H2SO4 + O2 + FeSO4 = H2O + Fe2(SO4)3

sulfuric acid + oxygen + duretter ⟶ water + iron(III) sulfate hydrate

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 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Fe: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 2 c_2 + 4 c_3 = c_4 + 12 c_5 S: | c_1 + c_3 = 3 c_5 Fe: | c_3 = 2 c_5 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 = 4 c_4 = 2 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 + + 4 ⟶ 2 + 2

+ + ⟶ +

sulfuric acid + oxygen + duretter ⟶ water + iron(III) sulfate hydrate

K_c = ([H2O]^2 [Fe2(SO4)3·xH2O]^2)/([H2SO4]^2 [O2] [FeSO4]^4)

rate = -1/2 (Δ[H2SO4])/(Δt) = -(Δ[O2])/(Δt) = -1/4 (Δ[FeSO4])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[Fe2(SO4)3·xH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | oxygen | duretter | water | iron(III) sulfate hydrate Hill formula | H_2O_4S | O_2 | FeO_4S | H_2O | Fe_2O_12S_3 name | sulfuric acid | oxygen | duretter | water | iron(III) sulfate hydrate IUPAC name | sulfuric acid | molecular oxygen | iron(+2) cation sulfate | water | diferric trisulfate