HCl + Bi2O5 = H2O + Cl2 + BiCl3

HCl hydrogen chloride + Bi2O5 ⟶ H_2O water + Cl_2 chlorine + BiCl_3 bismuth chloride

Balance the chemical equation algebraically: HCl + Bi2O5 ⟶ H_2O + Cl_2 + BiCl_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Bi2O5 ⟶ c_3 H_2O + c_4 Cl_2 + c_5 BiCl_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Bi and O: Cl: | c_1 = 2 c_4 + 3 c_5 H: | c_1 = 2 c_3 Bi: | 2 c_2 = c_5 O: | 5 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 = 10 c_2 = 1 c_3 = 5 c_4 = 2 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 HCl + Bi2O5 ⟶ 5 H_2O + 2 Cl_2 + 2 BiCl_3

+ Bi2O5 ⟶ + +

hydrogen chloride + Bi2O5 ⟶ water + chlorine + bismuth chloride

Construct the equilibrium constant, K, expression for: HCl + Bi2O5 ⟶ H_2O + Cl_2 + BiCl_3 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: 10 HCl + Bi2O5 ⟶ 5 H_2O + 2 Cl_2 + 2 BiCl_3 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 | 10 | -10 Bi2O5 | 1 | -1 H_2O | 5 | 5 Cl_2 | 2 | 2 BiCl_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 10 | -10 | ([HCl])^(-10) Bi2O5 | 1 | -1 | ([Bi2O5])^(-1) H_2O | 5 | 5 | ([H2O])^5 Cl_2 | 2 | 2 | ([Cl2])^2 BiCl_3 | 2 | 2 | ([BiCl3])^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])^(-10) ([Bi2O5])^(-1) ([H2O])^5 ([Cl2])^2 ([BiCl3])^2 = (([H2O])^5 ([Cl2])^2 ([BiCl3])^2)/(([HCl])^10 [Bi2O5])

Construct the rate of reaction expression for: HCl + Bi2O5 ⟶ H_2O + Cl_2 + BiCl_3 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: 10 HCl + Bi2O5 ⟶ 5 H_2O + 2 Cl_2 + 2 BiCl_3 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 | 10 | -10 Bi2O5 | 1 | -1 H_2O | 5 | 5 Cl_2 | 2 | 2 BiCl_3 | 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 | 10 | -10 | -1/10 (Δ[HCl])/(Δt) Bi2O5 | 1 | -1 | -(Δ[Bi2O5])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) Cl_2 | 2 | 2 | 1/2 (Δ[Cl2])/(Δt) BiCl_3 | 2 | 2 | 1/2 (Δ[BiCl3])/(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 = -1/10 (Δ[HCl])/(Δt) = -(Δ[Bi2O5])/(Δt) = 1/5 (Δ[H2O])/(Δt) = 1/2 (Δ[Cl2])/(Δt) = 1/2 (Δ[BiCl3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen chloride | Bi2O5 | water | chlorine | bismuth chloride formula | HCl | Bi2O5 | H_2O | Cl_2 | BiCl_3 Hill formula | ClH | Bi2O5 | H_2O | Cl_2 | BiCl_3 name | hydrogen chloride | | water | chlorine | bismuth chloride IUPAC name | hydrogen chloride | | water | molecular chlorine | trichlorobismuthane