Al + CaCl2 = Ca + AlCl3

Al aluminum + CaCl_2 calcium chloride ⟶ Ca calcium + AlCl_3 aluminum chloride

Balance the chemical equation algebraically: Al + CaCl_2 ⟶ Ca + AlCl_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Al + c_2 CaCl_2 ⟶ c_3 Ca + c_4 AlCl_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Al, Ca and Cl: Al: | c_1 = c_4 Ca: | c_2 = c_3 Cl: | 2 c_2 = 3 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 = 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 CaCl_2 ⟶ 3 Ca + 2 AlCl_3

+ ⟶ +

aluminum + calcium chloride ⟶ calcium + aluminum chloride

| aluminum | calcium chloride | calcium | aluminum chloride molecular enthalpy | 0 kJ/mol | -795.4 kJ/mol | 0 kJ/mol | -704.2 kJ/mol total enthalpy | 0 kJ/mol | -2386 kJ/mol | 0 kJ/mol | -1408 kJ/mol | H_initial = -2386 kJ/mol | | H_final = -1408 kJ/mol | ΔH_rxn^0 | -1408 kJ/mol - -2386 kJ/mol = 977.8 kJ/mol (endothermic) | | |

Construct the equilibrium constant, K, expression for: Al + CaCl_2 ⟶ Ca + 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 CaCl_2 ⟶ 3 Ca + 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 CaCl_2 | 3 | -3 Ca | 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) CaCl_2 | 3 | -3 | ([CaCl2])^(-3) Ca | 3 | 3 | ([Ca])^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) ([CaCl2])^(-3) ([Ca])^3 ([AlCl3])^2 = (([Ca])^3 ([AlCl3])^2)/(([Al])^2 ([CaCl2])^3)

Construct the rate of reaction expression for: Al + CaCl_2 ⟶ Ca + 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 CaCl_2 ⟶ 3 Ca + 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 CaCl_2 | 3 | -3 Ca | 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) CaCl_2 | 3 | -3 | -1/3 (Δ[CaCl2])/(Δt) Ca | 3 | 3 | 1/3 (Δ[Ca])/(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[CaCl2])/(Δt) = 1/3 (Δ[Ca])/(Δt) = 1/2 (Δ[AlCl3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| aluminum | calcium chloride | calcium | aluminum chloride formula | Al | CaCl_2 | Ca | AlCl_3 name | aluminum | calcium chloride | calcium | aluminum chloride IUPAC name | aluminum | calcium dichloride | calcium | trichloroalumane

| aluminum | calcium chloride | calcium | aluminum chloride molar mass | 26.9815385 g/mol | 111 g/mol | 40.078 g/mol | 133.3 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 660.4 °C | 772 °C | 850 °C | 190 °C boiling point | 2460 °C | | 1484 °C | density | 2.7 g/cm^3 | 2.15 g/cm^3 | 1.54 g/cm^3 | solubility in water | insoluble | soluble | decomposes | surface tension | 0.817 N/m | | | dynamic viscosity | 1.5×10^-4 Pa s (at 760 °C) | | | odor | odorless | | |