January 2012 Chemistry Regents #79-81

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Questions 1-10 Questions 11-20 Questions 21-30 Questions 31-40 Questions 41-50 Questions 51-54 Questions 55-57 Questions 58-59 Questions 60-62 Questions 63-65 Questions 66-69  Questions 70-71  Questions 72-74 Questions 75-78  Questions 79-81  Questions 82-85

Question

Base your answers to questions 79 through 81 on the information below.   Several steps are involved in the industrial production of sulfuric acid. One step involves the oxidation of sulfur dioxide gas to form sulfur trioxide gas. A catalyst is used to increase the rate of production of sulfur trioxide gas. In a rigid cylinder with a movable piston, this reaction reaches equilibrium, as represented by the equation below. 2SO2(g) + O2(g) <==> 2SO3(g) + 392 kJ 79 Explain, in terms of collision theory, why increasing the pressure of the gases in the cylinder increases the rate of the forward reaction. [1] HIGHLIGHT TO SEE THE ANSWER When the pressure in the cylinder is increased, the SO2(g) molecules and O2(g) molecules collide more frequently, producing more SO3(g). or reactants collide more 80 Determine the amount of heat released by the production of 1.0 mole of SO3(g). [1] HIGHLIGHT TO SEE THE ANSWER 196kJ from 1SO3 /2SO3=  x kJ / 392 kJ 81 State, in terms of the concentration of SO3(g) , what occurs when more O2(g)  is added to the reaction at equilibrium. [1] HIGHLIGHT TO SEE THE ANSWER Concentration of SO3 increases   on to Questions 82-85

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