3. Given the reaction Fe2C () FeCl2 (02) a. Predict what would happen to the sys

Question

3. Given the reaction Fe2C () FeCl2 (02) a. Predict what would happen to the system at equilibrium if the concentration of C was increased. Which direction will equili b. Predict what would happen to the system at equilibrium if the concentration of Fe was decreased. Which direction will equilibrium shift? Predict what would happen to the system at equilibrium if the concentration of FeCl was increased. Which direction will equilibrium shift? c. Predict what would happen to the system at equilibrium if the concentration of FeCl was decreased. Which direction will equilibrium shift? d.

Explanation / Answer

A. If we increase the concentration of Cl-, more Cl- will be available to combine with Fe2+ and form FeCl2. So, the reaction will move forward. Or the equilibrium qilw shift forward.

B. If Fe2+ is decreased, the reaction will try to oppose this and will move backwards, to form more Fe2+, i.e the equilibrium will shift backwards.

C. If the concentration of FeCl2 is increased , more Fecl2 will be available to dissociate and hence the reaction will move backwards.

D. It is just opposite to the earlier , this time the reaction will move forward to form more FeCl2 and the equilibrium will shift forward.

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