Cl2 + SnCl2 = SnCl4

Cl_2 chlorine + SnCl_2 stannous chloride ⟶ SnCl_4 stannic chloride

Balance the chemical equation algebraically: Cl_2 + SnCl_2 ⟶ SnCl_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 SnCl_2 ⟶ c_3 SnCl_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl and Sn: Cl: | 2 c_1 + 2 c_2 = 4 c_3 Sn: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Cl_2 + SnCl_2 ⟶ SnCl_4

+ ⟶

chlorine + stannous chloride ⟶ stannic chloride

Construct the equilibrium constant, K, expression for: Cl_2 + SnCl_2 ⟶ SnCl_4 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: Cl_2 + SnCl_2 ⟶ SnCl_4 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 Cl_2 | 1 | -1 SnCl_2 | 1 | -1 SnCl_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 1 | -1 | ([Cl2])^(-1) SnCl_2 | 1 | -1 | ([SnCl2])^(-1) SnCl_4 | 1 | 1 | [SnCl4] 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 = ([Cl2])^(-1) ([SnCl2])^(-1) [SnCl4] = ([SnCl4])/([Cl2] [SnCl2])

Construct the rate of reaction expression for: Cl_2 + SnCl_2 ⟶ SnCl_4 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: Cl_2 + SnCl_2 ⟶ SnCl_4 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 Cl_2 | 1 | -1 SnCl_2 | 1 | -1 SnCl_4 | 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 Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) SnCl_2 | 1 | -1 | -(Δ[SnCl2])/(Δt) SnCl_4 | 1 | 1 | (Δ[SnCl4])/(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[Cl2])/(Δt) = -(Δ[SnCl2])/(Δt) = (Δ[SnCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| chlorine | stannous chloride | stannic chloride formula | Cl_2 | SnCl_2 | SnCl_4 Hill formula | Cl_2 | Cl_2Sn | Cl_4Sn name | chlorine | stannous chloride | stannic chloride IUPAC name | molecular chlorine | dichlorotin | tetrachlorostannane

| chlorine | stannous chloride | stannic chloride molar mass | 70.9 g/mol | 189.6 g/mol | 260.5 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) melting point | -101 °C | 246 °C | -33 °C boiling point | -34 °C | 652 °C | 114 °C density | 0.003214 g/cm^3 (at 0 °C) | 3.354 g/cm^3 | 2.226 g/cm^3 solubility in water | | | soluble dynamic viscosity | | 7 Pa s (at 25 °C) | 5.8×10^-4 Pa s (at 60 °C) odor | | odorless |