Cu + SnCl2 = CuCl2 + Sn

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

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

+ ⟶ +

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

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

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

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

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