cobalt complexes. You may refer to the experimental procedure. CoCla2-(ag) + 6H2
ID: 551231 • Letter: C
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cobalt complexes. You may refer to the experimental procedure. CoCla2-(ag) + 6H204C1+ Co(H2O)62@g) + energy 8. Data Table #3. Change to the DropsVisual Observations products, to reactants, Shift in the Reaction(to Reaction added or no change Test tube 1:CoCl2+ pink water Test tube I: CoCh+4 purple Shift to the left toward reactants water + concentrated Test tube 2: CoClz water + heat Test tube 2: CoCl2+ water + ice bath Test Tube 3: CoClh + AgNO Test Tube 4: CoClh + KNO purple pink Pink cloudy Pink clear Shift to the left toward reactants Shift to the right toward products Shift to the right toward products Shift to the right toward products 4 9. Using equation 5 (page 38), interpret your observations in terms of Le Châtelier's principle when you placed the test tube containing the pink solution in a hot water bath. PART D-The Equilibria of Saturated SolutionsExplanation / Answer
the shifts in reaction can be understood using Le Chatelier's principle which states that any change at equilibrium will make system readjust so as to counter the effect of changes and in the process a new equilibrium state is reached
in test tube 1 : on addition, the concentrations of components on right hand side increases therefore to restore equilibrium reaction shifts backwards
in test tube 2": heat is added, since the reaction is exothermic , on addition of any further heat will push the system to backward direction
test tube 2 , ice bath: on putting test tube in an ice bth, temperatures will comedown therefore more heat is required to restore system, and since it is exothermic reaction, reaction will move in forward direction
test tube 3: on addition of AgNO3 , AgCl will precipitate , thereforem more chloride ion will get consumed and hence reaction wil move in forward direction
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