HCl + Fe2S3 = H2S + FeCl3

HCl hydrogen chloride + Fe2S3 ⟶ H_2S hydrogen sulfide + FeCl_3 iron(III) chloride

Balance the chemical equation algebraically: HCl + Fe2S3 ⟶ H_2S + FeCl_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Fe2S3 ⟶ c_3 H_2S + c_4 FeCl_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Fe and S: Cl: | c_1 = 3 c_4 H: | c_1 = 2 c_3 Fe: | 2 c_2 = c_4 S: | 3 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 = 6 c_2 = 1 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HCl + Fe2S3 ⟶ 3 H_2S + 2 FeCl_3

+ Fe2S3 ⟶ +

hydrogen chloride + Fe2S3 ⟶ hydrogen sulfide + iron(III) chloride

Construct the equilibrium constant, K, expression for: HCl + Fe2S3 ⟶ H_2S + FeCl_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: 6 HCl + Fe2S3 ⟶ 3 H_2S + 2 FeCl_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 | 6 | -6 Fe2S3 | 1 | -1 H_2S | 3 | 3 FeCl_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 | 6 | -6 | ([HCl])^(-6) Fe2S3 | 1 | -1 | ([Fe2S3])^(-1) H_2S | 3 | 3 | ([H2S])^3 FeCl_3 | 2 | 2 | ([FeCl3])^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])^(-6) ([Fe2S3])^(-1) ([H2S])^3 ([FeCl3])^2 = (([H2S])^3 ([FeCl3])^2)/(([HCl])^6 [Fe2S3])

Construct the rate of reaction expression for: HCl + Fe2S3 ⟶ H_2S + FeCl_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: 6 HCl + Fe2S3 ⟶ 3 H_2S + 2 FeCl_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 | 6 | -6 Fe2S3 | 1 | -1 H_2S | 3 | 3 FeCl_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 | 6 | -6 | -1/6 (Δ[HCl])/(Δt) Fe2S3 | 1 | -1 | -(Δ[Fe2S3])/(Δt) H_2S | 3 | 3 | 1/3 (Δ[H2S])/(Δt) FeCl_3 | 2 | 2 | 1/2 (Δ[FeCl3])/(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 = -1/6 (Δ[HCl])/(Δt) = -(Δ[Fe2S3])/(Δt) = 1/3 (Δ[H2S])/(Δt) = 1/2 (Δ[FeCl3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen chloride | Fe2S3 | hydrogen sulfide | iron(III) chloride formula | HCl | Fe2S3 | H_2S | FeCl_3 Hill formula | ClH | Fe2S3 | H_2S | Cl_3Fe name | hydrogen chloride | | hydrogen sulfide | iron(III) chloride IUPAC name | hydrogen chloride | | hydrogen sulfide | trichloroiron

| hydrogen chloride | Fe2S3 | hydrogen sulfide | iron(III) chloride molar mass | 36.46 g/mol | 207.9 g/mol | 34.08 g/mol | 162.2 g/mol phase | gas (at STP) | | gas (at STP) | solid (at STP) melting point | -114.17 °C | | -85 °C | 304 °C boiling point | -85 °C | | -60 °C | density | 0.00149 g/cm^3 (at 25 °C) | | 0.001393 g/cm^3 (at 25 °C) | solubility in water | miscible | | | dynamic viscosity | | | 1.239×10^-5 Pa s (at 25 °C) |