SnCl2 + BiCl = SnCl4 + Bi

SnCl_2 stannous chloride + BiCl ⟶ SnCl_4 stannic chloride + Bi bismuth

Balance the chemical equation algebraically: SnCl_2 + BiCl ⟶ SnCl_4 + Bi Add stoichiometric coefficients, c_i, to the reactants and products: c_1 SnCl_2 + c_2 BiCl ⟶ c_3 SnCl_4 + c_4 Bi Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Sn and Bi: Cl: | 2 c_1 + c_2 = 4 c_3 Sn: | c_1 = c_3 Bi: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | SnCl_2 + 2 BiCl ⟶ SnCl_4 + 2 Bi

+ BiCl ⟶ +

stannous chloride + BiCl ⟶ stannic chloride + bismuth

Construct the equilibrium constant, K, expression for: SnCl_2 + BiCl ⟶ SnCl_4 + Bi 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: SnCl_2 + 2 BiCl ⟶ SnCl_4 + 2 Bi 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 SnCl_2 | 1 | -1 BiCl | 2 | -2 SnCl_4 | 1 | 1 Bi | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression SnCl_2 | 1 | -1 | ([SnCl2])^(-1) BiCl | 2 | -2 | ([BiCl])^(-2) SnCl_4 | 1 | 1 | [SnCl4] Bi | 2 | 2 | ([Bi])^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 = ([SnCl2])^(-1) ([BiCl])^(-2) [SnCl4] ([Bi])^2 = ([SnCl4] ([Bi])^2)/([SnCl2] ([BiCl])^2)

Construct the rate of reaction expression for: SnCl_2 + BiCl ⟶ SnCl_4 + Bi 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: SnCl_2 + 2 BiCl ⟶ SnCl_4 + 2 Bi 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 SnCl_2 | 1 | -1 BiCl | 2 | -2 SnCl_4 | 1 | 1 Bi | 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 SnCl_2 | 1 | -1 | -(Δ[SnCl2])/(Δt) BiCl | 2 | -2 | -1/2 (Δ[BiCl])/(Δt) SnCl_4 | 1 | 1 | (Δ[SnCl4])/(Δt) Bi | 2 | 2 | 1/2 (Δ[Bi])/(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[SnCl2])/(Δt) = -1/2 (Δ[BiCl])/(Δt) = (Δ[SnCl4])/(Δt) = 1/2 (Δ[Bi])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| stannous chloride | BiCl | stannic chloride | bismuth formula | SnCl_2 | BiCl | SnCl_4 | Bi Hill formula | Cl_2Sn | BiCl | Cl_4Sn | Bi name | stannous chloride | | stannic chloride | bismuth IUPAC name | dichlorotin | | tetrachlorostannane | bismuth

| stannous chloride | BiCl | stannic chloride | bismuth molar mass | 189.6 g/mol | 244.43 g/mol | 260.5 g/mol | 208.9804 g/mol phase | solid (at STP) | | liquid (at STP) | solid (at STP) melting point | 246 °C | | -33 °C | 271 °C boiling point | 652 °C | | 114 °C | 1560 °C density | 3.354 g/cm^3 | | 2.226 g/cm^3 | 9.8 g/cm^3 solubility in water | | | soluble | insoluble dynamic viscosity | 7 Pa s (at 25 °C) | | 5.8×10^-4 Pa s (at 60 °C) | 1.19×10^-4 Pa s (at 500 °C) odor | odorless | | |