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Ca + AlCl3 = Al + CaCl2

Input interpretation

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

Balanced equation

Balance the chemical equation algebraically: Ca + AlCl_3 ⟶ Al + CaCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca + c_2 AlCl_3 ⟶ c_3 Al + c_4 CaCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, Al and Cl: Ca: | c_1 = c_4 Al: | c_2 = c_3 Cl: | 3 c_2 = 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 = 3/2 c_2 = 1 c_3 = 1 c_4 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 2 c_3 = 2 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: |   | 3 Ca + 2 AlCl_3 ⟶ 2 Al + 3 CaCl_2
Balance the chemical equation algebraically: Ca + AlCl_3 ⟶ Al + CaCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca + c_2 AlCl_3 ⟶ c_3 Al + c_4 CaCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, Al and Cl: Ca: | c_1 = c_4 Al: | c_2 = c_3 Cl: | 3 c_2 = 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 = 3/2 c_2 = 1 c_3 = 1 c_4 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 2 c_3 = 2 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Ca + 2 AlCl_3 ⟶ 2 Al + 3 CaCl_2

Structures

 + ⟶ +
+ ⟶ +

Names

calcium + aluminum chloride ⟶ aluminum + calcium chloride
calcium + aluminum chloride ⟶ aluminum + calcium chloride

Reaction thermodynamics

Enthalpy

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

Equilibrium constant

Construct the equilibrium constant, K, expression for: Ca + AlCl_3 ⟶ Al + CaCl_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: 3 Ca + 2 AlCl_3 ⟶ 2 Al + 3 CaCl_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 Ca | 3 | -3 AlCl_3 | 2 | -2 Al | 2 | 2 CaCl_2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ca | 3 | -3 | ([Ca])^(-3) AlCl_3 | 2 | -2 | ([AlCl3])^(-2) Al | 2 | 2 | ([Al])^2 CaCl_2 | 3 | 3 | ([CaCl2])^3 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 = ([Ca])^(-3) ([AlCl3])^(-2) ([Al])^2 ([CaCl2])^3 = (([Al])^2 ([CaCl2])^3)/(([Ca])^3 ([AlCl3])^2)
Construct the equilibrium constant, K, expression for: Ca + AlCl_3 ⟶ Al + CaCl_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: 3 Ca + 2 AlCl_3 ⟶ 2 Al + 3 CaCl_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 Ca | 3 | -3 AlCl_3 | 2 | -2 Al | 2 | 2 CaCl_2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ca | 3 | -3 | ([Ca])^(-3) AlCl_3 | 2 | -2 | ([AlCl3])^(-2) Al | 2 | 2 | ([Al])^2 CaCl_2 | 3 | 3 | ([CaCl2])^3 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 = ([Ca])^(-3) ([AlCl3])^(-2) ([Al])^2 ([CaCl2])^3 = (([Al])^2 ([CaCl2])^3)/(([Ca])^3 ([AlCl3])^2)

Rate of reaction

Construct the rate of reaction expression for: Ca + AlCl_3 ⟶ Al + CaCl_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: 3 Ca + 2 AlCl_3 ⟶ 2 Al + 3 CaCl_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 Ca | 3 | -3 AlCl_3 | 2 | -2 Al | 2 | 2 CaCl_2 | 3 | 3 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 Ca | 3 | -3 | -1/3 (Δ[Ca])/(Δt) AlCl_3 | 2 | -2 | -1/2 (Δ[AlCl3])/(Δt) Al | 2 | 2 | 1/2 (Δ[Al])/(Δt) CaCl_2 | 3 | 3 | 1/3 (Δ[CaCl2])/(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 = -1/3 (Δ[Ca])/(Δt) = -1/2 (Δ[AlCl3])/(Δt) = 1/2 (Δ[Al])/(Δt) = 1/3 (Δ[CaCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Ca + AlCl_3 ⟶ Al + CaCl_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: 3 Ca + 2 AlCl_3 ⟶ 2 Al + 3 CaCl_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 Ca | 3 | -3 AlCl_3 | 2 | -2 Al | 2 | 2 CaCl_2 | 3 | 3 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 Ca | 3 | -3 | -1/3 (Δ[Ca])/(Δt) AlCl_3 | 2 | -2 | -1/2 (Δ[AlCl3])/(Δt) Al | 2 | 2 | 1/2 (Δ[Al])/(Δt) CaCl_2 | 3 | 3 | 1/3 (Δ[CaCl2])/(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 = -1/3 (Δ[Ca])/(Δt) = -1/2 (Δ[AlCl3])/(Δt) = 1/2 (Δ[Al])/(Δt) = 1/3 (Δ[CaCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

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

Substance properties

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

Units