Using the Kf value of 1.2x10^9 calculate the concentration of Ni^+2 (aq) and Ni(NH3)6^+2 that are present at equilibrium after dissolving 1.22g NiCl2 in 100.0 mL of NH3 (aq) solution such that the equilibrium concentration of NH3 is equal to 0.20 M

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.

false

because it does not have the potential to be entirely used up