H2O + Al = H2 + Al(OH)3

H_2O (water) + Al (aluminum) ⟶ H_2 (hydrogen) + Al(OH)_3 (aluminum hydroxide)

Balance the chemical equation algebraically: H_2O + Al ⟶ H_2 + Al(OH)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Al ⟶ c_3 H_2 + c_4 Al(OH)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and Al: H: | 2 c_1 = 2 c_3 + 3 c_4 O: | c_1 = 3 c_4 Al: | c_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 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 H_2O + 2 Al ⟶ 3 H_2 + 2 Al(OH)_3

+ ⟶ +

water + aluminum ⟶ hydrogen + aluminum hydroxide

Construct the equilibrium constant, K, expression for: H_2O + Al ⟶ H_2 + 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: 6 H_2O + 2 Al ⟶ 3 H_2 + 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 H_2O | 6 | -6 Al | 2 | -2 H_2 | 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 H_2O | 6 | -6 | ([H2O])^(-6) Al | 2 | -2 | ([Al])^(-2) H_2 | 3 | 3 | ([H2])^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 = ([H2O])^(-6) ([Al])^(-2) ([H2])^3 ([Al(OH)3])^2 = (([H2])^3 ([Al(OH)3])^2)/(([H2O])^6 ([Al])^2)

Construct the rate of reaction expression for: H_2O + Al ⟶ H_2 + 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: 6 H_2O + 2 Al ⟶ 3 H_2 + 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 H_2O | 6 | -6 Al | 2 | -2 H_2 | 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 H_2O | 6 | -6 | -1/6 (Δ[H2O])/(Δt) Al | 2 | -2 | -1/2 (Δ[Al])/(Δt) H_2 | 3 | 3 | 1/3 (Δ[H2])/(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 = -1/6 (Δ[H2O])/(Δt) = -1/2 (Δ[Al])/(Δt) = 1/3 (Δ[H2])/(Δt) = 1/2 (Δ[Al(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| water | aluminum | hydrogen | aluminum hydroxide formula | H_2O | Al | H_2 | Al(OH)_3 Hill formula | H_2O | Al | H_2 | AlH_3O_3 name | water | aluminum | hydrogen | aluminum hydroxide IUPAC name | water | aluminum | molecular hydrogen | aluminum hydroxide