Oxidation of SO2 by O2 is exothermic reaction. The yield of SO3 will be maximum if:
Correct answer: B. Temperature is reduced and pressure is increased
- A. Temperature is increased and pressure is kept constant
- B. Temperature is reduced and pressure is increased
- C. Both temperature and pressure are increased
- D. Both temperature and pressure are decreased
Explanation
A decreased temperature will favor the exothermic forward reaction (production of SO3), and increased pressure will favor the side with less number of moles that is the product side SO3 in this case. Thus, the yield is at maximum.
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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