HCl + FeS = H2S + FeCl2

HCl (hydrogen chloride) + FeS (ferrous sulfide) ⟶ H_2S (hydrogen sulfide) + FeCl_2 (iron(II) chloride)

Balance the chemical equation algebraically: HCl + FeS ⟶ H_2S + FeCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 FeS ⟶ c_3 H_2S + c_4 FeCl_2 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 = 2 c_4 H: | c_1 = 2 c_3 Fe: | c_2 = c_4 S: | 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 + FeS ⟶ H_2S + FeCl_2

+ ⟶ +

hydrogen chloride + ferrous sulfide ⟶ hydrogen sulfide + iron(II) chloride

| hydrogen chloride | ferrous sulfide | hydrogen sulfide | iron(II) chloride molecular enthalpy | -92.3 kJ/mol | -100 kJ/mol | -20.6 kJ/mol | -341.8 kJ/mol total enthalpy | -184.6 kJ/mol | -100 kJ/mol | -20.6 kJ/mol | -341.8 kJ/mol | H_initial = -284.6 kJ/mol | | H_final = -362.4 kJ/mol | ΔH_rxn^0 | -362.4 kJ/mol - -284.6 kJ/mol = -77.8 kJ/mol (exothermic) | | |

| hydrogen chloride | ferrous sulfide | hydrogen sulfide | iron(II) chloride molecular free energy | -95.3 kJ/mol | -100.4 kJ/mol | -33.4 kJ/mol | -302.3 kJ/mol total free energy | -190.6 kJ/mol | -100.4 kJ/mol | -33.4 kJ/mol | -302.3 kJ/mol | G_initial = -291 kJ/mol | | G_final = -335.7 kJ/mol | ΔG_rxn^0 | -335.7 kJ/mol - -291 kJ/mol = -44.7 kJ/mol (exergonic) | | |

Construct the equilibrium constant, K, expression for: HCl + FeS ⟶ H_2S + FeCl_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 + FeS ⟶ H_2S + FeCl_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 FeS | 1 | -1 H_2S | 1 | 1 FeCl_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) FeS | 1 | -1 | ([FeS])^(-1) H_2S | 1 | 1 | [H2S] FeCl_2 | 1 | 1 | [FeCl2] 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) ([FeS])^(-1) [H2S] [FeCl2] = ([H2S] [FeCl2])/(([HCl])^2 [FeS])

Construct the rate of reaction expression for: HCl + FeS ⟶ H_2S + FeCl_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 + FeS ⟶ H_2S + FeCl_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 FeS | 1 | -1 H_2S | 1 | 1 FeCl_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) FeS | 1 | -1 | -(Δ[FeS])/(Δt) H_2S | 1 | 1 | (Δ[H2S])/(Δt) FeCl_2 | 1 | 1 | (Δ[FeCl2])/(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[FeS])/(Δt) = (Δ[H2S])/(Δt) = (Δ[FeCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen chloride | ferrous sulfide | hydrogen sulfide | iron(II) chloride formula | HCl | FeS | H_2S | FeCl_2 Hill formula | ClH | FeS | H_2S | Cl_2Fe name | hydrogen chloride | ferrous sulfide | hydrogen sulfide | iron(II) chloride IUPAC name | hydrogen chloride | | hydrogen sulfide | dichloroiron

| hydrogen chloride | ferrous sulfide | hydrogen sulfide | iron(II) chloride molar mass | 36.46 g/mol | 87.9 g/mol | 34.08 g/mol | 126.7 g/mol phase | gas (at STP) | solid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | 1195 °C | -85 °C | 677 °C boiling point | -85 °C | | -60 °C | density | 0.00149 g/cm^3 (at 25 °C) | 4.84 g/cm^3 | 0.001393 g/cm^3 (at 25 °C) | 3.16 g/cm^3 solubility in water | miscible | insoluble | | dynamic viscosity | | 0.00343 Pa s (at 1250 °C) | 1.239×10^-5 Pa s (at 25 °C) |