a)

Co(H2O)6^2 + 4 Cl^‐1 (aq) ⇄ CoCl4^‐2 (aq) + 6 H2O (l)

Rewrite the net ionic equation above including the energy term where appropriate. The Delta H for this reaction is +50 kJ/mol.

b)

Silver chloride (AgCl) is a white solid. For the equilibrium reaction AgCl(s) = Ag+(aq) + Cl‐(aq) The Ksp for AgCl = 1.6 * 10‐10. At equilibrium, would you expect to have more silver and chloride ions or more solid silver chloride?

Co(H2O)6^2 + 4 Cl^‐1 (aq) ⇄ CoCl4^‐2 (aq) + 6 H2O (l) + 50 kJ

AgCl(s) = Ag+(aq) + Cl‐(aq)
1.6E-10 = (Ag^+)(Cl^-)
If the right side is only 1.6E-10, doesn't that mean there is much more solid than ions?

a) To rewrite the net ionic equation, we need to cancel out the spectator ions, which are the ions that appear on both sides of the equation and do not participate in the chemical reaction.

The net ionic equation for the given reaction would be:
Co(H2O)6^2+(aq) + 4Cl^-(aq) ⇄ CoCl4^2-(aq)

Since this is a dissolution reaction, there is no direct involvement of energy terms like heat or enthalpy. The energy term you mentioned, Delta H (+50 kJ/mol), is the enthalpy change for the reaction, but it does not appear in the net ionic equation.

b) The Ksp (solubility product constant) for AgCl is a measure of the equilibrium between the solid silver chloride and the dissolved Ag+ and Cl- ions. It tells us the tendency for the solid AgCl to dissolve.

In this case, the Ksp value for AgCl is 1.6 * 10^-10. This value is very small, indicating that AgCl has a low solubility in water. At equilibrium, the system will try to minimize the dissolution of AgCl and maintain a higher concentration of solid AgCl.

Therefore, at equilibrium, we would expect to have more solid silver chloride (AgCl) than dissolved Ag+ and Cl- ions.

a) The net ionic equation for the given reaction is:

Co(H2O)6^2+ (aq) + 4 Cl^-(aq) ⇄ CoCl4^-(aq) + 6 H2O(l)

The energy change (ΔH) for this reaction is +50 kJ/mol.

b) The equilibrium reaction is:

AgCl(s) ⇄ Ag+(aq) + Cl^-(aq)

The Ksp (solubility product constant) for AgCl is 1.6 × 10^-10.

Based on the magnitude of the Ksp, we can determine the relative concentrations at equilibrium. Since the Ksp is very small, it indicates that the dissociation of AgCl to form Ag+ and Cl- ions is favored. Therefore, at equilibrium, we would expect to have a higher concentration of silver and chloride ions (Ag+ and Cl-) compared to solid silver chloride (AgCl).