H2 + CuCl2 = HCl + Cu

H_2 hydrogen + CuCl_2 copper(II) chloride ⟶ HCl hydrogen chloride + Cu copper

Balance the chemical equation algebraically: H_2 + CuCl_2 ⟶ HCl + Cu Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2 + c_2 CuCl_2 ⟶ c_3 HCl + c_4 Cu Set the number of atoms in the reactants equal to the number of atoms in the products for H, Cl and Cu: H: | 2 c_1 = c_3 Cl: | 2 c_2 = c_3 Cu: | 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: | | H_2 + CuCl_2 ⟶ 2 HCl + Cu

+ ⟶ +

hydrogen + copper(II) chloride ⟶ hydrogen chloride + copper

| hydrogen | copper(II) chloride | hydrogen chloride | copper molecular enthalpy | 0 kJ/mol | -220.1 kJ/mol | -92.3 kJ/mol | 0 kJ/mol total enthalpy | 0 kJ/mol | -220.1 kJ/mol | -184.6 kJ/mol | 0 kJ/mol | H_initial = -220.1 kJ/mol | | H_final = -184.6 kJ/mol | ΔH_rxn^0 | -184.6 kJ/mol - -220.1 kJ/mol = 35.5 kJ/mol (endothermic) | | |

Construct the equilibrium constant, K, expression for: H_2 + CuCl_2 ⟶ HCl + Cu 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: H_2 + CuCl_2 ⟶ 2 HCl + Cu 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 H_2 | 1 | -1 CuCl_2 | 1 | -1 HCl | 2 | 2 Cu | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2 | 1 | -1 | ([H2])^(-1) CuCl_2 | 1 | -1 | ([CuCl2])^(-1) HCl | 2 | 2 | ([HCl])^2 Cu | 1 | 1 | [Cu] 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 = ([H2])^(-1) ([CuCl2])^(-1) ([HCl])^2 [Cu] = (([HCl])^2 [Cu])/([H2] [CuCl2])

Construct the rate of reaction expression for: H_2 + CuCl_2 ⟶ HCl + Cu 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: H_2 + CuCl_2 ⟶ 2 HCl + Cu 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 H_2 | 1 | -1 CuCl_2 | 1 | -1 HCl | 2 | 2 Cu | 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 H_2 | 1 | -1 | -(Δ[H2])/(Δt) CuCl_2 | 1 | -1 | -(Δ[CuCl2])/(Δt) HCl | 2 | 2 | 1/2 (Δ[HCl])/(Δt) Cu | 1 | 1 | (Δ[Cu])/(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[H2])/(Δt) = -(Δ[CuCl2])/(Δt) = 1/2 (Δ[HCl])/(Δt) = (Δ[Cu])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen | copper(II) chloride | hydrogen chloride | copper formula | H_2 | CuCl_2 | HCl | Cu Hill formula | H_2 | Cl_2Cu | ClH | Cu name | hydrogen | copper(II) chloride | hydrogen chloride | copper IUPAC name | molecular hydrogen | dichlorocopper | hydrogen chloride | copper

| hydrogen | copper(II) chloride | hydrogen chloride | copper molar mass | 2.016 g/mol | 134.4 g/mol | 36.46 g/mol | 63.546 g/mol phase | gas (at STP) | solid (at STP) | gas (at STP) | solid (at STP) melting point | -259.2 °C | 620 °C | -114.17 °C | 1083 °C boiling point | -252.8 °C | | -85 °C | 2567 °C density | 8.99×10^-5 g/cm^3 (at 0 °C) | 3.386 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 8.96 g/cm^3 solubility in water | | | miscible | insoluble dynamic viscosity | 8.9×10^-6 Pa s (at 25 °C) | | | odor | odorless | | | odorless