Fe2(CO3)3 = CO2 + Fe2O3

Fe2(CO3)3 ⟶ CO_2 carbon dioxide + Fe_2O_3 iron(III) oxide

Balance the chemical equation algebraically: Fe2(CO3)3 ⟶ CO_2 + Fe_2O_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe2(CO3)3 ⟶ c_2 CO_2 + c_3 Fe_2O_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, C and O: Fe: | 2 c_1 = 2 c_3 C: | 3 c_1 = c_2 O: | 9 c_1 = 2 c_2 + 3 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 = 3 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe2(CO3)3 ⟶ 3 CO_2 + Fe_2O_3

Fe2(CO3)3 ⟶ +

Fe2(CO3)3 ⟶ carbon dioxide + iron(III) oxide

Construct the equilibrium constant, K, expression for: Fe2(CO3)3 ⟶ CO_2 + Fe_2O_3 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: Fe2(CO3)3 ⟶ 3 CO_2 + Fe_2O_3 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 Fe2(CO3)3 | 1 | -1 CO_2 | 3 | 3 Fe_2O_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe2(CO3)3 | 1 | -1 | ([Fe2(CO3)3])^(-1) CO_2 | 3 | 3 | ([CO2])^3 Fe_2O_3 | 1 | 1 | [Fe2O3] 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(CO3)3])^(-1) ([CO2])^3 [Fe2O3] = (([CO2])^3 [Fe2O3])/([Fe2(CO3)3])

Construct the rate of reaction expression for: Fe2(CO3)3 ⟶ CO_2 + Fe_2O_3 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: Fe2(CO3)3 ⟶ 3 CO_2 + Fe_2O_3 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 Fe2(CO3)3 | 1 | -1 CO_2 | 3 | 3 Fe_2O_3 | 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 Fe2(CO3)3 | 1 | -1 | -(Δ[Fe2(CO3)3])/(Δt) CO_2 | 3 | 3 | 1/3 (Δ[CO2])/(Δt) Fe_2O_3 | 1 | 1 | (Δ[Fe2O3])/(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(CO3)3])/(Δt) = 1/3 (Δ[CO2])/(Δt) = (Δ[Fe2O3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| Fe2(CO3)3 | carbon dioxide | iron(III) oxide formula | Fe2(CO3)3 | CO_2 | Fe_2O_3 Hill formula | C3Fe2O9 | CO_2 | Fe_2O_3 name | | carbon dioxide | iron(III) oxide

| Fe2(CO3)3 | carbon dioxide | iron(III) oxide molar mass | 291.71 g/mol | 44.009 g/mol | 159.69 g/mol phase | | gas (at STP) | solid (at STP) melting point | | -56.56 °C (at triple point) | 1565 °C boiling point | | -78.5 °C (at sublimation point) | density | | 0.00184212 g/cm^3 (at 20 °C) | 5.26 g/cm^3 solubility in water | | | insoluble dynamic viscosity | | 1.491×10^-5 Pa s (at 25 °C) | odor | | odorless | odorless