For the following equilibrium reaction, when the forward reaction is exothermic; an increase in temperature shifts the equilibrium position towards the left. What will occur in that scenario?2SO2 + O2 ⇌ 2SO3
Correct answer: A. The concentrations of SO2 and O2 increases and concentration of SO3 decreases as the temperature increases.
- A. The concentrations of SO2 and O2 increases and concentration of SO3 decreases as the temperature increases.
- B. The concentrations of SO3, SO2, and O2 increase as the temperature increases.
- C. The concentrations of SO2 and O2 decreases and concentration of SO3 increases as the temperature increases.
- D. The concentrations of SO2 and O2 and SO3 remains the same as the temperature increases.
Explanation
Since the equilibrium of the reaction shifts to the left, this means that the left hand side of the reaction is favoured. Increasing the reactants (LHS) and decreasing the products (RHS). Le Chatelier's principle will be used.
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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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