AlCl3 + N2OH = Al(OH)3 + N2Cl

AlCl_3 aluminum chloride + N2OH ⟶ Al(OH)_3 aluminum hydroxide + N2Cl

Balance the chemical equation algebraically: AlCl_3 + N2OH ⟶ Al(OH)_3 + N2Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AlCl_3 + c_2 N2OH ⟶ c_3 Al(OH)_3 + c_4 N2Cl Set the number of atoms in the reactants equal to the number of atoms in the products for Al, Cl, N, O and H: Al: | c_1 = c_3 Cl: | 3 c_1 = c_4 N: | 2 c_2 = 2 c_4 O: | c_2 = 3 c_3 H: | c_2 = 3 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 = 3 c_3 = 1 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | AlCl_3 + 3 N2OH ⟶ Al(OH)_3 + 3 N2Cl

+ N2OH ⟶ + N2Cl

aluminum chloride + N2OH ⟶ aluminum hydroxide + N2Cl

Construct the equilibrium constant, K, expression for: AlCl_3 + N2OH ⟶ Al(OH)_3 + N2Cl 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 + 3 N2OH ⟶ Al(OH)_3 + 3 N2Cl 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 N2OH | 3 | -3 Al(OH)_3 | 1 | 1 N2Cl | 3 | 3 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) N2OH | 3 | -3 | ([N2OH])^(-3) Al(OH)_3 | 1 | 1 | [Al(OH)3] N2Cl | 3 | 3 | ([N2Cl])^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 = ([AlCl3])^(-1) ([N2OH])^(-3) [Al(OH)3] ([N2Cl])^3 = ([Al(OH)3] ([N2Cl])^3)/([AlCl3] ([N2OH])^3)

Construct the rate of reaction expression for: AlCl_3 + N2OH ⟶ Al(OH)_3 + N2Cl 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 + 3 N2OH ⟶ Al(OH)_3 + 3 N2Cl 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 N2OH | 3 | -3 Al(OH)_3 | 1 | 1 N2Cl | 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 AlCl_3 | 1 | -1 | -(Δ[AlCl3])/(Δt) N2OH | 3 | -3 | -1/3 (Δ[N2OH])/(Δt) Al(OH)_3 | 1 | 1 | (Δ[Al(OH)3])/(Δt) N2Cl | 3 | 3 | 1/3 (Δ[N2Cl])/(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) = -1/3 (Δ[N2OH])/(Δt) = (Δ[Al(OH)3])/(Δt) = 1/3 (Δ[N2Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| aluminum chloride | N2OH | aluminum hydroxide | N2Cl formula | AlCl_3 | N2OH | Al(OH)_3 | N2Cl Hill formula | AlCl_3 | HN2O | AlH_3O_3 | ClN2 name | aluminum chloride | | aluminum hydroxide | IUPAC name | trichloroalumane | | aluminum hydroxide |

| aluminum chloride | N2OH | aluminum hydroxide | N2Cl molar mass | 133.3 g/mol | 45.021 g/mol | 78.003 g/mol | 63.46 g/mol phase | solid (at STP) | | | melting point | 190 °C | | |