Write the dissolution reaction for manganese(II) chloride in water. Use the pull-down menus to specify the state of each reactant and product. + Is manganese(II) chloride considered soluble or not soluble ? ... ... A. Soluble ... B. Not soluble Based upon this, the equilibrium constant for this reaction will be: ... ... A. Greater than 1 ... B. Less than 1

See explanation for detailed answer.

Explanation:

MnCl2(s) + 6H2O <> [Mn(H2O)6]2+(aq) + 2Cl- (aq)

MnCl2 is soluble in water hence the equilibrium constant for the reaction will be greater than one.

It dissolves in water to form the complex stated above thereby tilting the pH of the solution towards the slightly acidic end.

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.

i think   the answer is c hope i'm right