H2SO4 + FeO = H2O + FeSO4

H_2SO_4 (sulfuric acid) + FeO (iron(II) oxide) ⟶ H_2O (water) + FeSO_4 (duretter)

Balance the chemical equation algebraically: H_2SO_4 + FeO ⟶ H_2O + FeSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 FeO ⟶ c_3 H_2O + c_4 FeSO_4 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_3 O: | 4 c_1 + c_2 = c_3 + 4 c_4 S: | c_1 = c_4 Fe: | c_2 = c_4 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_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + FeO ⟶ H_2O + FeSO_4

+ ⟶ +

sulfuric acid + iron(II) oxide ⟶ water + duretter

Construct the equilibrium constant, K, expression for: H_2SO_4 + FeO ⟶ H_2O + FeSO_4 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: H_2SO_4 + FeO ⟶ H_2O + FeSO_4 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_2SO_4 | 1 | -1 FeO | 1 | -1 H_2O | 1 | 1 FeSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) FeO | 1 | -1 | ([FeO])^(-1) H_2O | 1 | 1 | [H2O] FeSO_4 | 1 | 1 | [FeSO4] 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 = ([H2SO4])^(-1) ([FeO])^(-1) [H2O] [FeSO4] = ([H2O] [FeSO4])/([H2SO4] [FeO])

Construct the rate of reaction expression for: H_2SO_4 + FeO ⟶ H_2O + FeSO_4 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: H_2SO_4 + FeO ⟶ H_2O + FeSO_4 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_2SO_4 | 1 | -1 FeO | 1 | -1 H_2O | 1 | 1 FeSO_4 | 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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) FeO | 1 | -1 | -(Δ[FeO])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) FeSO_4 | 1 | 1 | (Δ[FeSO4])/(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 = -(Δ[H2SO4])/(Δt) = -(Δ[FeO])/(Δt) = (Δ[H2O])/(Δt) = (Δ[FeSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | iron(II) oxide | water | duretter formula | H_2SO_4 | FeO | H_2O | FeSO_4 Hill formula | H_2O_4S | FeO | H_2O | FeO_4S name | sulfuric acid | iron(II) oxide | water | duretter IUPAC name | sulfuric acid | oxoiron | water | iron(+2) cation sulfate

| sulfuric acid | iron(II) oxide | water | duretter molar mass | 98.07 g/mol | 71.844 g/mol | 18.015 g/mol | 151.9 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | melting point | 10.371 °C | 1360 °C | 0 °C | boiling point | 279.6 °C | | 99.9839 °C | density | 1.8305 g/cm^3 | 5.7 g/cm^3 | 1 g/cm^3 | 2.841 g/cm^3 solubility in water | very soluble | insoluble | | surface tension | 0.0735 N/m | | 0.0728 N/m | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless |