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Na + Al(OH)3 = H2 + Na3AlO3

Input interpretation

Na sodium + Al(OH)_3 aluminum hydroxide ⟶ H_2 hydrogen + Na3AlO3
Na sodium + Al(OH)_3 aluminum hydroxide ⟶ H_2 hydrogen + Na3AlO3

Balanced equation

Balance the chemical equation algebraically: Na + Al(OH)_3 ⟶ H_2 + Na3AlO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Na + c_2 Al(OH)_3 ⟶ c_3 H_2 + c_4 Na3AlO3 Set the number of atoms in the reactants equal to the number of atoms in the products for Na, Al, H and O: Na: | c_1 = 3 c_4 Al: | c_2 = c_4 H: | 3 c_2 = 2 c_3 O: | 3 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 3/2 c_4 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 6 c_2 = 2 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 Na + 2 Al(OH)_3 ⟶ 3 H_2 + 2 Na3AlO3
Balance the chemical equation algebraically: Na + Al(OH)_3 ⟶ H_2 + Na3AlO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Na + c_2 Al(OH)_3 ⟶ c_3 H_2 + c_4 Na3AlO3 Set the number of atoms in the reactants equal to the number of atoms in the products for Na, Al, H and O: Na: | c_1 = 3 c_4 Al: | c_2 = c_4 H: | 3 c_2 = 2 c_3 O: | 3 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 3/2 c_4 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 6 c_2 = 2 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 Na + 2 Al(OH)_3 ⟶ 3 H_2 + 2 Na3AlO3

Structures

+ ⟶ + Na3AlO3
+ ⟶ + Na3AlO3

Names

sodium + aluminum hydroxide ⟶ hydrogen + Na3AlO3
sodium + aluminum hydroxide ⟶ hydrogen + Na3AlO3

Equilibrium constant

Construct the equilibrium constant, K, expression for: Na + Al(OH)_3 ⟶ H_2 + Na3AlO3 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: 6 Na + 2 Al(OH)_3 ⟶ 3 H_2 + 2 Na3AlO3 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 Na | 6 | -6 Al(OH)_3 | 2 | -2 H_2 | 3 | 3 Na3AlO3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Na | 6 | -6 | ([Na])^(-6) Al(OH)_3 | 2 | -2 | ([Al(OH)3])^(-2) H_2 | 3 | 3 | ([H2])^3 Na3AlO3 | 2 | 2 | ([Na3AlO3])^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 = ([Na])^(-6) ([Al(OH)3])^(-2) ([H2])^3 ([Na3AlO3])^2 = (([H2])^3 ([Na3AlO3])^2)/(([Na])^6 ([Al(OH)3])^2)
Construct the equilibrium constant, K, expression for: Na + Al(OH)_3 ⟶ H_2 + Na3AlO3 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: 6 Na + 2 Al(OH)_3 ⟶ 3 H_2 + 2 Na3AlO3 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 Na | 6 | -6 Al(OH)_3 | 2 | -2 H_2 | 3 | 3 Na3AlO3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Na | 6 | -6 | ([Na])^(-6) Al(OH)_3 | 2 | -2 | ([Al(OH)3])^(-2) H_2 | 3 | 3 | ([H2])^3 Na3AlO3 | 2 | 2 | ([Na3AlO3])^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 = ([Na])^(-6) ([Al(OH)3])^(-2) ([H2])^3 ([Na3AlO3])^2 = (([H2])^3 ([Na3AlO3])^2)/(([Na])^6 ([Al(OH)3])^2)

Rate of reaction

Construct the rate of reaction expression for: Na + Al(OH)_3 ⟶ H_2 + Na3AlO3 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: 6 Na + 2 Al(OH)_3 ⟶ 3 H_2 + 2 Na3AlO3 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 Na | 6 | -6 Al(OH)_3 | 2 | -2 H_2 | 3 | 3 Na3AlO3 | 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 Na | 6 | -6 | -1/6 (Δ[Na])/(Δt) Al(OH)_3 | 2 | -2 | -1/2 (Δ[Al(OH)3])/(Δt) H_2 | 3 | 3 | 1/3 (Δ[H2])/(Δt) Na3AlO3 | 2 | 2 | 1/2 (Δ[Na3AlO3])/(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 = -1/6 (Δ[Na])/(Δt) = -1/2 (Δ[Al(OH)3])/(Δt) = 1/3 (Δ[H2])/(Δt) = 1/2 (Δ[Na3AlO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Na + Al(OH)_3 ⟶ H_2 + Na3AlO3 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: 6 Na + 2 Al(OH)_3 ⟶ 3 H_2 + 2 Na3AlO3 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 Na | 6 | -6 Al(OH)_3 | 2 | -2 H_2 | 3 | 3 Na3AlO3 | 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 Na | 6 | -6 | -1/6 (Δ[Na])/(Δt) Al(OH)_3 | 2 | -2 | -1/2 (Δ[Al(OH)3])/(Δt) H_2 | 3 | 3 | 1/3 (Δ[H2])/(Δt) Na3AlO3 | 2 | 2 | 1/2 (Δ[Na3AlO3])/(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 = -1/6 (Δ[Na])/(Δt) = -1/2 (Δ[Al(OH)3])/(Δt) = 1/3 (Δ[H2])/(Δt) = 1/2 (Δ[Na3AlO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium | aluminum hydroxide | hydrogen | Na3AlO3 formula | Na | Al(OH)_3 | H_2 | Na3AlO3 Hill formula | Na | AlH_3O_3 | H_2 | AlNa3O3 name | sodium | aluminum hydroxide | hydrogen | IUPAC name | sodium | aluminum hydroxide | molecular hydrogen |
| sodium | aluminum hydroxide | hydrogen | Na3AlO3 formula | Na | Al(OH)_3 | H_2 | Na3AlO3 Hill formula | Na | AlH_3O_3 | H_2 | AlNa3O3 name | sodium | aluminum hydroxide | hydrogen | IUPAC name | sodium | aluminum hydroxide | molecular hydrogen |

Substance properties

| sodium | aluminum hydroxide | hydrogen | Na3AlO3 molar mass | 22.98976928 g/mol | 78.003 g/mol | 2.016 g/mol | 143.95 g/mol phase | solid (at STP) | | gas (at STP) | melting point | 97.8 °C | | -259.2 °C | boiling point | 883 °C | | -252.8 °C | density | 0.968 g/cm^3 | | 8.99×10^-5 g/cm^3 (at 0 °C) | solubility in water | decomposes | | | dynamic viscosity | 1.413×10^-5 Pa s (at 527 °C) | | 8.9×10^-6 Pa s (at 25 °C) | odor | | | odorless |
| sodium | aluminum hydroxide | hydrogen | Na3AlO3 molar mass | 22.98976928 g/mol | 78.003 g/mol | 2.016 g/mol | 143.95 g/mol phase | solid (at STP) | | gas (at STP) | melting point | 97.8 °C | | -259.2 °C | boiling point | 883 °C | | -252.8 °C | density | 0.968 g/cm^3 | | 8.99×10^-5 g/cm^3 (at 0 °C) | solubility in water | decomposes | | | dynamic viscosity | 1.413×10^-5 Pa s (at 527 °C) | | 8.9×10^-6 Pa s (at 25 °C) | odor | | | odorless |

Units

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