H2S + H2SO3 = H2O + S

H_2S (hydrogen sulfide) + H_2SO_3 (sulfurous acid) ⟶ H_2O (water) + S (mixed sulfur)

Balance the chemical equation algebraically: H_2S + H_2SO_3 ⟶ H_2O + S Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2S + c_2 H_2SO_3 ⟶ c_3 H_2O + c_4 S Set the number of atoms in the reactants equal to the number of atoms in the products for H, S and O: H: | 2 c_1 + 2 c_2 = 2 c_3 S: | c_1 + c_2 = c_4 O: | 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 = 2 c_2 = 1 c_3 = 3 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2S + H_2SO_3 ⟶ 3 H_2O + 3 S

+ ⟶ +

hydrogen sulfide + sulfurous acid ⟶ water + mixed sulfur

Construct the equilibrium constant, K, expression for: H_2S + H_2SO_3 ⟶ H_2O + S 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 H_2S + H_2SO_3 ⟶ 3 H_2O + 3 S 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 H_2S | 2 | -2 H_2SO_3 | 1 | -1 H_2O | 3 | 3 S | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2S | 2 | -2 | ([H2S])^(-2) H_2SO_3 | 1 | -1 | ([H2SO3])^(-1) H_2O | 3 | 3 | ([H2O])^3 S | 3 | 3 | ([S])^3 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 = ([H2S])^(-2) ([H2SO3])^(-1) ([H2O])^3 ([S])^3 = (([H2O])^3 ([S])^3)/(([H2S])^2 [H2SO3])

Construct the rate of reaction expression for: H_2S + H_2SO_3 ⟶ H_2O + S 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 H_2S + H_2SO_3 ⟶ 3 H_2O + 3 S 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 H_2S | 2 | -2 H_2SO_3 | 1 | -1 H_2O | 3 | 3 S | 3 | 3 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 H_2S | 2 | -2 | -1/2 (Δ[H2S])/(Δt) H_2SO_3 | 1 | -1 | -(Δ[H2SO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) S | 3 | 3 | 1/3 (Δ[S])/(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[H2S])/(Δt) = -(Δ[H2SO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/3 (Δ[S])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen sulfide | sulfurous acid | water | mixed sulfur formula | H_2S | H_2SO_3 | H_2O | S Hill formula | H_2S | H_2O_3S | H_2O | S name | hydrogen sulfide | sulfurous acid | water | mixed sulfur IUPAC name | hydrogen sulfide | sulfurous acid | water | sulfur

| hydrogen sulfide | sulfurous acid | water | mixed sulfur molar mass | 34.08 g/mol | 82.07 g/mol | 18.015 g/mol | 32.06 g/mol phase | gas (at STP) | | liquid (at STP) | solid (at STP) melting point | -85 °C | | 0 °C | 112.8 °C boiling point | -60 °C | | 99.9839 °C | 444.7 °C density | 0.001393 g/cm^3 (at 25 °C) | 1.03 g/cm^3 | 1 g/cm^3 | 2.07 g/cm^3 solubility in water | | very soluble | | surface tension | | | 0.0728 N/m | dynamic viscosity | 1.239×10^-5 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless |