HCl + BaO = H2O + BaCl2

HCl hydrogen chloride + BaO barium oxide ⟶ H_2O water + BaCl_2 barium chloride

Balance the chemical equation algebraically: HCl + BaO ⟶ H_2O + BaCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 BaO ⟶ c_3 H_2O + c_4 BaCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Ba and O: Cl: | c_1 = 2 c_4 H: | c_1 = 2 c_3 Ba: | 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 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + BaO ⟶ H_2O + BaCl_2

+ ⟶ +

hydrogen chloride + barium oxide ⟶ water + barium chloride

| hydrogen chloride | barium oxide | water | barium chloride molecular enthalpy | -92.3 kJ/mol | -548 kJ/mol | -285.8 kJ/mol | -855 kJ/mol total enthalpy | -184.6 kJ/mol | -548 kJ/mol | -285.8 kJ/mol | -855 kJ/mol | H_initial = -732.6 kJ/mol | | H_final = -1141 kJ/mol | ΔH_rxn^0 | -1141 kJ/mol - -732.6 kJ/mol = -408.2 kJ/mol (exothermic) | | |

| hydrogen chloride | barium oxide | water | barium chloride molecular free energy | -95.3 kJ/mol | -520.3 kJ/mol | -237.1 kJ/mol | -806.7 kJ/mol total free energy | -190.6 kJ/mol | -520.3 kJ/mol | -237.1 kJ/mol | -806.7 kJ/mol | G_initial = -710.9 kJ/mol | | G_final = -1044 kJ/mol | ΔG_rxn^0 | -1044 kJ/mol - -710.9 kJ/mol = -332.9 kJ/mol (exergonic) | | |

Construct the equilibrium constant, K, expression for: HCl + BaO ⟶ H_2O + BaCl_2 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 + BaO ⟶ H_2O + BaCl_2 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 BaO | 1 | -1 H_2O | 1 | 1 BaCl_2 | 1 | 1 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) BaO | 1 | -1 | ([BaO])^(-1) H_2O | 1 | 1 | [H2O] BaCl_2 | 1 | 1 | [BaCl2] 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) ([BaO])^(-1) [H2O] [BaCl2] = ([H2O] [BaCl2])/(([HCl])^2 [BaO])

Construct the rate of reaction expression for: HCl + BaO ⟶ H_2O + BaCl_2 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 + BaO ⟶ H_2O + BaCl_2 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 BaO | 1 | -1 H_2O | 1 | 1 BaCl_2 | 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 HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) BaO | 1 | -1 | -(Δ[BaO])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) BaCl_2 | 1 | 1 | (Δ[BaCl2])/(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[BaO])/(Δt) = (Δ[H2O])/(Δt) = (Δ[BaCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen chloride | barium oxide | water | barium chloride formula | HCl | BaO | H_2O | BaCl_2 Hill formula | ClH | BaO | H_2O | BaCl_2 name | hydrogen chloride | barium oxide | water | barium chloride IUPAC name | hydrogen chloride | oxobarium | water | barium(+2) cation dichloride

| hydrogen chloride | barium oxide | water | barium chloride molar mass | 36.46 g/mol | 153.326 g/mol | 18.015 g/mol | 208.2 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | -114.17 °C | 1920 °C | 0 °C | 963 °C boiling point | -85 °C | | 99.9839 °C | density | 0.00149 g/cm^3 (at 25 °C) | 5.72 g/cm^3 | 1 g/cm^3 | 3.856 g/cm^3 solubility in water | miscible | | | surface tension | | | 0.0728 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless | odorless