H2SO4 + H2S + Na2SO3 = H2O + S + Na2SO4

sulfuric acid + hydrogen sulfide + sodium sulfite ⟶ water + mixed sulfur + sodium sulfate

Balance the chemical equation algebraically: + + ⟶ + + Add stoichiometric coefficients, c_i, to the reactants and products: c_1 + c_2 + c_3 ⟶ c_4 + c_5 + c_6 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Na: H: | 2 c_1 + 2 c_2 = 2 c_4 O: | 4 c_1 + 3 c_3 = c_4 + 4 c_6 S: | c_1 + c_2 + c_3 = c_5 + c_6 Na: | 2 c_3 = 2 c_6 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_3 = 3 - c_2 c_4 = c_2 + 1 c_5 = c_2 + 1 c_6 = 3 - c_2 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_2 = 1 and solve for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 2 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | + + 2 ⟶ 2 + 2 + 2

+ + ⟶ + +

sulfuric acid + hydrogen sulfide + sodium sulfite ⟶ water + mixed sulfur + sodium sulfate

K_c = ([H2O]^2 [S]^2 [Na2SO4]^2)/([H2SO4] [H2S] [Na2SO3]^2)

rate = -(Δ[H2SO4])/(Δt) = -(Δ[H2S])/(Δt) = -1/2 (Δ[Na2SO3])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[S])/(Δt) = 1/2 (Δ[Na2SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | hydrogen sulfide | sodium sulfite | water | mixed sulfur | sodium sulfate Hill formula | H_2O_4S | H_2S | Na_2O_3S | H_2O | S | Na_2O_4S name | sulfuric acid | hydrogen sulfide | sodium sulfite | water | mixed sulfur | sodium sulfate IUPAC name | sulfuric acid | hydrogen sulfide | disodium sulfite | water | sulfur | disodium sulfate