C + Fe3O4 = CO2 + Fe

C (activated charcoal) + FeO·Fe_2O_3 (iron(II, III) oxide) ⟶ CO_2 (carbon dioxide) + Fe (iron)

Balance the chemical equation algebraically: C + FeO·Fe_2O_3 ⟶ CO_2 + Fe Add stoichiometric coefficients, c_i, to the reactants and products: c_1 C + c_2 FeO·Fe_2O_3 ⟶ c_3 CO_2 + c_4 Fe Set the number of atoms in the reactants equal to the number of atoms in the products for C, Fe and O: C: | c_1 = c_3 Fe: | 3 c_2 = c_4 O: | 4 c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 C + FeO·Fe_2O_3 ⟶ 2 CO_2 + 3 Fe

+ ⟶ +

activated charcoal + iron(II, III) oxide ⟶ carbon dioxide + iron

Construct the equilibrium constant, K, expression for: C + FeO·Fe_2O_3 ⟶ CO_2 + Fe 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: 2 C + FeO·Fe_2O_3 ⟶ 2 CO_2 + 3 Fe 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 C | 2 | -2 FeO·Fe_2O_3 | 1 | -1 CO_2 | 2 | 2 Fe | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression C | 2 | -2 | ([C])^(-2) FeO·Fe_2O_3 | 1 | -1 | ([FeO·Fe2O3])^(-1) CO_2 | 2 | 2 | ([CO2])^2 Fe | 3 | 3 | ([Fe])^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 = ([C])^(-2) ([FeO·Fe2O3])^(-1) ([CO2])^2 ([Fe])^3 = (([CO2])^2 ([Fe])^3)/(([C])^2 [FeO·Fe2O3])

Construct the rate of reaction expression for: C + FeO·Fe_2O_3 ⟶ CO_2 + Fe 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: 2 C + FeO·Fe_2O_3 ⟶ 2 CO_2 + 3 Fe 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 C | 2 | -2 FeO·Fe_2O_3 | 1 | -1 CO_2 | 2 | 2 Fe | 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 C | 2 | -2 | -1/2 (Δ[C])/(Δt) FeO·Fe_2O_3 | 1 | -1 | -(Δ[FeO·Fe2O3])/(Δt) CO_2 | 2 | 2 | 1/2 (Δ[CO2])/(Δt) Fe | 3 | 3 | 1/3 (Δ[Fe])/(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 = -1/2 (Δ[C])/(Δt) = -(Δ[FeO·Fe2O3])/(Δt) = 1/2 (Δ[CO2])/(Δt) = 1/3 (Δ[Fe])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| activated charcoal | iron(II, III) oxide | carbon dioxide | iron formula | C | FeO·Fe_2O_3 | CO_2 | Fe Hill formula | C | Fe_3O_4 | CO_2 | Fe name | activated charcoal | iron(II, III) oxide | carbon dioxide | iron IUPAC name | carbon | | carbon dioxide | iron