What is the Delta G degree_rxn for the precipitation of BaCI_2 (write the net io

Question

What is the Delta G degree_rxn for the precipitation of BaCI_2 (write the net ionic equation as well). b.) How does the Delta G degree_rxn above support or not support the net ionic equation that shows BaCI_2 will spontaneously precipitate when 1.0 M solutions of Ba_(aq) and CI_(aq) are mixed? Why? Under what temperature conditions (high/low) are endothermic processes spontaneous? Explain: Given the value of Delta G degree_rxn for Ca^2+ is -553.58 kJ/mol and the Delta F degree_rxn for carbonate is -563.63 kJ/mol. The value for Delta G degree_rxn for CaCO_3 is -1128.79 kJ/mol. Will a precipitate form when an equal volume of 0.20 M Ca^2+ solution is mixed with a volume of 0.20 M CO_3^2- solution (be careful here)? Calculate the Delta G_rxn and determine if a precipitation reaction will occur at room temperature (25.0 degree C) or not.

Explanation / Answer

1]Ba+2 + 2Cl- -----> BaCl2(s)

since BaCl2 is soluble it doesnt form a precipitate actualy[ it remains in ionic form]

Delta G value is postive for the precipitation

b]

I dont support the above reaction since BaCl2 is soluble in water and doesnt form precipitate .

They wont precipitate at all .since Delta G value is large and postive for the above reaction

2] delta G = delta H - T delta S

when delta G is negative the process will be spontaneous

deltha H is positive

At very high temperature endothermic reaction are spontaneous [ assuming delta S positive ]

3]

Ca+2 + CO3-2 ----> CaCO3(s)

delta G of reaction = delta G of products - delta G of reactants

= -11.58KJ/mol

At 25C

since delta G is negative , the reaction is spontaneous and the precipitation occurs.

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