Input interpretation
![Fe (iron) + CuCl_2 (copper(II) chloride) ⟶ Cu (copper) + FeCl_2 (iron(II) chloride)](../image_source/79e6985ffcb6a9447c4df828e68c8f22.png)
Fe (iron) + CuCl_2 (copper(II) chloride) ⟶ Cu (copper) + FeCl_2 (iron(II) chloride)
Balanced equation
![Balance the chemical equation algebraically: Fe + CuCl_2 ⟶ Cu + FeCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe + c_2 CuCl_2 ⟶ 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: | 2 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 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe + CuCl_2 ⟶ Cu + FeCl_2](../image_source/47c66ca00cbec2a20842b4e0f925bf71.png)
Balance the chemical equation algebraically: Fe + CuCl_2 ⟶ Cu + FeCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe + c_2 CuCl_2 ⟶ 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: | 2 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 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe + CuCl_2 ⟶ Cu + FeCl_2
Structures
![+ ⟶ +](../image_source/643b105a097889114ddaa8851126b9a6.png)
+ ⟶ +
Names
![iron + copper(II) chloride ⟶ copper + iron(II) chloride](../image_source/ce72710ecd40a146e08159a41ba99947.png)
iron + copper(II) chloride ⟶ copper + iron(II) chloride
Reaction thermodynamics
Enthalpy
![| iron | copper(II) chloride | copper | iron(II) chloride molecular enthalpy | 0 kJ/mol | -220.1 kJ/mol | 0 kJ/mol | -341.8 kJ/mol total enthalpy | 0 kJ/mol | -220.1 kJ/mol | 0 kJ/mol | -341.8 kJ/mol | H_initial = -220.1 kJ/mol | | H_final = -341.8 kJ/mol | ΔH_rxn^0 | -341.8 kJ/mol - -220.1 kJ/mol = -121.7 kJ/mol (exothermic) | | |](../image_source/573e2279ffbb2297319c465b4bc639bf.png)
| iron | copper(II) chloride | copper | iron(II) chloride molecular enthalpy | 0 kJ/mol | -220.1 kJ/mol | 0 kJ/mol | -341.8 kJ/mol total enthalpy | 0 kJ/mol | -220.1 kJ/mol | 0 kJ/mol | -341.8 kJ/mol | H_initial = -220.1 kJ/mol | | H_final = -341.8 kJ/mol | ΔH_rxn^0 | -341.8 kJ/mol - -220.1 kJ/mol = -121.7 kJ/mol (exothermic) | | |
Equilibrium constant
![Construct the equilibrium constant, K, expression for: Fe + CuCl_2 ⟶ 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 + 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 | 1 | -1 Cu | 1 | 1 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 | 1 | -1 | ([CuCl2])^(-1) Cu | 1 | 1 | [Cu] 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) ([CuCl2])^(-1) [Cu] [FeCl2] = ([Cu] [FeCl2])/([Fe] [CuCl2])](../image_source/e9cabfa580b6b6cb3cbd8c91fc54a5d9.png)
Construct the equilibrium constant, K, expression for: Fe + CuCl_2 ⟶ 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 + 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 | 1 | -1 Cu | 1 | 1 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 | 1 | -1 | ([CuCl2])^(-1) Cu | 1 | 1 | [Cu] 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) ([CuCl2])^(-1) [Cu] [FeCl2] = ([Cu] [FeCl2])/([Fe] [CuCl2])
Rate of reaction
![Construct the rate of reaction expression for: Fe + CuCl_2 ⟶ 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 + 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 | 1 | -1 Cu | 1 | 1 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 | 1 | -1 | -(Δ[CuCl2])/(Δt) Cu | 1 | 1 | (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) = -(Δ[CuCl2])/(Δt) = (Δ[Cu])/(Δt) = (Δ[FeCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/9dd92105d06efcfdec39ba1ed96d881b.png)
Construct the rate of reaction expression for: Fe + CuCl_2 ⟶ 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 + 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 | 1 | -1 Cu | 1 | 1 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 | 1 | -1 | -(Δ[CuCl2])/(Δt) Cu | 1 | 1 | (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) = -(Δ[CuCl2])/(Δt) = (Δ[Cu])/(Δt) = (Δ[FeCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| iron | copper(II) chloride | copper | iron(II) chloride formula | Fe | CuCl_2 | Cu | FeCl_2 Hill formula | Fe | Cl_2Cu | Cu | Cl_2Fe name | iron | copper(II) chloride | copper | iron(II) chloride IUPAC name | iron | dichlorocopper | copper | dichloroiron](../image_source/7bb1a51aee248550a8fbafce436e5f38.png)
| iron | copper(II) chloride | copper | iron(II) chloride formula | Fe | CuCl_2 | Cu | FeCl_2 Hill formula | Fe | Cl_2Cu | Cu | Cl_2Fe name | iron | copper(II) chloride | copper | iron(II) chloride IUPAC name | iron | dichlorocopper | copper | dichloroiron
Substance properties
![| iron | copper(II) chloride | copper | iron(II) chloride molar mass | 55.845 g/mol | 134.4 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 | 620 °C | 1083 °C | 677 °C boiling point | 2750 °C | | 2567 °C | density | 7.874 g/cm^3 | 3.386 g/cm^3 | 8.96 g/cm^3 | 3.16 g/cm^3 solubility in water | insoluble | | insoluble | odor | | | odorless |](../image_source/448d14330b5b3edf32fc15dbad907b5a.png)
| iron | copper(II) chloride | copper | iron(II) chloride molar mass | 55.845 g/mol | 134.4 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 | 620 °C | 1083 °C | 677 °C boiling point | 2750 °C | | 2567 °C | density | 7.874 g/cm^3 | 3.386 g/cm^3 | 8.96 g/cm^3 | 3.16 g/cm^3 solubility in water | insoluble | | insoluble | odor | | | odorless |
Units