CuCl2 + Sn = Cu + SnCl2

CuCl_2 copper(II) chloride + Sn white tin ⟶ Cu copper + SnCl_2 stannous chloride

Balance the chemical equation algebraically: CuCl_2 + Sn ⟶ Cu + SnCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CuCl_2 + c_2 Sn ⟶ c_3 Cu + c_4 SnCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Cu and Sn: Cl: | 2 c_1 = 2 c_4 Cu: | c_1 = c_3 Sn: | 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 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CuCl_2 + Sn ⟶ Cu + SnCl_2

+ ⟶ +

copper(II) chloride + white tin ⟶ copper + stannous chloride

Construct the equilibrium constant, K, expression for: CuCl_2 + Sn ⟶ Cu + SnCl_2 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: CuCl_2 + Sn ⟶ Cu + SnCl_2 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 CuCl_2 | 1 | -1 Sn | 1 | -1 Cu | 1 | 1 SnCl_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CuCl_2 | 1 | -1 | ([CuCl2])^(-1) Sn | 1 | -1 | ([Sn])^(-1) Cu | 1 | 1 | [Cu] SnCl_2 | 1 | 1 | [SnCl2] 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 = ([CuCl2])^(-1) ([Sn])^(-1) [Cu] [SnCl2] = ([Cu] [SnCl2])/([CuCl2] [Sn])

Construct the rate of reaction expression for: CuCl_2 + Sn ⟶ Cu + SnCl_2 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: CuCl_2 + Sn ⟶ Cu + SnCl_2 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 CuCl_2 | 1 | -1 Sn | 1 | -1 Cu | 1 | 1 SnCl_2 | 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 CuCl_2 | 1 | -1 | -(Δ[CuCl2])/(Δt) Sn | 1 | -1 | -(Δ[Sn])/(Δt) Cu | 1 | 1 | (Δ[Cu])/(Δt) SnCl_2 | 1 | 1 | (Δ[SnCl2])/(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[CuCl2])/(Δt) = -(Δ[Sn])/(Δt) = (Δ[Cu])/(Δt) = (Δ[SnCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| copper(II) chloride | white tin | copper | stannous chloride formula | CuCl_2 | Sn | Cu | SnCl_2 Hill formula | Cl_2Cu | Sn | Cu | Cl_2Sn name | copper(II) chloride | white tin | copper | stannous chloride IUPAC name | dichlorocopper | tin | copper | dichlorotin

| copper(II) chloride | white tin | copper | stannous chloride molar mass | 134.4 g/mol | 118.71 g/mol | 63.546 g/mol | 189.6 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 620 °C | 231.9 °C | 1083 °C | 246 °C boiling point | | 2602 °C | 2567 °C | 652 °C density | 3.386 g/cm^3 | 7.31 g/cm^3 | 8.96 g/cm^3 | 3.354 g/cm^3 solubility in water | | insoluble | insoluble | dynamic viscosity | | 0.001 Pa s (at 600 °C) | | 7 Pa s (at 25 °C) odor | | odorless | odorless | odorless