Propose an interpretation of the values of the enthalpy and entropy of the overall reaction. Why are ΔS and ΔH positive (negative)?
The overall reaction: Zn(Hg) (l) + PbSO4(s) --> Zn2+(m) + SO42-(m) + Pb(Hg) (l).
Where 'm' denotes the molality of the ion in aqueous solution.
From the above reaction we can easily predict about the entropy .
AS we can see that on the reactant side one compound is solid while other are in liquid and there are total two components here while on the product side there are three components and all are in liquid form ,So the entropy of product is higher in comparison to the reactants
Now coming to the enthalpy part on going from reactants to products there are two bonds are breaking and one bond is forming ,apart from that the zinc and sulphate ions are solvated so the overall energy will be negative i.e the energy will be released which means that
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