Full solution please a) When 2.76 g of potassium carbonate was added to 30.0 cm³ of approximately 2 mol dm-3hydrochloric acid, the temperature rose by 5.20 °C.(i) Write an equation, including state symbols, for this reaction.(ii) Calculate the enthalpy change for this reaction per mole of potassium carbonate. Assumethat the specific heat capacity and density of all solutions are 4.18 J g-1K-1 and 1.00 g cm3respectively.(iii) Explain why the hydrochloric acid need only be approximately 2 mol dm-3.b) When 2.00 g of potassium hydrogencarbonate was added to 30.0 cm3 of the same hydrochloricacid, the temperature fell by 3.70 °C.(i) Write an equation, including state symbols, for this reaction.(ii) Calculate the enthalpy change for this reaction per mole of potassium hydrogencarbonate.c) When potassium hydrogencarbonate is heated, it decomposes into potassium carbonate, carbondioxide and water. By applying Hess' Law and your results in (a) and (b), calculate the enthalpychange for the decomposition of potassium hydrogencarbonate.

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a) When 2.76 g of potassium carbonate was added to 30.0 cm3 of approximately 2 mol dm hydrochloric acid, the temperature rose by 5.20 °C. -3 (i) Write an equation, including state symbols, for this reaction. (ii) Calculate the enthalpy change for this reaction per mole of potassium carbonate. Assume that the specific heat capacity and density of all solutions are 4.18 J g1K-1 and 1.00 g cm3 respectively. (iii) Explain why the hydrochloric acid need only be approximately 2 mol dm-3.