CO + Fe2O2 = CO2 + Fe

CO carbon monoxide + Fe2O2 ⟶ CO_2 carbon dioxide + Fe iron

Balance the chemical equation algebraically: CO + Fe2O2 ⟶ CO_2 + Fe Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CO + c_2 Fe2O2 ⟶ 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, O and Fe: C: | c_1 = c_3 O: | c_1 + 2 c_2 = 2 c_3 Fe: | 2 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 = 2 c_2 = 1 c_3 = 2 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 CO + Fe2O2 ⟶ 2 CO_2 + 2 Fe

+ Fe2O2 ⟶ +

carbon monoxide + Fe2O2 ⟶ carbon dioxide + iron

Construct the equilibrium constant, K, expression for: CO + Fe2O2 ⟶ 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 CO + Fe2O2 ⟶ 2 CO_2 + 2 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 CO | 2 | -2 Fe2O2 | 1 | -1 CO_2 | 2 | 2 Fe | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CO | 2 | -2 | ([CO])^(-2) Fe2O2 | 1 | -1 | ([Fe2O2])^(-1) CO_2 | 2 | 2 | ([CO2])^2 Fe | 2 | 2 | ([Fe])^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 = ([CO])^(-2) ([Fe2O2])^(-1) ([CO2])^2 ([Fe])^2 = (([CO2])^2 ([Fe])^2)/(([CO])^2 [Fe2O2])

Construct the rate of reaction expression for: CO + Fe2O2 ⟶ 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 CO + Fe2O2 ⟶ 2 CO_2 + 2 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 CO | 2 | -2 Fe2O2 | 1 | -1 CO_2 | 2 | 2 Fe | 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 CO | 2 | -2 | -1/2 (Δ[CO])/(Δt) Fe2O2 | 1 | -1 | -(Δ[Fe2O2])/(Δt) CO_2 | 2 | 2 | 1/2 (Δ[CO2])/(Δt) Fe | 2 | 2 | 1/2 (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[CO])/(Δt) = -(Δ[Fe2O2])/(Δt) = 1/2 (Δ[CO2])/(Δt) = 1/2 (Δ[Fe])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| carbon monoxide | Fe2O2 | carbon dioxide | iron formula | CO | Fe2O2 | CO_2 | Fe name | carbon monoxide | | carbon dioxide | iron

| carbon monoxide | Fe2O2 | carbon dioxide | iron molar mass | 28.01 g/mol | 143.69 g/mol | 44.009 g/mol | 55.845 g/mol phase | gas (at STP) | | gas (at STP) | solid (at STP) melting point | -205 °C | | -56.56 °C (at triple point) | 1535 °C boiling point | -191.5 °C | | -78.5 °C (at sublimation point) | 2750 °C density | 0.001145 g/cm^3 (at 25 °C) | | 0.00184212 g/cm^3 (at 20 °C) | 7.874 g/cm^3 solubility in water | | | | insoluble dynamic viscosity | 1.772×10^-5 Pa s (at 25 °C) | | 1.491×10^-5 Pa s (at 25 °C) | odor | odorless | | odorless |