SO2 + Fe2O3 + SO3 = FeSO4

SO_2 sulfur dioxide + Fe_2O_3 iron(III) oxide + SO_3 sulfur trioxide ⟶ FeSO_4 duretter

Balance the chemical equation algebraically: SO_2 + Fe_2O_3 + SO_3 ⟶ FeSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 SO_2 + c_2 Fe_2O_3 + c_3 SO_3 ⟶ c_4 FeSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for O, S and Fe: O: | 2 c_1 + 3 c_2 + 3 c_3 = 4 c_4 S: | c_1 + c_3 = c_4 Fe: | 2 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 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | SO_2 + Fe_2O_3 + SO_3 ⟶ 2 FeSO_4

+ + ⟶

sulfur dioxide + iron(III) oxide + sulfur trioxide ⟶ duretter

Construct the equilibrium constant, K, expression for: SO_2 + Fe_2O_3 + SO_3 ⟶ 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: SO_2 + Fe_2O_3 + SO_3 ⟶ 2 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 SO_2 | 1 | -1 Fe_2O_3 | 1 | -1 SO_3 | 1 | -1 FeSO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression SO_2 | 1 | -1 | ([SO2])^(-1) Fe_2O_3 | 1 | -1 | ([Fe2O3])^(-1) SO_3 | 1 | -1 | ([SO3])^(-1) FeSO_4 | 2 | 2 | ([FeSO4])^2 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 = ([SO2])^(-1) ([Fe2O3])^(-1) ([SO3])^(-1) ([FeSO4])^2 = ([FeSO4])^2/([SO2] [Fe2O3] [SO3])

Construct the rate of reaction expression for: SO_2 + Fe_2O_3 + SO_3 ⟶ 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: SO_2 + Fe_2O_3 + SO_3 ⟶ 2 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 SO_2 | 1 | -1 Fe_2O_3 | 1 | -1 SO_3 | 1 | -1 FeSO_4 | 2 | 2 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 SO_2 | 1 | -1 | -(Δ[SO2])/(Δt) Fe_2O_3 | 1 | -1 | -(Δ[Fe2O3])/(Δt) SO_3 | 1 | -1 | -(Δ[SO3])/(Δt) FeSO_4 | 2 | 2 | 1/2 (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[SO2])/(Δt) = -(Δ[Fe2O3])/(Δt) = -(Δ[SO3])/(Δt) = 1/2 (Δ[FeSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfur dioxide | iron(III) oxide | sulfur trioxide | duretter formula | SO_2 | Fe_2O_3 | SO_3 | FeSO_4 Hill formula | O_2S | Fe_2O_3 | O_3S | FeO_4S name | sulfur dioxide | iron(III) oxide | sulfur trioxide | duretter IUPAC name | sulfur dioxide | | sulfur trioxide | iron(+2) cation sulfate

| sulfur dioxide | iron(III) oxide | sulfur trioxide | duretter molar mass | 64.06 g/mol | 159.69 g/mol | 80.06 g/mol | 151.9 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | melting point | -73 °C | 1565 °C | 16.8 °C | boiling point | -10 °C | | 44.7 °C | density | 0.002619 g/cm^3 (at 25 °C) | 5.26 g/cm^3 | 1.97 g/cm^3 | 2.841 g/cm^3 solubility in water | | insoluble | reacts | surface tension | 0.02859 N/m | | | dynamic viscosity | 1.282×10^-5 Pa s (at 25 °C) | | 0.00159 Pa s (at 30 °C) | odor | | odorless | |