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AlCl3 + K3[Al(OH)6] = KCl + Al(OH)3

Input interpretation

AlCl_3 aluminum chloride + K3Al(OH)6 ⟶ KCl potassium chloride + Al(OH)_3 aluminum hydroxide
AlCl_3 aluminum chloride + K3Al(OH)6 ⟶ KCl potassium chloride + Al(OH)_3 aluminum hydroxide

Balanced equation

Balance the chemical equation algebraically: AlCl_3 + K3Al(OH)6 ⟶ KCl + Al(OH)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AlCl_3 + c_2 K3Al(OH)6 ⟶ c_3 KCl + c_4 Al(OH)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Al, Cl, K, O and H: Al: | c_1 + c_2 = c_4 Cl: | 3 c_1 = c_3 K: | 3 c_2 = c_3 O: | 6 c_2 = 3 c_4 H: | 6 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 = 1 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | AlCl_3 + K3Al(OH)6 ⟶ 3 KCl + 2 Al(OH)_3
Balance the chemical equation algebraically: AlCl_3 + K3Al(OH)6 ⟶ KCl + Al(OH)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AlCl_3 + c_2 K3Al(OH)6 ⟶ c_3 KCl + c_4 Al(OH)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Al, Cl, K, O and H: Al: | c_1 + c_2 = c_4 Cl: | 3 c_1 = c_3 K: | 3 c_2 = c_3 O: | 6 c_2 = 3 c_4 H: | 6 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 = 1 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | AlCl_3 + K3Al(OH)6 ⟶ 3 KCl + 2 Al(OH)_3

Structures

+ K3Al(OH)6 ⟶ +
+ K3Al(OH)6 ⟶ +

Names

aluminum chloride + K3Al(OH)6 ⟶ potassium chloride + aluminum hydroxide
aluminum chloride + K3Al(OH)6 ⟶ potassium chloride + aluminum hydroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: AlCl_3 + K3Al(OH)6 ⟶ KCl + Al(OH)_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: AlCl_3 + K3Al(OH)6 ⟶ 3 KCl + 2 Al(OH)_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 AlCl_3 | 1 | -1 K3Al(OH)6 | 1 | -1 KCl | 3 | 3 Al(OH)_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression AlCl_3 | 1 | -1 | ([AlCl3])^(-1) K3Al(OH)6 | 1 | -1 | ([K3Al(OH)6])^(-1) KCl | 3 | 3 | ([KCl])^3 Al(OH)_3 | 2 | 2 | ([Al(OH)3])^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 = ([AlCl3])^(-1) ([K3Al(OH)6])^(-1) ([KCl])^3 ([Al(OH)3])^2 = (([KCl])^3 ([Al(OH)3])^2)/([AlCl3] [K3Al(OH)6])
Construct the equilibrium constant, K, expression for: AlCl_3 + K3Al(OH)6 ⟶ KCl + Al(OH)_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: AlCl_3 + K3Al(OH)6 ⟶ 3 KCl + 2 Al(OH)_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 AlCl_3 | 1 | -1 K3Al(OH)6 | 1 | -1 KCl | 3 | 3 Al(OH)_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression AlCl_3 | 1 | -1 | ([AlCl3])^(-1) K3Al(OH)6 | 1 | -1 | ([K3Al(OH)6])^(-1) KCl | 3 | 3 | ([KCl])^3 Al(OH)_3 | 2 | 2 | ([Al(OH)3])^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 = ([AlCl3])^(-1) ([K3Al(OH)6])^(-1) ([KCl])^3 ([Al(OH)3])^2 = (([KCl])^3 ([Al(OH)3])^2)/([AlCl3] [K3Al(OH)6])

Rate of reaction

Construct the rate of reaction expression for: AlCl_3 + K3Al(OH)6 ⟶ KCl + Al(OH)_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: AlCl_3 + K3Al(OH)6 ⟶ 3 KCl + 2 Al(OH)_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 AlCl_3 | 1 | -1 K3Al(OH)6 | 1 | -1 KCl | 3 | 3 Al(OH)_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 AlCl_3 | 1 | -1 | -(Δ[AlCl3])/(Δt) K3Al(OH)6 | 1 | -1 | -(Δ[K3Al(OH)6])/(Δt) KCl | 3 | 3 | 1/3 (Δ[KCl])/(Δt) Al(OH)_3 | 2 | 2 | 1/2 (Δ[Al(OH)3])/(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[AlCl3])/(Δt) = -(Δ[K3Al(OH)6])/(Δt) = 1/3 (Δ[KCl])/(Δt) = 1/2 (Δ[Al(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: AlCl_3 + K3Al(OH)6 ⟶ KCl + Al(OH)_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: AlCl_3 + K3Al(OH)6 ⟶ 3 KCl + 2 Al(OH)_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 AlCl_3 | 1 | -1 K3Al(OH)6 | 1 | -1 KCl | 3 | 3 Al(OH)_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 AlCl_3 | 1 | -1 | -(Δ[AlCl3])/(Δt) K3Al(OH)6 | 1 | -1 | -(Δ[K3Al(OH)6])/(Δt) KCl | 3 | 3 | 1/3 (Δ[KCl])/(Δt) Al(OH)_3 | 2 | 2 | 1/2 (Δ[Al(OH)3])/(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[AlCl3])/(Δt) = -(Δ[K3Al(OH)6])/(Δt) = 1/3 (Δ[KCl])/(Δt) = 1/2 (Δ[Al(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| aluminum chloride | K3Al(OH)6 | potassium chloride | aluminum hydroxide formula | AlCl_3 | K3Al(OH)6 | KCl | Al(OH)_3 Hill formula | AlCl_3 | H6AlK3O6 | ClK | AlH_3O_3 name | aluminum chloride | | potassium chloride | aluminum hydroxide IUPAC name | trichloroalumane | | potassium chloride | aluminum hydroxide
| aluminum chloride | K3Al(OH)6 | potassium chloride | aluminum hydroxide formula | AlCl_3 | K3Al(OH)6 | KCl | Al(OH)_3 Hill formula | AlCl_3 | H6AlK3O6 | ClK | AlH_3O_3 name | aluminum chloride | | potassium chloride | aluminum hydroxide IUPAC name | trichloroalumane | | potassium chloride | aluminum hydroxide

Substance properties

| aluminum chloride | K3Al(OH)6 | potassium chloride | aluminum hydroxide molar mass | 133.3 g/mol | 246.32 g/mol | 74.55 g/mol | 78.003 g/mol phase | solid (at STP) | | solid (at STP) | melting point | 190 °C | | 770 °C | boiling point | | | 1420 °C | density | | | 1.98 g/cm^3 | solubility in water | | | soluble | odor | | | odorless |
| aluminum chloride | K3Al(OH)6 | potassium chloride | aluminum hydroxide molar mass | 133.3 g/mol | 246.32 g/mol | 74.55 g/mol | 78.003 g/mol phase | solid (at STP) | | solid (at STP) | melting point | 190 °C | | 770 °C | boiling point | | | 1420 °C | density | | | 1.98 g/cm^3 | solubility in water | | | soluble | odor | | | odorless |

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