NaCl + FeO = FeCl2 + Na2O

NaCl sodium chloride + FeO iron(II) oxide ⟶ FeCl_2 iron(II) chloride + Na_2O sodium oxide

Balance the chemical equation algebraically: NaCl + FeO ⟶ FeCl_2 + Na_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaCl + c_2 FeO ⟶ c_3 FeCl_2 + c_4 Na_2O Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Na, Fe and O: Cl: | c_1 = 2 c_3 Na: | c_1 = 2 c_4 Fe: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NaCl + FeO ⟶ FeCl_2 + Na_2O

+ ⟶ +

sodium chloride + iron(II) oxide ⟶ iron(II) chloride + sodium oxide

Construct the equilibrium constant, K, expression for: NaCl + FeO ⟶ FeCl_2 + Na_2O 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 NaCl + FeO ⟶ FeCl_2 + Na_2O 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 NaCl | 2 | -2 FeO | 1 | -1 FeCl_2 | 1 | 1 Na_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaCl | 2 | -2 | ([NaCl])^(-2) FeO | 1 | -1 | ([FeO])^(-1) FeCl_2 | 1 | 1 | [FeCl2] Na_2O | 1 | 1 | [Na2O] 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 = ([NaCl])^(-2) ([FeO])^(-1) [FeCl2] [Na2O] = ([FeCl2] [Na2O])/(([NaCl])^2 [FeO])

Construct the rate of reaction expression for: NaCl + FeO ⟶ FeCl_2 + Na_2O 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 NaCl + FeO ⟶ FeCl_2 + Na_2O 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 NaCl | 2 | -2 FeO | 1 | -1 FeCl_2 | 1 | 1 Na_2O | 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 NaCl | 2 | -2 | -1/2 (Δ[NaCl])/(Δt) FeO | 1 | -1 | -(Δ[FeO])/(Δt) FeCl_2 | 1 | 1 | (Δ[FeCl2])/(Δt) Na_2O | 1 | 1 | (Δ[Na2O])/(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[NaCl])/(Δt) = -(Δ[FeO])/(Δt) = (Δ[FeCl2])/(Δt) = (Δ[Na2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sodium chloride | iron(II) oxide | iron(II) chloride | sodium oxide formula | NaCl | FeO | FeCl_2 | Na_2O Hill formula | ClNa | FeO | Cl_2Fe | Na_2O name | sodium chloride | iron(II) oxide | iron(II) chloride | sodium oxide IUPAC name | sodium chloride | oxoiron | dichloroiron | disodium oxygen(-2) anion

| sodium chloride | iron(II) oxide | iron(II) chloride | sodium oxide molar mass | 58.44 g/mol | 71.844 g/mol | 126.7 g/mol | 61.979 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 801 °C | 1360 °C | 677 °C | boiling point | 1413 °C | | | density | 2.16 g/cm^3 | 5.7 g/cm^3 | 3.16 g/cm^3 | 2.27 g/cm^3 solubility in water | soluble | insoluble | | odor | odorless | | |