The romans used calcium oxide, cao, to produce a strong mortar to build stone structures. calcium oxide was mixed with water to give calcium hydroxide, which reacted slowly with carbon dioxide in the air to give calcium carbonate. ca(oh)2(s) + co2 → caco3(s) + h2o(g) calculate the standard enthalpy change for this reaction. kj/mol-rxn what is the change in enthalpy if 3.50 kg of calcium hydroxide reacts with a stoichiometric amount of carbon dioxide? kj

ΔH°rxn = -68.7 kJ/mol

ΔH = -3249.5 kJ

Explanation:

The standard enthalpy change of the reaction (ΔH°rxn) can be calculated by the standard enthalpy of formation of the compounds (H°f), which can be found in thermodynamics tables.

H°f, Ca(OH)₂(s) = -986.6 kJ/mol

H°f, CO₂(g) = -393.5 kJ/mol

H°f, CaCO₃(s) =-1207.0 kJ/mol

H°f, H₂O(g) = -241.8 kJ/mol

ΔH°rxn = ∑n*H°f, products - ∑n*H°f,reactants (where n is the number of moles in the balanced equation).

ΔH°rxn = (-241.8 - 1207.0) - (-393.5 - 986.6)

ΔH°rxn = -68.7 kJ/mol

The molar mass of calcium hydroxide is 74 g/mol (Ca = 40 g/mol, O = 16 g/mol, and H = 1 g/mol), so the number of moles, is the mass (3500g) divided by the molar mass:

n = 3500/74 = 47.3 moles

The change in enthalpy is the standard enthalpy of the reaction multiplied by the number of moles of the limiting reactant. Because stoichiometry is 1:1, and they have the same amount of moles, there's no reactant in excess:

ΔH = -68.7 * 47.3

ΔH = -3249.5 kJ

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