HCl + Li2O = H2O + LiCl

HCl hydrogen chloride + Li_2O lithium oxide ⟶ H_2O water + LiCl lithium chloride

Balance the chemical equation algebraically: HCl + Li_2O ⟶ H_2O + LiCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Li_2O ⟶ c_3 H_2O + c_4 LiCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Li and O: Cl: | c_1 = c_4 H: | c_1 = 2 c_3 Li: | 2 c_2 = c_4 O: | 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 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + Li_2O ⟶ H_2O + 2 LiCl

+ ⟶ +

hydrogen chloride + lithium oxide ⟶ water + lithium chloride

Construct the equilibrium constant, K, expression for: HCl + Li_2O ⟶ H_2O + LiCl 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 HCl + Li_2O ⟶ H_2O + 2 LiCl 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 HCl | 2 | -2 Li_2O | 1 | -1 H_2O | 1 | 1 LiCl | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) Li_2O | 1 | -1 | ([Li2O])^(-1) H_2O | 1 | 1 | [H2O] LiCl | 2 | 2 | ([LiCl])^2 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 = ([HCl])^(-2) ([Li2O])^(-1) [H2O] ([LiCl])^2 = ([H2O] ([LiCl])^2)/(([HCl])^2 [Li2O])

Construct the rate of reaction expression for: HCl + Li_2O ⟶ H_2O + LiCl 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 HCl + Li_2O ⟶ H_2O + 2 LiCl 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 HCl | 2 | -2 Li_2O | 1 | -1 H_2O | 1 | 1 LiCl | 2 | 2 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 HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) Li_2O | 1 | -1 | -(Δ[Li2O])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) LiCl | 2 | 2 | 1/2 (Δ[LiCl])/(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[HCl])/(Δt) = -(Δ[Li2O])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[LiCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen chloride | lithium oxide | water | lithium chloride formula | HCl | Li_2O | H_2O | LiCl Hill formula | ClH | Li_2O | H_2O | ClLi name | hydrogen chloride | lithium oxide | water | lithium chloride IUPAC name | hydrogen chloride | dilithium oxygen(-2) anion | water | lithium chloride

| hydrogen chloride | lithium oxide | water | lithium chloride molar mass | 36.46 g/mol | 29.9 g/mol | 18.015 g/mol | 42.4 g/mol phase | gas (at STP) | | liquid (at STP) | solid (at STP) melting point | -114.17 °C | | 0 °C | 605 °C boiling point | -85 °C | | 99.9839 °C | 1382 °C density | 0.00149 g/cm^3 (at 25 °C) | 2.013 g/cm^3 | 1 g/cm^3 | 2.07 g/cm^3 solubility in water | miscible | | | surface tension | | | 0.0728 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | 0.00525 Pa s (at 20 °C) odor | | | odorless |