Problem: When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+ (ag) + Cl - (aq) → AgCI(s)       Δ H = - 65.5 kJ a) Calculate ΔH (kJ) for formation of 0.430 mol of AgCl by this reaction.  b) Calculate ΔH (kJ) for the formation of 6.00 g of AgCl.c) Calculate ΔH (J) when 9.23 x 10-4 mol of AgCI dissolves in water.

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FREE Expert Solution

First, we have to take note that we were given the standard enthalpy of formation for  AgCI(s)  and this is for 1 mole of  AgCI(s). 

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When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates:

 Ag+ (ag) + Cl - (aq) → AgCI(s)       Δ H = - 65.5 kJ 

a) Calculate ΔH (kJ) for formation of 0.430 mol of AgCl by this reaction.  

b) Calculate ΔH (kJ) for the formation of 6.00 g of AgCl.

c) Calculate ΔH (J) when 9.23 x 10-4 mol of AgCI dissolves in water.


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