CuCl2 + K2S = KCl + CuS

CuCl_2 copper(II) chloride + K2S ⟶ KCl potassium chloride + CuS cupric sulfide

Balance the chemical equation algebraically: CuCl_2 + K2S ⟶ KCl + CuS Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CuCl_2 + c_2 K2S ⟶ c_3 KCl + c_4 CuS Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Cu, K and S: Cl: | 2 c_1 = c_3 Cu: | c_1 = c_4 K: | 2 c_2 = c_3 S: | 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 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CuCl_2 + K2S ⟶ 2 KCl + CuS

+ K2S ⟶ +

copper(II) chloride + K2S ⟶ potassium chloride + cupric sulfide

Construct the equilibrium constant, K, expression for: CuCl_2 + K2S ⟶ KCl + CuS 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 + K2S ⟶ 2 KCl + CuS 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 K2S | 1 | -1 KCl | 2 | 2 CuS | 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) K2S | 1 | -1 | ([K2S])^(-1) KCl | 2 | 2 | ([KCl])^2 CuS | 1 | 1 | [CuS] 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) ([K2S])^(-1) ([KCl])^2 [CuS] = (([KCl])^2 [CuS])/([CuCl2] [K2S])

Construct the rate of reaction expression for: CuCl_2 + K2S ⟶ KCl + CuS 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 + K2S ⟶ 2 KCl + CuS 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 K2S | 1 | -1 KCl | 2 | 2 CuS | 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) K2S | 1 | -1 | -(Δ[K2S])/(Δt) KCl | 2 | 2 | 1/2 (Δ[KCl])/(Δt) CuS | 1 | 1 | (Δ[CuS])/(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[K2S])/(Δt) = 1/2 (Δ[KCl])/(Δt) = (Δ[CuS])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| copper(II) chloride | K2S | potassium chloride | cupric sulfide formula | CuCl_2 | K2S | KCl | CuS Hill formula | Cl_2Cu | K2S | ClK | CuS name | copper(II) chloride | | potassium chloride | cupric sulfide IUPAC name | dichlorocopper | | potassium chloride |

| copper(II) chloride | K2S | potassium chloride | cupric sulfide molar mass | 134.4 g/mol | 110.26 g/mol | 74.55 g/mol | 95.61 g/mol phase | solid (at STP) | | solid (at STP) | solid (at STP) melting point | 620 °C | | 770 °C | 220 °C boiling point | | | 1420 °C | density | 3.386 g/cm^3 | | 1.98 g/cm^3 | 4.6 g/cm^3 solubility in water | | | soluble | dynamic viscosity | | | | 3.68×10^-5 Pa s (at 1250 °C) odor | | | odorless |