Input interpretation
![Al aluminum + FeCl_2 iron(II) chloride ⟶ Fe iron + AlCl_3 aluminum chloride](../image_source/c43fd55c2b627852cdcc6c9c6809c1de.png)
Al aluminum + FeCl_2 iron(II) chloride ⟶ Fe iron + AlCl_3 aluminum chloride
Balanced equation
![Balance the chemical equation algebraically: Al + FeCl_2 ⟶ Fe + AlCl_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Al + c_2 FeCl_2 ⟶ c_3 Fe + c_4 AlCl_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Al, Cl and Fe: Al: | c_1 = c_4 Cl: | 2 c_2 = 3 c_4 Fe: | 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 = 3/2 c_3 = 3/2 c_4 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 2 c_2 = 3 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Al + 3 FeCl_2 ⟶ 3 Fe + 2 AlCl_3](../image_source/41694f23ac7221addead679aa2b92951.png)
Balance the chemical equation algebraically: Al + FeCl_2 ⟶ Fe + AlCl_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Al + c_2 FeCl_2 ⟶ c_3 Fe + c_4 AlCl_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Al, Cl and Fe: Al: | c_1 = c_4 Cl: | 2 c_2 = 3 c_4 Fe: | 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 = 3/2 c_3 = 3/2 c_4 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 2 c_2 = 3 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Al + 3 FeCl_2 ⟶ 3 Fe + 2 AlCl_3
Structures
![+ ⟶ +](../image_source/41cb36a30d7573d34aff9db8e3396b9c.png)
+ ⟶ +
Names
![aluminum + iron(II) chloride ⟶ iron + aluminum chloride](../image_source/34fc752a8851b16b071aba8e932e0e62.png)
aluminum + iron(II) chloride ⟶ iron + aluminum chloride
Reaction thermodynamics
Enthalpy
![| aluminum | iron(II) chloride | iron | aluminum chloride molecular enthalpy | 0 kJ/mol | -341.8 kJ/mol | 0 kJ/mol | -704.2 kJ/mol total enthalpy | 0 kJ/mol | -1025 kJ/mol | 0 kJ/mol | -1408 kJ/mol | H_initial = -1025 kJ/mol | | H_final = -1408 kJ/mol | ΔH_rxn^0 | -1408 kJ/mol - -1025 kJ/mol = -383 kJ/mol (exothermic) | | |](../image_source/dd75b38b18bc47a43e9eb09d8fa5fc3d.png)
| aluminum | iron(II) chloride | iron | aluminum chloride molecular enthalpy | 0 kJ/mol | -341.8 kJ/mol | 0 kJ/mol | -704.2 kJ/mol total enthalpy | 0 kJ/mol | -1025 kJ/mol | 0 kJ/mol | -1408 kJ/mol | H_initial = -1025 kJ/mol | | H_final = -1408 kJ/mol | ΔH_rxn^0 | -1408 kJ/mol - -1025 kJ/mol = -383 kJ/mol (exothermic) | | |
Equilibrium constant
![Construct the equilibrium constant, K, expression for: Al + FeCl_2 ⟶ Fe + AlCl_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 Al + 3 FeCl_2 ⟶ 3 Fe + 2 AlCl_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 Al | 2 | -2 FeCl_2 | 3 | -3 Fe | 3 | 3 AlCl_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Al | 2 | -2 | ([Al])^(-2) FeCl_2 | 3 | -3 | ([FeCl2])^(-3) Fe | 3 | 3 | ([Fe])^3 AlCl_3 | 2 | 2 | ([AlCl3])^2 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 = ([Al])^(-2) ([FeCl2])^(-3) ([Fe])^3 ([AlCl3])^2 = (([Fe])^3 ([AlCl3])^2)/(([Al])^2 ([FeCl2])^3)](../image_source/94f28297ff46f0d85d63217c29315f47.png)
Construct the equilibrium constant, K, expression for: Al + FeCl_2 ⟶ Fe + AlCl_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 Al + 3 FeCl_2 ⟶ 3 Fe + 2 AlCl_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 Al | 2 | -2 FeCl_2 | 3 | -3 Fe | 3 | 3 AlCl_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Al | 2 | -2 | ([Al])^(-2) FeCl_2 | 3 | -3 | ([FeCl2])^(-3) Fe | 3 | 3 | ([Fe])^3 AlCl_3 | 2 | 2 | ([AlCl3])^2 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 = ([Al])^(-2) ([FeCl2])^(-3) ([Fe])^3 ([AlCl3])^2 = (([Fe])^3 ([AlCl3])^2)/(([Al])^2 ([FeCl2])^3)
Rate of reaction
![Construct the rate of reaction expression for: Al + FeCl_2 ⟶ Fe + AlCl_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 Al + 3 FeCl_2 ⟶ 3 Fe + 2 AlCl_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 Al | 2 | -2 FeCl_2 | 3 | -3 Fe | 3 | 3 AlCl_3 | 2 | 2 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 Al | 2 | -2 | -1/2 (Δ[Al])/(Δt) FeCl_2 | 3 | -3 | -1/3 (Δ[FeCl2])/(Δt) Fe | 3 | 3 | 1/3 (Δ[Fe])/(Δt) AlCl_3 | 2 | 2 | 1/2 (Δ[AlCl3])/(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[Al])/(Δt) = -1/3 (Δ[FeCl2])/(Δt) = 1/3 (Δ[Fe])/(Δt) = 1/2 (Δ[AlCl3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/650244ba2c3311bede8fc3ef755e6379.png)
Construct the rate of reaction expression for: Al + FeCl_2 ⟶ Fe + AlCl_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 Al + 3 FeCl_2 ⟶ 3 Fe + 2 AlCl_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 Al | 2 | -2 FeCl_2 | 3 | -3 Fe | 3 | 3 AlCl_3 | 2 | 2 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 Al | 2 | -2 | -1/2 (Δ[Al])/(Δt) FeCl_2 | 3 | -3 | -1/3 (Δ[FeCl2])/(Δt) Fe | 3 | 3 | 1/3 (Δ[Fe])/(Δt) AlCl_3 | 2 | 2 | 1/2 (Δ[AlCl3])/(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[Al])/(Δt) = -1/3 (Δ[FeCl2])/(Δt) = 1/3 (Δ[Fe])/(Δt) = 1/2 (Δ[AlCl3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| aluminum | iron(II) chloride | iron | aluminum chloride formula | Al | FeCl_2 | Fe | AlCl_3 Hill formula | Al | Cl_2Fe | Fe | AlCl_3 name | aluminum | iron(II) chloride | iron | aluminum chloride IUPAC name | aluminum | dichloroiron | iron | trichloroalumane](../image_source/7c44e4b6360c6650b309802e57ecad43.png)
| aluminum | iron(II) chloride | iron | aluminum chloride formula | Al | FeCl_2 | Fe | AlCl_3 Hill formula | Al | Cl_2Fe | Fe | AlCl_3 name | aluminum | iron(II) chloride | iron | aluminum chloride IUPAC name | aluminum | dichloroiron | iron | trichloroalumane
Substance properties
![| aluminum | iron(II) chloride | iron | aluminum chloride molar mass | 26.9815385 g/mol | 126.7 g/mol | 55.845 g/mol | 133.3 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 660.4 °C | 677 °C | 1535 °C | 190 °C boiling point | 2460 °C | | 2750 °C | density | 2.7 g/cm^3 | 3.16 g/cm^3 | 7.874 g/cm^3 | solubility in water | insoluble | | insoluble | surface tension | 0.817 N/m | | | dynamic viscosity | 1.5×10^-4 Pa s (at 760 °C) | | | odor | odorless | | |](../image_source/dddcbd2b6341b615152905cb4ea008d8.png)
| aluminum | iron(II) chloride | iron | aluminum chloride molar mass | 26.9815385 g/mol | 126.7 g/mol | 55.845 g/mol | 133.3 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 660.4 °C | 677 °C | 1535 °C | 190 °C boiling point | 2460 °C | | 2750 °C | density | 2.7 g/cm^3 | 3.16 g/cm^3 | 7.874 g/cm^3 | solubility in water | insoluble | | insoluble | surface tension | 0.817 N/m | | | dynamic viscosity | 1.5×10^-4 Pa s (at 760 °C) | | | odor | odorless | | |
Units