The exothermic formation of ClF3 is represented by the equation:Cl2 (g) + 3F2 (g) ⇋ 2ClF3 (g) ΔH=-329kJWhich of the following will increase the quantity of ClF3 in an equilibrium mixture of F2,Cl2 and ClF3?
Correct answer: A. Adding F2
- A. Adding F2
- B. Increasing the volume of the container
- C. Removing Cl2
- D. Increasing the temperature
Explanation
The correct answer is to add F2. According to Le Chatelier's Principle, adding more of a reactant shifts the equilibrium towards the products to counteract the change, increasing the concentration of ClF3. Increasing the volume of the container decreases the pressure, which shifts the equilibrium towards the reactants (since there are more moles of gas on the reactant side), thus reducing ClF3 production. Removing Cl2 decreases its concentration, causing the equilibrium to shift towards the reactants to replace the missing Cl2, also reducing ClF3 production. Increasing the temperature shifts the equilibrium towards the reactants because the reaction is exothermic, thus also reducing ClF3 production.
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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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