Haber reaction at N2(g) + 3 H2(g) «2 NH3(g) + heat Which stress on the system will decrease the production of NH3(g)? A) increasing the N2(g) B) increasing the pressure on the system C) decreasing the H2(g) D) decreasing the temperature on the system 26. Which chemical reaction will always be spontaneous? A) an exothermic reaction in which entropy decreases B) an exothermic reaction in which entropy increases C) an endothermic reaction in which entropy decreases D) an endothermic reaction in which entropy increases 27. Base your answer to the following question on Given the equation representing a reaction at H2(g) + I2(g) + heat «2HI(g) Which change favors the reverse reaction? A) decreasing the HI(g) B) decreasing the temperature C) increasing the I2(g) D) increasing the pressure 28. As the temperature increases, the rate of an exothermic reaction 29. Given the reaction at 2 SO2(g) + O2(g) «2 SO3(g) + heat Which change will shift the equilibrium to the right? A) increasing the temperature B) increasing the pressure C) decreasing the amount of SO2(g) D) decreasing the amount of O2(g) 30. Given the reaction at The addition of a catalyst will A(g) + B(g) «C(g) + D(g) A) shift the equilibrium to the right B) shift the equilibrium to the left C) increase the rate of forward and reverse reactions equally D) have no effect on the forward or reverse reactions 31. Which equation represents an exothermic reaction at 298 K? A) B) C) D) 32. Base your answer to the following question on Given the equation representing a reaction at Which change causes the equilibrium to shift to the right? A) decreasing the B) decreasing the pressure C) increasing the D) increasing the temperature A) decreases B) increases C) remains the same Page 4

5 33. Given the equilibrium reaction in a closed system: 37. Given the reaction: H2(g) + I2(g) + heat «2 HI(g) What will be the result of an increase in temperature? A) The equilibrium will shift to the left and [H2] will increase. B) The equilibrium will shift to the left and [H2] will decrease. C) The equilibrium will shift to the right and [HI] will increase. D) The equilibrium will shift to the right and [HI] will decrease. S(s) + O2(g) SO2(g) + energy Which diagram best represents the potential energy changes for this reaction? A) B) 34. Given the system at H2(g) + F2(g) 2 HF(g) + heat Which change will not shift the point of equilibrium? A) changing the pressure B) changing the temperature C) changing the H2(g) D) changing the HF(g) 35. Why can an increase in temperature lead to more effective collisions between reactant particles and an increase in the rate of a chemical reaction? A) The activation energy of the reaction increases. B) The activation energy of the reaction decreases. C) The number of molecules with sufficient energy to react increases. D) The number of molecules with sufficient energy to react decreases. 36. When a single 1-gram piece of zinc is added to 3 M hydrochloric acid at 25ºC, the reaction is slow. Which procedure would most likely increase the rate of reaction if the reaction were repeated? A) using 1 gram of powdered zinc B) using 1 M hydrochloric acid C) decreasing the temperature to 20.ºC D) decreasing the the zinc C) D) 38. Given the balanced equation representing a reaction at kpa and 298 K: N2(g) + 3H2(g) 2NH3(g) kj Which statement is true about this reaction? A) It is exothermic and H equals 91.8 kj. B) It is exothermic and H equals kj. C) It is endothermic and H equals 91.8 kj. D) It is endothermic and H equals kj. Page 5

6 39. Given the system at PbCO3(s) «Pb 2+ (aq) + CO3 2 (aq) How will the addition of Na2CO3(aq) affect [Pb 2+ ](aq) and the mass of PbCO3(s)? 40. Which interval on the potential energy diagram shown below represents the DH of the reaction a + b c + d? A) [Pb 2+ ](aq) will decrease and the mass of PbCO3(s) Will decrease. B) [Pb 2+ ](aq) will decrease and the mass of PbCO3(s) will increase. C) [Pb 2+ ](aq) will increase and the mass of PbCO3(s) will decrease. D) [Pb 2+ ](aq) will increase and the mass of PbCO3(s) will increase. A) 1 B) 2 C) 3 D) 4 Page 6

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