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Al2(SO4)3 + Na3[AlF6] = Na2SO4 + AlF3

Input interpretation

Al_2(SO_4)_3 aluminum sulfate + Na_3AlF_6 sodium hexafluoroaluminate ⟶ Na_2SO_4 sodium sulfate + AlF_3 aluminum fluoride
Al_2(SO_4)_3 aluminum sulfate + Na_3AlF_6 sodium hexafluoroaluminate ⟶ Na_2SO_4 sodium sulfate + AlF_3 aluminum fluoride

Balanced equation

Balance the chemical equation algebraically: Al_2(SO_4)_3 + Na_3AlF_6 ⟶ Na_2SO_4 + AlF_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Al_2(SO_4)_3 + c_2 Na_3AlF_6 ⟶ c_3 Na_2SO_4 + c_4 AlF_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Al, O, S, F and Na: Al: | 2 c_1 + c_2 = c_4 O: | 12 c_1 = 4 c_3 S: | 3 c_1 = c_3 F: | 6 c_2 = 3 c_4 Na: | 3 c_2 = 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 = 2 c_3 = 3 c_4 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Al_2(SO_4)_3 + 2 Na_3AlF_6 ⟶ 3 Na_2SO_4 + 4 AlF_3
Balance the chemical equation algebraically: Al_2(SO_4)_3 + Na_3AlF_6 ⟶ Na_2SO_4 + AlF_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Al_2(SO_4)_3 + c_2 Na_3AlF_6 ⟶ c_3 Na_2SO_4 + c_4 AlF_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Al, O, S, F and Na: Al: | 2 c_1 + c_2 = c_4 O: | 12 c_1 = 4 c_3 S: | 3 c_1 = c_3 F: | 6 c_2 = 3 c_4 Na: | 3 c_2 = 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 = 2 c_3 = 3 c_4 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Al_2(SO_4)_3 + 2 Na_3AlF_6 ⟶ 3 Na_2SO_4 + 4 AlF_3

Structures

+ ⟶ +
+ ⟶ +

Names

aluminum sulfate + sodium hexafluoroaluminate ⟶ sodium sulfate + aluminum fluoride
aluminum sulfate + sodium hexafluoroaluminate ⟶ sodium sulfate + aluminum fluoride

Equilibrium constant

Construct the equilibrium constant, K, expression for: Al_2(SO_4)_3 + Na_3AlF_6 ⟶ Na_2SO_4 + AlF_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: Al_2(SO_4)_3 + 2 Na_3AlF_6 ⟶ 3 Na_2SO_4 + 4 AlF_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(SO_4)_3 | 1 | -1 Na_3AlF_6 | 2 | -2 Na_2SO_4 | 3 | 3 AlF_3 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Al_2(SO_4)_3 | 1 | -1 | ([Al2(SO4)3])^(-1) Na_3AlF_6 | 2 | -2 | ([Na3AlF6])^(-2) Na_2SO_4 | 3 | 3 | ([Na2SO4])^3 AlF_3 | 4 | 4 | ([AlF3])^4 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 = ([Al2(SO4)3])^(-1) ([Na3AlF6])^(-2) ([Na2SO4])^3 ([AlF3])^4 = (([Na2SO4])^3 ([AlF3])^4)/([Al2(SO4)3] ([Na3AlF6])^2)
Construct the equilibrium constant, K, expression for: Al_2(SO_4)_3 + Na_3AlF_6 ⟶ Na_2SO_4 + AlF_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: Al_2(SO_4)_3 + 2 Na_3AlF_6 ⟶ 3 Na_2SO_4 + 4 AlF_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(SO_4)_3 | 1 | -1 Na_3AlF_6 | 2 | -2 Na_2SO_4 | 3 | 3 AlF_3 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Al_2(SO_4)_3 | 1 | -1 | ([Al2(SO4)3])^(-1) Na_3AlF_6 | 2 | -2 | ([Na3AlF6])^(-2) Na_2SO_4 | 3 | 3 | ([Na2SO4])^3 AlF_3 | 4 | 4 | ([AlF3])^4 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 = ([Al2(SO4)3])^(-1) ([Na3AlF6])^(-2) ([Na2SO4])^3 ([AlF3])^4 = (([Na2SO4])^3 ([AlF3])^4)/([Al2(SO4)3] ([Na3AlF6])^2)

Rate of reaction

Construct the rate of reaction expression for: Al_2(SO_4)_3 + Na_3AlF_6 ⟶ Na_2SO_4 + AlF_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: Al_2(SO_4)_3 + 2 Na_3AlF_6 ⟶ 3 Na_2SO_4 + 4 AlF_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(SO_4)_3 | 1 | -1 Na_3AlF_6 | 2 | -2 Na_2SO_4 | 3 | 3 AlF_3 | 4 | 4 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(SO_4)_3 | 1 | -1 | -(Δ[Al2(SO4)3])/(Δt) Na_3AlF_6 | 2 | -2 | -1/2 (Δ[Na3AlF6])/(Δt) Na_2SO_4 | 3 | 3 | 1/3 (Δ[Na2SO4])/(Δt) AlF_3 | 4 | 4 | 1/4 (Δ[AlF3])/(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[Al2(SO4)3])/(Δt) = -1/2 (Δ[Na3AlF6])/(Δt) = 1/3 (Δ[Na2SO4])/(Δt) = 1/4 (Δ[AlF3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Al_2(SO_4)_3 + Na_3AlF_6 ⟶ Na_2SO_4 + AlF_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: Al_2(SO_4)_3 + 2 Na_3AlF_6 ⟶ 3 Na_2SO_4 + 4 AlF_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(SO_4)_3 | 1 | -1 Na_3AlF_6 | 2 | -2 Na_2SO_4 | 3 | 3 AlF_3 | 4 | 4 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(SO_4)_3 | 1 | -1 | -(Δ[Al2(SO4)3])/(Δt) Na_3AlF_6 | 2 | -2 | -1/2 (Δ[Na3AlF6])/(Δt) Na_2SO_4 | 3 | 3 | 1/3 (Δ[Na2SO4])/(Δt) AlF_3 | 4 | 4 | 1/4 (Δ[AlF3])/(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[Al2(SO4)3])/(Δt) = -1/2 (Δ[Na3AlF6])/(Δt) = 1/3 (Δ[Na2SO4])/(Δt) = 1/4 (Δ[AlF3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| aluminum sulfate | sodium hexafluoroaluminate | sodium sulfate | aluminum fluoride formula | Al_2(SO_4)_3 | Na_3AlF_6 | Na_2SO_4 | AlF_3 Hill formula | Al_2O_12S_3 | AlF_6Na_3 | Na_2O_4S | AlF_3 name | aluminum sulfate | sodium hexafluoroaluminate | sodium sulfate | aluminum fluoride IUPAC name | dialuminum trisulfate | trisodium hexafluoroaluminum | disodium sulfate | trifluoroalumane
| aluminum sulfate | sodium hexafluoroaluminate | sodium sulfate | aluminum fluoride formula | Al_2(SO_4)_3 | Na_3AlF_6 | Na_2SO_4 | AlF_3 Hill formula | Al_2O_12S_3 | AlF_6Na_3 | Na_2O_4S | AlF_3 name | aluminum sulfate | sodium hexafluoroaluminate | sodium sulfate | aluminum fluoride IUPAC name | dialuminum trisulfate | trisodium hexafluoroaluminum | disodium sulfate | trifluoroalumane

Substance properties

| aluminum sulfate | sodium hexafluoroaluminate | sodium sulfate | aluminum fluoride molar mass | 342.1 g/mol | 209.9412653 g/mol | 142.04 g/mol | 83.976748 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 770 °C | 977 °C | 884 °C | 1040 °C boiling point | | | 1429 °C | density | 2.71 g/cm^3 | 2.9 g/cm^3 | 2.68 g/cm^3 | 3.1 g/cm^3 solubility in water | soluble | insoluble | soluble |
| aluminum sulfate | sodium hexafluoroaluminate | sodium sulfate | aluminum fluoride molar mass | 342.1 g/mol | 209.9412653 g/mol | 142.04 g/mol | 83.976748 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 770 °C | 977 °C | 884 °C | 1040 °C boiling point | | | 1429 °C | density | 2.71 g/cm^3 | 2.9 g/cm^3 | 2.68 g/cm^3 | 3.1 g/cm^3 solubility in water | soluble | insoluble | soluble |

Units

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