Consider the endothermic reaction Fe^3+ (aq) + Cl^- (aq) FeCl^2+ (aq). Use lesst

Question

Consider the endothermic reaction Fe^3+ (aq) + Cl^- (aq) FeCl^2+ (aq). Use lessthanorequalto Chatelier's principle to predict how the equilibrium concentration of the complex ion FeCl^2+ will change after the following changes. Fe(NO_3)_3 is added. The [FeCl^2+] will increase. The [FeCl^2+] will decrease. The [FeCl^2+] will remain the same. Cl^- is precipitated as AgCl by addition of AgNO_3. The [FeCl^2+] will increase. The [FeCl^2+] will decrease. The [FeCl^2+] will remain the same. The temperature is increased. The [FeCl^2+] will increase. The [FeCl^2+] will decrease. The [FeCl^2+] will remain the same.

Explanation / Answer

Part A:

Ans : A

Fe(NO3)3 is added. So reactant concentration is increased, to maintain the equlibrium the reactants are transformed into product results FeCl2+ concentration increases.

Part B:

Ans : B.

AgNO3 is added means chlorine will react with AgNO3 gives AgCl. So chlorine concentration decreases, to maintain equlibrim backward reaction takes pleace results FeCl2+ concentration decreases.

Part C;

Ans: A.

The reaction is endothermic. If you increase the temperature, the heat absorbed by the reactants, forward reaction takes place results FeCl2+ concentration increases.

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