NH3 + SnCl4 = HCl + N2 + SnCl3

NH_3 ammonia + SnCl_4 stannic chloride ⟶ HCl hydrogen chloride + N_2 nitrogen + SnCl3

Balance the chemical equation algebraically: NH_3 + SnCl_4 ⟶ HCl + N_2 + SnCl3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH_3 + c_2 SnCl_4 ⟶ c_3 HCl + c_4 N_2 + c_5 SnCl3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, Cl and Sn: H: | 3 c_1 = c_3 N: | c_1 = 2 c_4 Cl: | 4 c_2 = c_3 + 3 c_5 Sn: | c_2 = c_5 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 6 c_3 = 6 c_4 = 1 c_5 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NH_3 + 6 SnCl_4 ⟶ 6 HCl + N_2 + 6 SnCl3

+ ⟶ + + SnCl3

ammonia + stannic chloride ⟶ hydrogen chloride + nitrogen + SnCl3

Construct the equilibrium constant, K, expression for: NH_3 + SnCl_4 ⟶ HCl + N_2 + SnCl3 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: 2 NH_3 + 6 SnCl_4 ⟶ 6 HCl + N_2 + 6 SnCl3 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 NH_3 | 2 | -2 SnCl_4 | 6 | -6 HCl | 6 | 6 N_2 | 1 | 1 SnCl3 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NH_3 | 2 | -2 | ([NH3])^(-2) SnCl_4 | 6 | -6 | ([SnCl4])^(-6) HCl | 6 | 6 | ([HCl])^6 N_2 | 1 | 1 | [N2] SnCl3 | 6 | 6 | ([SnCl3])^6 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 = ([NH3])^(-2) ([SnCl4])^(-6) ([HCl])^6 [N2] ([SnCl3])^6 = (([HCl])^6 [N2] ([SnCl3])^6)/(([NH3])^2 ([SnCl4])^6)

Construct the rate of reaction expression for: NH_3 + SnCl_4 ⟶ HCl + N_2 + SnCl3 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: 2 NH_3 + 6 SnCl_4 ⟶ 6 HCl + N_2 + 6 SnCl3 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 NH_3 | 2 | -2 SnCl_4 | 6 | -6 HCl | 6 | 6 N_2 | 1 | 1 SnCl3 | 6 | 6 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 NH_3 | 2 | -2 | -1/2 (Δ[NH3])/(Δt) SnCl_4 | 6 | -6 | -1/6 (Δ[SnCl4])/(Δt) HCl | 6 | 6 | 1/6 (Δ[HCl])/(Δt) N_2 | 1 | 1 | (Δ[N2])/(Δt) SnCl3 | 6 | 6 | 1/6 (Δ[SnCl3])/(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 = -1/2 (Δ[NH3])/(Δt) = -1/6 (Δ[SnCl4])/(Δt) = 1/6 (Δ[HCl])/(Δt) = (Δ[N2])/(Δt) = 1/6 (Δ[SnCl3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| ammonia | stannic chloride | hydrogen chloride | nitrogen | SnCl3 formula | NH_3 | SnCl_4 | HCl | N_2 | SnCl3 Hill formula | H_3N | Cl_4Sn | ClH | N_2 | Cl3Sn name | ammonia | stannic chloride | hydrogen chloride | nitrogen | IUPAC name | ammonia | tetrachlorostannane | hydrogen chloride | molecular nitrogen |

| ammonia | stannic chloride | hydrogen chloride | nitrogen | SnCl3 molar mass | 17.031 g/mol | 260.5 g/mol | 36.46 g/mol | 28.014 g/mol | 225.1 g/mol phase | gas (at STP) | liquid (at STP) | gas (at STP) | gas (at STP) | melting point | -77.73 °C | -33 °C | -114.17 °C | -210 °C | boiling point | -33.33 °C | 114 °C | -85 °C | -195.79 °C | density | 6.96×10^-4 g/cm^3 (at 25 °C) | 2.226 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 0.001251 g/cm^3 (at 0 °C) | solubility in water | | soluble | miscible | insoluble | surface tension | 0.0234 N/m | | | 0.0066 N/m | dynamic viscosity | 1.009×10^-5 Pa s (at 25 °C) | 5.8×10^-4 Pa s (at 60 °C) | | 1.78×10^-5 Pa s (at 25 °C) | odor | | | | odorless |