Fe + CuO = Cu + FeO

Fe iron + CuO cupric oxide ⟶ Cu copper + FeO iron(II) oxide

Balance the chemical equation algebraically: Fe + CuO ⟶ Cu + FeO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe + c_2 CuO ⟶ c_3 Cu + c_4 FeO 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 = c_4 Cu: | c_2 = c_3 O: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe + CuO ⟶ Cu + FeO

+ ⟶ +

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

| iron | cupric oxide | copper | iron(II) oxide molecular enthalpy | 0 kJ/mol | -157.3 kJ/mol | 0 kJ/mol | -272 kJ/mol total enthalpy | 0 kJ/mol | -157.3 kJ/mol | 0 kJ/mol | -272 kJ/mol | H_initial = -157.3 kJ/mol | | H_final = -272 kJ/mol | ΔH_rxn^0 | -272 kJ/mol - -157.3 kJ/mol = -114.7 kJ/mol (exothermic) | | |

| iron | cupric oxide | copper | iron(II) oxide molecular entropy | 27 J/(mol K) | 43 J/(mol K) | 33 J/(mol K) | 61 J/(mol K) total entropy | 27 J/(mol K) | 43 J/(mol K) | 33 J/(mol K) | 61 J/(mol K) | S_initial = 70 J/(mol K) | | S_final = 94 J/(mol K) | ΔS_rxn^0 | 94 J/(mol K) - 70 J/(mol K) = 24 J/(mol K) (endoentropic) | | |

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

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

| iron | cupric oxide | copper | iron(II) oxide formula | Fe | CuO | Cu | FeO name | iron | cupric oxide | copper | iron(II) oxide IUPAC name | iron | | copper | oxoiron

| iron | cupric oxide | copper | iron(II) oxide molar mass | 55.845 g/mol | 79.545 g/mol | 63.546 g/mol | 71.844 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 1535 °C | 1326 °C | 1083 °C | 1360 °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 | 5.7 g/cm^3 solubility in water | insoluble | insoluble | insoluble | insoluble odor | | | odorless |