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salam
can anyone please explain q1(c) partts (i) and (ii) from May June 2012 paper 42
http://papers.xtremepapers.com/CIE/Cambridge International A and AS Level/Chemistry (9701)/9701_s12_qp_42.pdf
ci) The enthalpy change of solution represents the change of state of an ionic compound from solid to aqueous form. This change corresponds to the difference in energy values for ΔHf MgCl2(s) and ΔHf mgCl2 (aq) as it represents the exact same state change.
So, ΔHsol = -801 - (-641) = -160 KJ/mol
ii) Use the answer form (i) for the formula in (ii). The hydration enthalpy of Cl- should be multiplied by 2 as one mole MgCl2 gives 2 mols of Cl- ions.
ΔHsol (MgCl2) = {2*ΔHhyd(Cl-) + ΔHhyd(Mg2+)} - ΔHlatt(MgCl2)
-160 = 2* ΔHhyd(Cl-) + (-1890) - (-2526)
Therefore, ΔHhyd(Cl-) = (-160 + 1890 - 2526)/2 = -398 Kj/mol