Fe + CuCl = Cu + FeCl2

Fe iron + CuCl cuprous chloride ⟶ Cu copper + FeCl_2 iron(II) chloride

Balance the chemical equation algebraically: Fe + CuCl ⟶ Cu + FeCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe + c_2 CuCl ⟶ c_3 Cu + c_4 FeCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, Cl and Cu: Fe: | c_1 = c_4 Cl: | c_2 = 2 c_4 Cu: | c_2 = c_3 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 = 2 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe + 2 CuCl ⟶ 2 Cu + FeCl_2

+ ⟶ +

iron + cuprous chloride ⟶ copper + iron(II) chloride

| iron | cuprous chloride | copper | iron(II) chloride molecular enthalpy | 0 kJ/mol | -137.2 kJ/mol | 0 kJ/mol | -341.8 kJ/mol total enthalpy | 0 kJ/mol | -274.4 kJ/mol | 0 kJ/mol | -341.8 kJ/mol | H_initial = -274.4 kJ/mol | | H_final = -341.8 kJ/mol | ΔH_rxn^0 | -341.8 kJ/mol - -274.4 kJ/mol = -67.4 kJ/mol (exothermic) | | |

Construct the equilibrium constant, K, expression for: Fe + CuCl ⟶ Cu + FeCl_2 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 + 2 CuCl ⟶ 2 Cu + FeCl_2 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 CuCl | 2 | -2 Cu | 2 | 2 FeCl_2 | 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) CuCl | 2 | -2 | ([CuCl])^(-2) Cu | 2 | 2 | ([Cu])^2 FeCl_2 | 1 | 1 | [FeCl2] 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) ([CuCl])^(-2) ([Cu])^2 [FeCl2] = (([Cu])^2 [FeCl2])/([Fe] ([CuCl])^2)

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

| iron | cuprous chloride | copper | iron(II) chloride formula | Fe | CuCl | Cu | FeCl_2 Hill formula | Fe | ClCu | Cu | Cl_2Fe name | iron | cuprous chloride | copper | iron(II) chloride IUPAC name | iron | | copper | dichloroiron

| iron | cuprous chloride | copper | iron(II) chloride molar mass | 55.845 g/mol | 99 g/mol | 63.546 g/mol | 126.7 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 1535 °C | 430 °C | 1083 °C | 677 °C boiling point | 2750 °C | 1490 °C | 2567 °C | density | 7.874 g/cm^3 | 4.145 g/cm^3 | 8.96 g/cm^3 | 3.16 g/cm^3 solubility in water | insoluble | | insoluble | odor | | | odorless |