How is this solved? Im using Chem101

Question

What is the change in enthalpy in joules when 5.44x10^-4mol of AgCl solid dissolves in water according to the following chemical equation: AgCl(s) -> Ag⁺(aq) + Cl^-(aq) H=65.5 kJ

Answer 1

The way you use ΔH_rxn of any reaction to find the heat given off or absorbed is to multiply the moles of the species in the equation times the ΔΗ_rxn/(stoichiometric coefficient of that reactant):

5.44 x 10^-4 moles of AgCl * (65.5 kJ/ 1 mole of AgCl) =

The question should really be what is the heat absorbed when so many moles of AgCl are dissolved?

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