5. Consider the following reaction to answer the questions below (you can use ar

Question

5. Consider the following reaction to answer the questions below (you can use arrows up or down to indicate increase or decrease, or write "no change" if there is no change): Pb(NO3)209) +2KIa) 2KNOs(a) + Pbl2s)Endothermic A. What will happen to the concentration of KNOs when KI is added? B. What will happen to the concentration of Pbl2 if Pb(NO3)2 is removed from the system? C. what will happen to the concentration of KI if the reaction is heated? D. What will happen to the concentration of Pb(NOs)2 if solid KI is added to the system? (Assume the reactant solutions are unsaturated.)

Explanation / Answer

Answer A : When KI is added to the solution at equillibrium, the equillibrium will get disturbed and hence according to Le Chatliers principle, equillibrium will try to restore itself by decreasing the concentration of KI. Hence equillibrium will shift to forward direction and so the concentration of KNO3 will be increased.

Answer B: If Pb(NO3)2 will be removed from the system, then again from the Le Chatalier's principle, the equillibrium will try to restore the concentration of Pb(NO3)2 and hence will shift to backward direction. thus more amount of PbI2 will be utilized hence its concentration will decrease.

Answer C: As the nature of the reaction is endothermic, increase in temperature will cause a shift of equillibrium in the forward direction in order to decrease the effect of increased temperature. Hence the concentration of KI will be reduced.

Answer D: As KI is added to a solution which is still unsaturated, more KI will get dissolved which will increase the concentration of KI. hence the equillibrium will sift to forward direction leading to the decrease in concentration of Pb(NO3)2

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