N 2 + 3H 2 2NH 3 + heat

Transcription

1 1. In which reaction will the point of equilibrium shift to the left when the pressure on the system is increased? 1) C(s) + O 2 (g) CO 2 (g) 2) CaCO 3 (s) CaO(s) + CO 2 (g) 3) 2Mg(s) + O 2 (g) 2MgO(s) 4) 2H 2 (g) + O 2 (g) 2H 2 O(g) 2. Ammonia is produced commercially by the Haber reaction: N 2 (g) + 3H 2 (g) 2NH 3 (g) + heat The formation of ammonia is favored by 1) an increase in pressure 2) a decrease in pressure 3) removal of N 2 (g) 4) removal of H 2 (g) Base your answers to questions 3 and 4 on the following system at equilibrium: 2CI 2 (g) + 2H 2 O(g) 4HCl(g) + O 2 (g) H = +27 kcal. 3. If O 2 is added to the system at a constant pressure and temperature, the number of moles of HCl will 4. If the temperature of the system is increased at a constant pressure, the rate of the forward reaction will 5. Given the reaction at equilibrium: PbCl 2 (s) Pb 2 + (aq) + 2Cl (aq) When KCl(s) is added to the system, the equilibrium shifts to the 1) right, and the concentration of Pb 2+ (aq) ions decreases 2) right, and the concentration of Pb 2+ (aq) ions increases 3) left, and the concentration of Pb 2+ (aq) ions decreases 4) left, and the concentration of Pb 2+ (aq) ions increases 6. Given the Haber reaction at equilibrium: N 2 (g) + 3H 2 (g) 2NH 3 (g) + heat Which stress on the system will decrease the production of NH 3 (g)? 1) increasing the concentration of N 2 (g) 2) increasing the pressure on the system 3) decreasing the concentration of H 2 (g) 4) decreasing the temperature on the system 7. Given the reaction at STP and at equilibrium: AgI(s) Ag + (aq) + I (aq) What will occur when AgNO 3 (s) is added to the equilibrium mixture? 1) The amount of AgI(s) will decrease, and the amount of I (aq) will decrease. 2) The amount of AgI(s) will decrease, and the amount of I (aq) will increase. 3) The amount of AgI(s) will increase, and the amount of I (aq) will decrease. 4) The amount of AgI(s) will increase, and the amount of I (aq) will increase. 8. Given the reaction at equilibrium: SO 2 (g) + NO 2 (g) = SO 3 (g) + NO(g) The amount of SO 3 (g) will increase if the concentration of 1) NO(g) increases 2) SO 2 (g) increases 3) NO 2 (g) decreases 4) SO 2 (g) decreases 9. Given the reaction for the Haber process: N 2 + 3H 2 2NH 3 + heat The temperature of the reaction is raised in order to 1) increase the percent yield of nitrogen the rate of formation of ammonia 3) affect the forward reaction rate most 4) affect the reverse reaction rate least 10. Given the reaction at equilibrium: N 2 (g) + 3H 2 (g) 2NH 3 (g) + 22 kcal Which stress would cause the equilibrium to shift to the left? 1) increasing the temperature 2) increasing the pressure 3) adding N 2 (g) to the system 4) adding H 2 (g) to the system 11. Given the reaction at equilibrium: C(s) + CO 2 (g) + heat 2CO(g) Which stress on the system would favor the production of CO(g)? 1) a decrease in the amount of C(s) 2) a decrease in the amount of CO 2 (g) 3) an increase in the pressure 4) an increase in the temperature 12. Which system at equilibrium will be least affected by a change in pressure? 1) 3H 2 (g) + N 2 (g) 2NH 3 (g) 2) 2S(s) + 3O 2 (g) 2SO 3 (g) 3) AgCl(s) Ag + (aq) + Cl (aq) 4) 2HgO(s) 2Hg( ) + O 2 (g)

2 13. Given the reaction at equilibrium: 2SO 2 (g) + O 2 (g) 2SO 3 (g) If the temperature remains constant, an increase in pressure will 1) have no effect on the equilibrium 2) shift the equilibrium to the right 3) shift the equilibrium to the left 4) change the value of the equilibrium constant 14. Given the system at equilibrium: PbCO 3 (s) Pb 2+ (aq) + CO 3 2 (aq) How will the addition of Na 2 CO 3 (aq) affect [Pb 2+ ](aq) and the mass of PbCO 3 (s)? 1) [Pb 2+ ] (aq) will decrease and the mass of PbCO 3 (s) Will decrease. 2) [Pb 2+ ] (aq) will decrease and the mass of PbCO 3 (s) will increase. 3) [Pb 2+ ] (aq) will increase and the mass of PbCO 3 (s) will decrease. 4) [Pb 2+ ] (aq) will increase and the mass of PbCO 3 (s) will increase. 15. Given the system at equilibrium: AgCl(s) Ag + (aq) + Cl (aq) When NaCl(s) is added to the system, the equilibrium will shift to the 1) right and the concentration of AgCl(s) will decrease 2) right and the concentration of AgCl(s) will increase 3) left and the concentration of Ag + (aq) will decrease 4) left and the concentration of Ag + (aq) will increase 16. The reaction A(g) + B(g) C(g) is occurring in the apparatus shown below. The rate of reaction can be decreased by increasing the 1) pressure on the reactants 2) temperature of the reactants 3) concentration of reactant A(g) 4) volume of the reaction chamber 17. Given the reaction at equilibrium: N 2 (g) + O 2 (g) kcal NO(g) The equilibrium will shift to the right if the 1) temperature increases 3) pressure increases 2) temperature decreases 4) pressure decreases 18. Given the system at equilibrium: CaSO 4 (s) Ca 2+ (aq) + SO 2 4 (aq) If K 2 SO 4 (s) is added and the temperature remains constant, the Ca 2+ (aq) concentration will 1) decrease, and the amount of CaSO 4 (s) will decrease 2) decrease, and the amount of CaSO 4 (s) will increase 3) increase, and the amount of CaSO 4 (s) will decrease 4) increase, and the amount of CaSO 4 (s) will increase 19. Given the balanced equation, which represents the Haber process: N 2 (g) + 3H 2 (g) 2NH 3 (g) Which effect will an increase of pressure have on the system? 1) a decrease in the amount of NH 3 and a decrease in the amount of N 2 2) a decrease in the amount of NH 3 and an increase in the amount of N 2 3) an increase in the amount of NH 3 and a decrease in the amount of N 2 4) an increase in the amount of NH 3 and an increase in the amount of N Given the reaction at equilibrium: N 2 (g) + O 2 (g) 2NO(g) As the concentration of N 2 (g) increases, the concentration of O 2 (g) will 21. Given the reaction at equilibrium: N 2 (g) + 3H 2 (g) 2NH 3 (g) If the pressure is increased at constant temperature, there will be an increase in the number of moles of 1) NH 3 (g), only 2) N 2 (g), only 3) H 2 (g), only 4) both N 2 (g) and H 2 (g) 22. Given the reaction: N 2 (g) + 3H 2 (g) 2NH 3 (g) + energy If the temperature is increased and the pressure is kept constant, the new equilibrium concentration will be 1) less for NH 3 (g) 2) the same for NH 3 (g) 3) less for N 2 (g) 4) the same for N 2 (g) 23. Given the reaction at equilibrium: A(g) + B(g) + heat C(g) + D(g) The equilibrium will shift to the right when the 1) pressure is decreased 2) temperature is increased 3) concentration of A(g) is decreased 4) concentration of C(g) is increased 24. In the equilibrium reaction: A(g) + 2B(g) + heat AB 2 (g) the rate of the forward reaction will increase if there is 1) an increase in pressure 2) an increase in the volume of the reaction vessel 3) a decrease in temperature 4) a decrease in the concentration of A (g)

3 25. Given the reaction at equilibrium: NaCl(s) Na + (aq) + Cl (aq) The addition of KCl to this system will cause a shift in the equilibrium to the 1) left, and the concentration of the Na + (aq) ions will increase 2) right, and the concentration of the Na + (aq) ions will increase 3) left, and the concentration of the Na + (aq) ions will decrease 4) right, and the concentration of the Na + (aq) ions will decrease 26. Given the reaction: N 2 (g) + O 2 (g) kj 2 NO(g) Which change would cause an immediate increase in the rate of the forward reaction? 1) increasing the concentration of NO(g) 2) increasing the concentration of N 2 (g) 3) decreasing the reaction temperature 4) decreasing the reaction pressure 27. Given the reaction: CO(g) + O 2 (g) CO 2 (g) kcal As the temperature increases, the rate of the forward reaction s 28. Given the reaction at equilibrium: N 2 (g) + 3H 2 (g) * 2NH 3 (g) + heat At constant temperature, which changes would produce a greater yield of NH 3 (g)? 1) decreasing the pressure and decreasing the concentration of N 2 (g) 2) decreasing the pressure and increasing the concentration of N 2 (g) 3) increasing the pressure and decreasing the concentration of N 2 (g) 4) increasing the pressure and increasing the concentration of N 2 (g) 29. Given the system at equilibrium: AgCl(s) Ag + (aq) + Cl (aq) When 0.1 M HCl is added to the system, the point of equilibrium will shift to the 1) right and the concentration of Ag + will decrease 2) right and the concentration of Ag + will increase 3) left and the concentration of Ag + (aq) will decrease 4) left and the concentration of Ag + (aq) will increase 30. The addition of a catalyst to a system at equilibrium will increase the rate of 1) the forward reaction, only 2) the reverse reaction, only 3) both the forward and reverse reactions 4) neither the forward nor reverse reaction 31. Given the closed system at equilibrium: CO 2 (g) CO 2 (aq) As the pressure on the system increases, the solubility of the CO 2 (g) s 32. Given the equilibrium system: 2A(g) + B(g) + 10 kcal C(g) Which conditions would yield the most product? 1) low temperature and high pressure 2) low temperature and low pressure 3) high temperature and high pressure 4) high temperature and low pressure 33. Given the reaction at equilibrium: N 2 (g) + 3H 2 (g) 2NH 3 (g) + heat Which change favors the formation of ammonia? 1) increasing the concentration of N 2 (g) 2) increasing the volume of the reaction vessel 3) decreasing the pressure 4) decreasing the H 2 (g) concentration 34. Given the reaction at equilibrium: X + Y 2Z + heat The concentration of the product could be increased by 1) adding a catalyst 2) adding more heat to the system 3) increasing the concentration of Y 4) decreasing the concentration of X 35. Given the reaction at equilibrium: C(s) + O 2 (g) CO 2 (g) + heat Which stress on the system will increase the concentration of CO 2 (g)? 1) increasing the temperature of the reaction 2) increasing the concentration of O 2 (g) 3) decreasing the pressure on the reaction 4) decreasing the amount of C(s) 36. Given the equilibrium reaction: N 2 (g) + O 2 (g) 2NO(g) An increase in pressure produced by a decrease in volume at constant temperature would produce an increase in the concentration of 1) N 2, only 2) NO, only 3) N 2 and O 2, only 4) N 2, O 2, and NO 37. Given the system, CO 2 (s) CO 2 (g) at equilibrium. As the pressure increases at constant temperature, the amount of CO 2 (g) will

4 38. Given the reversible reaction A(g) + B(g) C(g) at equilibrium. If the concentration of A is increased at constant temperature and pressure, which will also increase? 1) the rate of the forward reaction 2) the value of the equilibrium constant 3) the activation energy 4) the concentration of B 39. Given the reaction at equilibrium: A(g) + B(g) C(g) + D(g) The addition of a catalyst will 1) shift the equilibrium to the right 2) shift the equilibrium to the left 3) increase the rate of forward and reverse reactions equally 4) have no effect on the forward or reverse reactions 40. Given the reaction at equilibrium: H 2 (g) + Cl 2 (g) 2HCl(g) As the pressure increases at constant temperature, the number of moles of HCl s 41. Given the reaction at equilibrium: BaCrO 4 (s) Ba 2+ (aq) + CrO 2 4 (aq) Which substance, when added to the mixture will cause an increase in the amount of BaCrO 4 (s)? 1) K 2 CO 3 2) CaCO 3 3) BaCl 2 4) CaCl Given the reaction at equilibrium: 2A(g) + 3B(g) A 2 B 3 (g) + heat Which change will not affect the equilibrium concentrations of A(g), B(g), and A 2 B 3 (g)? 1) adding more A(g) 2) adding a catalyst 3) increasing the temperature 4) increasing the pressure 43. Given the system at equilibrium: N 2 O 4 (g) kj * 2 NO 2 (g) What will be the result of an increase in temperature at constant pressure? 1) The equilibrium will shift to the left, and the concentration of NO2(g) will decrease. 2) The equilibrium will shift to the left, and the concentration of NO2(g) will increase. 3) The equilibrium will shift to the right, and the concentration of NO2(g) will decrease. 4) The equilibrium will shift to the right, and the concentration of NO2(g) will increase. 44. Given the reaction at equilibrium: 2SO 2 (g) + O 2 (g) 2SO 3 (g) + heat Which change will shift the equilibrium to the right? 1) decreasing [SO 2 ] 2) decreasing the pressure 3) increasing [O 2 ] 4) increasing the temperature 45. Given the reaction at equilibrium: 2SO 2 (g) + O 2 (g) 2SO 3 (g) + heat The concentration of SO 3 (g) may be increased by 1) decreasing the concentration of SO 2 (g) 2) decreasing the concentration of O 2 (g) 3) increasing the pressure 4) increasing the temperature 46. For a given system at equilibrium, lowering the temperature will always 1) increase the rate of reaction the concentration of products 3) favor the exothermic reaction 4) favor the endothermic reaction 47. Given the reaction at equilibrium: 2CO(g) + O 2 (g) 2CO 2 (g) When the reaction is subjected to stress, a change will occur in the concentration of 1) reactants, only 2) products, only 3) both reactants and products 4) neither reactants nor products 48. Given the reaction at equilibrium: 2SO 2 (g) + O 2 (g) 2SO 3 (g) As the pressure is increased at constant temperature, the number of moles of SO 3 (g) produced will 49. Given the reaction at equilibrium: X 2 (g) + 2Y 2 (g) 2XY 2 (g) + 80 kcal The equilibrium point will shift to the right if the pressure is 1) increased and the temperature is increased d and the temperature is decreased 3) decreased and the temperature is increased 4) decreased and the temperature is decreased 50. Given the system at equilibrium: H 2 (g) + F 2 (g) * 2HF(g) + heat Which change will not shift the point of equilibrium? 1) changing the pressure 2) changing the temperature 3) changing the concentration of H 2 (g) 4) changing the concentration of HF(g) 51. Given the reaction at equilibrium: N 2 (g) + 3H 2 (g) 2NH 3 (g) + Heat Which change would shift the equilibrium to the right? 1) Increase the temperature. 2) Increase the pressure. 3) Decrease the [N 2 ] 4) Decrease the [H 2 ]

5 52. Given the reaction at equilibrium: C 2 (g) + D 2 (g) 2CD(g) + energy Which change will cause the equilibrium to shift? 1) increase in pressure 3) addition of heat in volume 4) addition of a catalyst 53. Given the solution at equilibrium: PbI 2 (s) Pb 2+ (aq) + 2I (aq) The addition of which nitrate salt will cause a decrease in the concentration of I (aq)? 1) Pb(NO 3 ) 2 2) Ca(NO 3 ) 2 3) LiNO 3 4) KNO Given the equilibrium reaction in a closed system: H 2 (g) + I 2 (g) + heat 2 HI(g) What will be the result of an increase in temperature? 1) The equilibrium will shift to the left and [H 2 ] will increase. 2) The equilibrium will shift to the left and [H 2 ] will decrease. 3) The equilibrium will shift to the right and [HI] will increase. 4) The equilibrium will shift to the right and [HI] will decrease. 55. Given the reaction at equilibrium: N 2 (g) + O 2 (g) + energy * 2NO(g) Which change will result in a decrease in the amount of NO(g) formed? 1) decreasing the pressure 2) decreasing the concentration of N 2 (g) 3) increasing the concentration of O 2 (g) 4) increasing the temperature 56. The Haber process is represented by the equation: N 2 (g) + 3H 2 (g) 2NH 3 (g) + heat. Which set of conditions is used during this reaction to increase the reaction rate and to produce a reasonable yield of NH 3 (g)? 1) lowered temperature and lowered pressure, only 2) lowered temperature and raised pressure, only 3) raised temperature, raised pressure, and addition of a catalyst 4) raised temperature, lowered pressure, and addition of a catalyst 57. What will happen if a catalyst is added to the system at equilibrium? A + B AB 1) The equilibrium concentration of AB will increase. 2) The equilibrium concentration of AB will decrease. 3) The rates of the forward and reverse reactions will change. 4) The equilibrium constant for the reaction will change. 58. Given the reaction at equilibrium: 4HCl(g) + O 2 (g) 2Cl 2 (g) + 2H 2 O(g) If the pressure on the system is increased, the concentration of Cl 2 (g) will 59. Given the reaction at equilibrium: AgBr(s) Ag + (aq) + Br (aq) Which change occurs when KBr(s) is dissolved in the reaction mixture? 1) The amount of AgBr(s) decreases. 2) The amount of AgBr(s) remains the same. 3) The concentration of Ag + (aq) decreases. 4) The concentration of Ag + (aq) remains the same. 60. Given the reaction at equilibrium: N 2 + 3H 2 (g) 2NH 3 (g) + heat Which change will increase the amount of NH 3 (g) in the system? 1) an increase in the concentration of N 2 (g) 2) an increase in temperature 3) a decrease in the concentration of H 2 (g) 4) a decrease in pressure 61. Given the equilibrium reaction at constant pressure: 2HBr(g) kcal H 2 (g) + Br 2 (g) When the temperature is increased, the equilibrium will shift to the 1) right, and the concentration of HBr(g) will decrease 2) right, and the concentration of HBr(g) will increase 3) left, and the concentration of HBr(g) will decrease 4) left, and the concentration of HBr(g) will increase 62. Given the reaction: Zn(s) + HCl(aq) ZnCl 2 (aq) + H 2 (g) As the concentration of the HCl(aq) decreases at constant temperature, the rate of the reaction s 63. In which reaction at equilibrium will the point of equilibrium shift to the right when the pressure decreases at constant temperature? 1) N 2 (g) + 3H 2 (g) 2NH 3 (g) 2) H 2 (g) + Br 2 (g) 2HBr(g) 3) CaCO 3 (s) CaO(s) + CO 2 (g) 4) N 2 (g) + O 2 (g) 2NO(g) 64. Given the reaction at equilibrium: 2SO 2 (g) + O 2 (g) 2SO 3 (g) + heat Which change will shift the equilibrium to the right? 1) increasing the temperature 2) increasing the pressure 3) decreasing the amount of SO 2 (g) 4) decreasing the amount of O 2 (g)

6 65. Given the reaction at equilibrium: N 2 (g) + 3H 2 (g) 2NH 3 (g) Increasing the concentration of N 2 (g) will increase the forward reaction rate due to 1) a decrease in the number of effective collisions 2) an increase in the number of effective collisions 3) a decrease in the activation energy 4) an increase in the activation energy 66. Given the system at equilibrium: AgBr(s) Ag 1+ (aq) + Br 1 (aq) The addition of crystals of AgNO 3 (s) to the solution at constant temperature will result in 1) an increase in the concentration of Br (aq) 2) a decrease in the concentration of Br (aq) 3) an increase in the K sp value 4) a decrease in the K sp value 67. Given the reaction: A(g) + B(g) AB(g) As the pressure increases at a constant temperature, the rate of the forward reaction will 68. Given the solution at equilibrium: CaSO 4 (s) * Ca 2+ (aq) + SO 2-4 (aq) When Na 2 SO 4 is added to the system, how will the equilibrium shift? 1) The amount of CaSO 4 (s) will decrease, and the concentration of Ca 2+ (aq) will decrease. 2) The amount of CaSO 4 (s) will decrease, and the concentration of Ca 2+ (aq) will increase. 3) The amount of CaSO 4 (s) will increase, and the concentration of Ca 2+ (aq) will decrease. 4) The amount of CaSO 4 (s) Will increase, and the concentration of Ca 2+ (aq) will increase. 69. Given the reaction at equilibrium: BaSO 4 (s) Ba 2+ (aq) + SO 2 4 (aq) The concentration of SO 2 4 ions can be decreased by the addition of 1) BaSO 4 (s) 2) BaCl 2 (s) 3) Na 2 SO 4 (s) 4) NaNO 3 (s) 70. Which system at equilibrium will shift to the right when the pressure is increased? 1) 2) 3) 4) 71. Given a saturated solution of silver chloride at constant temperature: AgCl(s) Ag + (aq) + Cl (aq) As NaCl(s) is dissolved in the solution, the concentration of the Ag + ions in the solution 1) decreases, and the concentration of Cl ions increases 2) decreases, and the concentration of Cl ions remains the same 3) increases, and the concentration of Cl ions increases 4) increases, and the concentration of Cl ions remains the same 72. A saturated solution is represented by the equation AgCl(s) + heat Ag + (aq) + Cl (aq). Which change will cause an increase in the amount of AgCl(s)? 1) a decrease in pressure 2) an increase in temperature 3) a decrease in the concentration of Ag + (aq) 4) an increase in the concentration of Cl (aq) 73. Given the reaction at STP and at equilibrium: H 2 (g) + Cl 2 (g) 2HCl(g) Which change will result in an increase in the concentration of Cl 2 (g)? 1) decreasing the pressure of the system 2) decreasing the concentration of HCl(g) 3) increasing the concentration of H 2 (g) 4) increasing the concentration of HCl(g) 74. Given the reaction at equilibrium: H 2 (g) + Cl 2 (g) 2HCl(g) As the pressure increases at constant temperature, the mass of H 2 (g) s 75. Given the equilibrium reaction: 2SO 2 (g) + O 2 (g) 2SO 3 (g) + Heat When the pressure on the system in increased, the concentration of the SO 3 will

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