HNO3 + AlCl3 = HCl + Al(NO3)3

HNO_3 nitric acid + AlCl_3 aluminum chloride ⟶ HCl hydrogen chloride + Al(NO_3)_3 aluminum nitrate

Balance the chemical equation algebraically: HNO_3 + AlCl_3 ⟶ HCl + Al(NO_3)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 AlCl_3 ⟶ c_3 HCl + c_4 Al(NO_3)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, Al and Cl: H: | c_1 = c_3 N: | c_1 = 3 c_4 O: | 3 c_1 = 9 c_4 Al: | c_2 = c_4 Cl: | 3 c_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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 HNO_3 + AlCl_3 ⟶ 3 HCl + Al(NO_3)_3

+ ⟶ +

nitric acid + aluminum chloride ⟶ hydrogen chloride + aluminum nitrate

Construct the equilibrium constant, K, expression for: HNO_3 + AlCl_3 ⟶ HCl + Al(NO_3)_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: 3 HNO_3 + AlCl_3 ⟶ 3 HCl + Al(NO_3)_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 HNO_3 | 3 | -3 AlCl_3 | 1 | -1 HCl | 3 | 3 Al(NO_3)_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 3 | -3 | ([HNO3])^(-3) AlCl_3 | 1 | -1 | ([AlCl3])^(-1) HCl | 3 | 3 | ([HCl])^3 Al(NO_3)_3 | 1 | 1 | [Al(NO3)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 = ([HNO3])^(-3) ([AlCl3])^(-1) ([HCl])^3 [Al(NO3)3] = (([HCl])^3 [Al(NO3)3])/(([HNO3])^3 [AlCl3])

Construct the rate of reaction expression for: HNO_3 + AlCl_3 ⟶ HCl + Al(NO_3)_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: 3 HNO_3 + AlCl_3 ⟶ 3 HCl + Al(NO_3)_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 HNO_3 | 3 | -3 AlCl_3 | 1 | -1 HCl | 3 | 3 Al(NO_3)_3 | 1 | 1 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 HNO_3 | 3 | -3 | -1/3 (Δ[HNO3])/(Δt) AlCl_3 | 1 | -1 | -(Δ[AlCl3])/(Δt) HCl | 3 | 3 | 1/3 (Δ[HCl])/(Δt) Al(NO_3)_3 | 1 | 1 | (Δ[Al(NO3)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 = -1/3 (Δ[HNO3])/(Δt) = -(Δ[AlCl3])/(Δt) = 1/3 (Δ[HCl])/(Δt) = (Δ[Al(NO3)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| nitric acid | aluminum chloride | hydrogen chloride | aluminum nitrate formula | HNO_3 | AlCl_3 | HCl | Al(NO_3)_3 Hill formula | HNO_3 | AlCl_3 | ClH | AlN_3O_9 name | nitric acid | aluminum chloride | hydrogen chloride | aluminum nitrate IUPAC name | nitric acid | trichloroalumane | hydrogen chloride | aluminum(+3) cation trinitrate

| nitric acid | aluminum chloride | hydrogen chloride | aluminum nitrate molar mass | 63.012 g/mol | 133.3 g/mol | 36.46 g/mol | 212.99 g/mol phase | liquid (at STP) | solid (at STP) | gas (at STP) | solid (at STP) melting point | -41.6 °C | 190 °C | -114.17 °C | 72.8 °C boiling point | 83 °C | | -85 °C | density | 1.5129 g/cm^3 | | 0.00149 g/cm^3 (at 25 °C) | 1.401 g/cm^3 solubility in water | miscible | | miscible | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | | 0.001338 Pa s (at 22 °C)