Fe + Fe2(SO4)3 = FeSO4

Fe iron + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate ⟶ FeSO_4 duretter

Balance the chemical equation algebraically: Fe + Fe_2(SO_4)_3·xH_2O ⟶ FeSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe + c_2 Fe_2(SO_4)_3·xH_2O ⟶ c_3 FeSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O and S: Fe: | c_1 + 2 c_2 = c_3 O: | 12 c_2 = 4 c_3 S: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe + Fe_2(SO_4)_3·xH_2O ⟶ 3 FeSO_4

+ ⟶

iron + iron(III) sulfate hydrate ⟶ duretter

Construct the equilibrium constant, K, expression for: Fe + Fe_2(SO_4)_3·xH_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: Fe + Fe_2(SO_4)_3·xH_2O ⟶ 3 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 Fe | 1 | -1 Fe_2(SO_4)_3·xH_2O | 1 | -1 FeSO_4 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe | 1 | -1 | ([Fe])^(-1) Fe_2(SO_4)_3·xH_2O | 1 | -1 | ([Fe2(SO4)3·xH2O])^(-1) FeSO_4 | 3 | 3 | ([FeSO4])^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 = ([Fe])^(-1) ([Fe2(SO4)3·xH2O])^(-1) ([FeSO4])^3 = ([FeSO4])^3/([Fe] [Fe2(SO4)3·xH2O])

Construct the rate of reaction expression for: Fe + Fe_2(SO_4)_3·xH_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: Fe + Fe_2(SO_4)_3·xH_2O ⟶ 3 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 Fe | 1 | -1 Fe_2(SO_4)_3·xH_2O | 1 | -1 FeSO_4 | 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 Fe | 1 | -1 | -(Δ[Fe])/(Δt) Fe_2(SO_4)_3·xH_2O | 1 | -1 | -(Δ[Fe2(SO4)3·xH2O])/(Δt) FeSO_4 | 3 | 3 | 1/3 (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[Fe])/(Δt) = -(Δ[Fe2(SO4)3·xH2O])/(Δt) = 1/3 (Δ[FeSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| iron | iron(III) sulfate hydrate | duretter formula | Fe | Fe_2(SO_4)_3·xH_2O | FeSO_4 Hill formula | Fe | Fe_2O_12S_3 | FeO_4S name | iron | iron(III) sulfate hydrate | duretter IUPAC name | iron | diferric trisulfate | iron(+2) cation sulfate

| iron | iron(III) sulfate hydrate | duretter molar mass | 55.845 g/mol | 399.9 g/mol | 151.9 g/mol phase | solid (at STP) | | melting point | 1535 °C | | boiling point | 2750 °C | | density | 7.874 g/cm^3 | | 2.841 g/cm^3 solubility in water | insoluble | slightly soluble |