Fe2(C2O4)3 = CO2 + FeC2O4

Fe_2(C_2O_4)_3 iron(III) oxalate ⟶ CO_2 carbon dioxide + C_2FeO_4 ferrous oxalate

Balance the chemical equation algebraically: Fe_2(C_2O_4)_3 ⟶ CO_2 + C_2FeO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe_2(C_2O_4)_3 ⟶ c_2 CO_2 + c_3 C_2FeO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for C, Fe and O: C: | 6 c_1 = c_2 + 2 c_3 Fe: | 2 c_1 = c_3 O: | 12 c_1 = 2 c_2 + 4 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 = 2 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe_2(C_2O_4)_3 ⟶ 2 CO_2 + 2 C_2FeO_4

⟶ +

iron(III) oxalate ⟶ carbon dioxide + ferrous oxalate

Construct the equilibrium constant, K, expression for: Fe_2(C_2O_4)_3 ⟶ CO_2 + C_2FeO_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_2(C_2O_4)_3 ⟶ 2 CO_2 + 2 C_2FeO_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_2(C_2O_4)_3 | 1 | -1 CO_2 | 2 | 2 C_2FeO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe_2(C_2O_4)_3 | 1 | -1 | ([Fe2(C2O4)3])^(-1) CO_2 | 2 | 2 | ([CO2])^2 C_2FeO_4 | 2 | 2 | ([C2FeO4])^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 = ([Fe2(C2O4)3])^(-1) ([CO2])^2 ([C2FeO4])^2 = (([CO2])^2 ([C2FeO4])^2)/([Fe2(C2O4)3])

Construct the rate of reaction expression for: Fe_2(C_2O_4)_3 ⟶ CO_2 + C_2FeO_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_2(C_2O_4)_3 ⟶ 2 CO_2 + 2 C_2FeO_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_2(C_2O_4)_3 | 1 | -1 CO_2 | 2 | 2 C_2FeO_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 Fe_2(C_2O_4)_3 | 1 | -1 | -(Δ[Fe2(C2O4)3])/(Δt) CO_2 | 2 | 2 | 1/2 (Δ[CO2])/(Δt) C_2FeO_4 | 2 | 2 | 1/2 (Δ[C2FeO4])/(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[Fe2(C2O4)3])/(Δt) = 1/2 (Δ[CO2])/(Δt) = 1/2 (Δ[C2FeO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| iron(III) oxalate | carbon dioxide | ferrous oxalate formula | Fe_2(C_2O_4)_3 | CO_2 | C_2FeO_4 Hill formula | C_6Fe_2O_12 | CO_2 | C_2FeO_4 name | iron(III) oxalate | carbon dioxide | ferrous oxalate IUPAC name | | carbon dioxide | iron(+2) cation; oxalate

| iron(III) oxalate | carbon dioxide | ferrous oxalate molar mass | 375.74 g/mol | 44.009 g/mol | 143.86 g/mol phase | | gas (at STP) | melting point | | -56.56 °C (at triple point) | boiling point | | -78.5 °C (at sublimation point) | density | | 0.00184212 g/cm^3 (at 20 °C) | 2.3 g/cm^3 solubility in water | | | slightly soluble dynamic viscosity | | 1.491×10^-5 Pa s (at 25 °C) | odor | | odorless |