Consider the dissolution reactions below for the simple salts NaCl (s), AgCl (s), and CaCl2​ (s). The ΔG∗ values for the

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Consider the dissolution reactions below for the simple salts NaCl (s), AgCl (s), and CaCl2​ (s). The ΔG∗ values for the formation of their aqueous ions is also given. NaCl⇌Na((aq) ∗​+Cl (oa) ΔG∗=−9.1 kJ mol−1 AgCl⇌Ag∗(aas )​+Cl(aa) ​ΔG∗=+55.6 kJ mol−1 CaCl2​⇌Ca2∗(ma)+2Cl(a) )​ΔG∘=−67.98 kJ mol−1 (i) Given the ΔG*  values, roughly sketch the Gibbs function vs the extent of the reaction for each of the dissolution reactions. (ii) Calculate the Kea for the respective salts at 298 K. Explain your answer using the Keq obtained. ​ obten (iii) When NaCl is dissolved in water. The temperature of the solution goes down. The opposite is seen when dissolving CaCl2 in water. The temperature of the solution increases. Fully explain why this happens. (iv) How will the ΔG∘ of the dissolution of the salts change with increasing temperature? Q 4(b) [10 Marks] (i) Draw a schematic of a bomb calorimeter and outline a procedure for its use. The drawing should highlight the name and function of each component of the device. (ii) The combustion of 0.67 g of naphthalene, C10​H8​, in a bomb calorimeter pressurized with oxygen at 298 K resulted in a temperature increase of 2.424 K. Under the same conditions, supplying 20.250 kJ of energy to the bomb calorimeter raised the temperature by 1.890 K. Hence calculate enthalpy of combustion (ΔHc​) and the molar enthalpy of combustion (ΔHc,m​) for naphthalene.