C + Fe3O4 = Fe + CO

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

Balance the chemical equation algebraically: + ⟶ + Add stoichiometric coefficients, c_i, to the reactants and products: c_1 + c_2 ⟶ c_3 + c_4 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_4 Fe: | 3 c_2 = c_3 O: | 4 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 1 c_3 = 3 c_4 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 + ⟶ 3 + 4

+ ⟶ +

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

Construct the equilibrium constant, K, expression for: + ⟶ + 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: 4 + ⟶ 3 + 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 | 4 | -4 | 1 | -1 | 3 | 3 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression | 4 | -4 | ([C])^(-4) | 1 | -1 | ([FeO·Fe2O3])^(-1) | 3 | 3 | ([Fe])^3 | 4 | 4 | ([CO])^4 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])^(-4) ([FeO·Fe2O3])^(-1) ([Fe])^3 ([CO])^4 = (([Fe])^3 ([CO])^4)/(([C])^4 [FeO·Fe2O3])

Construct the rate of reaction expression for: + ⟶ + 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: 4 + ⟶ 3 + 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 | 4 | -4 | 1 | -1 | 3 | 3 | 4 | 4 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 | 4 | -4 | -1/4 (Δ[C])/(Δt) | 1 | -1 | -(Δ[FeO·Fe2O3])/(Δt) | 3 | 3 | 1/3 (Δ[Fe])/(Δt) | 4 | 4 | 1/4 (Δ[CO])/(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 = -1/4 (Δ[C])/(Δt) = -(Δ[FeO·Fe2O3])/(Δt) = 1/3 (Δ[Fe])/(Δt) = 1/4 (Δ[CO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| activated charcoal | iron(II, III) oxide | iron | carbon monoxide Hill formula | C | Fe_3O_4 | Fe | CO name | activated charcoal | iron(II, III) oxide | iron | carbon monoxide IUPAC name | carbon | | iron | carbon monoxide

| activated charcoal | iron(II, III) oxide | iron | carbon monoxide molar mass | 12.011 g/mol | 231.53 g/mol | 55.845 g/mol | 28.01 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | gas (at STP) melting point | 3550 °C | 1538 °C | 1535 °C | -205 °C boiling point | 4027 °C | | 2750 °C | -191.5 °C density | 2.26 g/cm^3 | 5 g/cm^3 | 7.874 g/cm^3 | 0.001145 g/cm^3 (at 25 °C) solubility in water | insoluble | | insoluble | dynamic viscosity | | | | 1.772×10^-5 Pa s (at 25 °C) odor | | | | odorless