H2O + CaO = Ca(OH)2H2O

H_2O water + CaO lime ⟶ Ca(OH)2H2O

Balance the chemical equation algebraically: H_2O + CaO ⟶ Ca(OH)2H2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 CaO ⟶ c_3 Ca(OH)2H2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and Ca: H: | 2 c_1 = 4 c_3 O: | c_1 + c_2 = 3 c_3 Ca: | c_2 = c_3 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + CaO ⟶ Ca(OH)2H2O

+ ⟶ Ca(OH)2H2O

water + lime ⟶ Ca(OH)2H2O

Construct the equilibrium constant, K, expression for: H_2O + CaO ⟶ Ca(OH)2H2O Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: 2 H_2O + CaO ⟶ Ca(OH)2H2O Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i H_2O | 2 | -2 CaO | 1 | -1 Ca(OH)2H2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) CaO | 1 | -1 | ([CaO])^(-1) Ca(OH)2H2O | 1 | 1 | [Ca(OH)2H2O] The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([H2O])^(-2) ([CaO])^(-1) [Ca(OH)2H2O] = ([Ca(OH)2H2O])/(([H2O])^2 [CaO])

Construct the rate of reaction expression for: H_2O + CaO ⟶ Ca(OH)2H2O Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: 2 H_2O + CaO ⟶ Ca(OH)2H2O Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i H_2O | 2 | -2 CaO | 1 | -1 Ca(OH)2H2O | 1 | 1 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term H_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) CaO | 1 | -1 | -(Δ[CaO])/(Δt) Ca(OH)2H2O | 1 | 1 | (Δ[Ca(OH)2H2O])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -1/2 (Δ[H2O])/(Δt) = -(Δ[CaO])/(Δt) = (Δ[Ca(OH)2H2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| water | lime | Ca(OH)2H2O formula | H_2O | CaO | Ca(OH)2H2O Hill formula | H_2O | CaO | H4CaO3 name | water | lime |

| water | lime | Ca(OH)2H2O molar mass | 18.015 g/mol | 56.077 g/mol | 92.11 g/mol phase | liquid (at STP) | solid (at STP) | melting point | 0 °C | 2580 °C | boiling point | 99.9839 °C | 2850 °C | density | 1 g/cm^3 | 3.3 g/cm^3 | solubility in water | | reacts | surface tension | 0.0728 N/m | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | odor | odorless | |