CuCl2 = Cl2 + CuCl

copper(II) chloride ⟶ chlorine + cuprous chloride

Balance the chemical equation algebraically: ⟶ + Add stoichiometric coefficients, c_i, to the reactants and products: c_1 ⟶ c_2 + c_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl and Cu: Cl: | 2 c_1 = 2 c_2 + c_3 Cu: | c_1 = c_3 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 ⟶ + 2

⟶ +

copper(II) chloride ⟶ chlorine + cuprous chloride

| copper(II) chloride | chlorine | cuprous chloride molecular enthalpy | -220.1 kJ/mol | 0 kJ/mol | -137.2 kJ/mol total enthalpy | -440.2 kJ/mol | 0 kJ/mol | -274.4 kJ/mol | H_initial = -440.2 kJ/mol | H_final = -274.4 kJ/mol | ΔH_rxn^0 | -274.4 kJ/mol - -440.2 kJ/mol = 165.8 kJ/mol (endothermic) | |

| copper(II) chloride | chlorine | cuprous chloride molecular free energy | -175.7 kJ/mol | 0 kJ/mol | -119.9 kJ/mol total free energy | -351.4 kJ/mol | 0 kJ/mol | -239.8 kJ/mol | G_initial = -351.4 kJ/mol | G_final = -239.8 kJ/mol | ΔG_rxn^0 | -239.8 kJ/mol - -351.4 kJ/mol = 111.6 kJ/mol (endergonic) | |

| copper(II) chloride | chlorine | cuprous chloride Hill formula | Cl_2Cu | Cl_2 | ClCu name | copper(II) chloride | chlorine | cuprous chloride IUPAC name | dichlorocopper | molecular chlorine |

| copper(II) chloride | chlorine | cuprous chloride molar mass | 134.4 g/mol | 70.9 g/mol | 99 g/mol phase | solid (at STP) | gas (at STP) | solid (at STP) melting point | 620 °C | -101 °C | 430 °C boiling point | | -34 °C | 1490 °C density | 3.386 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | 4.145 g/cm^3