Fe + CuO = Cu + Fe2O3

Fe iron + CuO cupric oxide ⟶ Cu copper + Fe_2O_3 iron(III) oxide

Balance the chemical equation algebraically: Fe + CuO ⟶ Cu + Fe_2O_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe + c_2 CuO ⟶ c_3 Cu + c_4 Fe_2O_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, Cu and O: Fe: | c_1 = 2 c_4 Cu: | c_2 = c_3 O: | c_2 = 3 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Fe + 3 CuO ⟶ 3 Cu + Fe_2O_3

+ ⟶ +

iron + cupric oxide ⟶ copper + iron(III) oxide

| iron | cupric oxide | copper | iron(III) oxide molecular enthalpy | 0 kJ/mol | -157.3 kJ/mol | 0 kJ/mol | -826 kJ/mol total enthalpy | 0 kJ/mol | -471.9 kJ/mol | 0 kJ/mol | -826 kJ/mol | H_initial = -471.9 kJ/mol | | H_final = -826 kJ/mol | ΔH_rxn^0 | -826 kJ/mol - -471.9 kJ/mol = -354.1 kJ/mol (exothermic) | | |

| iron | cupric oxide | copper | iron(III) oxide molecular entropy | 27 J/(mol K) | 43 J/(mol K) | 33 J/(mol K) | 90 J/(mol K) total entropy | 54 J/(mol K) | 129 J/(mol K) | 99 J/(mol K) | 90 J/(mol K) | S_initial = 183 J/(mol K) | | S_final = 189 J/(mol K) | ΔS_rxn^0 | 189 J/(mol K) - 183 J/(mol K) = 6 J/(mol K) (endoentropic) | | |

Construct the equilibrium constant, K, expression for: Fe + CuO ⟶ Cu + 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: 2 Fe + 3 CuO ⟶ 3 Cu + 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 Fe | 2 | -2 CuO | 3 | -3 Cu | 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 Fe | 2 | -2 | ([Fe])^(-2) CuO | 3 | -3 | ([CuO])^(-3) Cu | 3 | 3 | ([Cu])^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 = ([Fe])^(-2) ([CuO])^(-3) ([Cu])^3 [Fe2O3] = (([Cu])^3 [Fe2O3])/(([Fe])^2 ([CuO])^3)

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

| iron | cupric oxide | copper | iron(III) oxide formula | Fe | CuO | Cu | Fe_2O_3 name | iron | cupric oxide | copper | iron(III) oxide

| iron | cupric oxide | copper | iron(III) oxide molar mass | 55.845 g/mol | 79.545 g/mol | 63.546 g/mol | 159.69 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 1535 °C | 1326 °C | 1083 °C | 1565 °C boiling point | 2750 °C | 2000 °C | 2567 °C | density | 7.874 g/cm^3 | 6.315 g/cm^3 | 8.96 g/cm^3 | 5.26 g/cm^3 solubility in water | insoluble | insoluble | insoluble | insoluble odor | | | odorless | odorless