CuCl2 + Pb = Cu + PbCl

CuCl_2 copper(II) chloride + Pb lead ⟶ Cu copper + PbCl

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

+ ⟶ + PbCl

copper(II) chloride + lead ⟶ copper + PbCl

Construct the equilibrium constant, K, expression for: CuCl_2 + Pb ⟶ Cu + PbCl 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 + 2 Pb ⟶ Cu + 2 PbCl 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 Pb | 2 | -2 Cu | 1 | 1 PbCl | 2 | 2 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) Pb | 2 | -2 | ([Pb])^(-2) Cu | 1 | 1 | [Cu] PbCl | 2 | 2 | ([PbCl])^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 = ([CuCl2])^(-1) ([Pb])^(-2) [Cu] ([PbCl])^2 = ([Cu] ([PbCl])^2)/([CuCl2] ([Pb])^2)

Construct the rate of reaction expression for: CuCl_2 + Pb ⟶ Cu + PbCl 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 + 2 Pb ⟶ Cu + 2 PbCl 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 Pb | 2 | -2 Cu | 1 | 1 PbCl | 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 CuCl_2 | 1 | -1 | -(Δ[CuCl2])/(Δt) Pb | 2 | -2 | -1/2 (Δ[Pb])/(Δt) Cu | 1 | 1 | (Δ[Cu])/(Δt) PbCl | 2 | 2 | 1/2 (Δ[PbCl])/(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) = -1/2 (Δ[Pb])/(Δt) = (Δ[Cu])/(Δt) = 1/2 (Δ[PbCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| copper(II) chloride | lead | copper | PbCl formula | CuCl_2 | Pb | Cu | PbCl Hill formula | Cl_2Cu | Pb | Cu | ClPb name | copper(II) chloride | lead | copper | IUPAC name | dichlorocopper | lead | copper |

| copper(II) chloride | lead | copper | PbCl molar mass | 134.4 g/mol | 207.2 g/mol | 63.546 g/mol | 242.7 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 620 °C | 327.4 °C | 1083 °C | boiling point | | 1740 °C | 2567 °C | density | 3.386 g/cm^3 | 11.34 g/cm^3 | 8.96 g/cm^3 | solubility in water | | insoluble | insoluble | dynamic viscosity | | 0.00183 Pa s (at 38 °C) | | odor | | | odorless |