Cl2 + H2 = H2Cl2

chlorine + hydrogen ⟶ H2Cl2

Balance the chemical equation algebraically: + ⟶ H2Cl2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 + c_2 ⟶ c_3 H2Cl2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl and H: Cl: | 2 c_1 = 2 c_3 H: | 2 c_2 = 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | + ⟶ H2Cl2

+ ⟶ H2Cl2

chlorine + hydrogen ⟶ H2Cl2

| chlorine | hydrogen | H2Cl2 formula | | | H2Cl2 Hill formula | Cl_2 | H_2 | H2Cl2 name | chlorine | hydrogen | IUPAC name | molecular chlorine | molecular hydrogen |

| chlorine | hydrogen | H2Cl2 molar mass | 70.9 g/mol | 2.016 g/mol | 72.92 g/mol phase | gas (at STP) | gas (at STP) | melting point | -101 °C | -259.2 °C | boiling point | -34 °C | -252.8 °C | density | 0.003214 g/cm^3 (at 0 °C) | 8.99×10^-5 g/cm^3 (at 0 °C) | dynamic viscosity | | 8.9×10^-6 Pa s (at 25 °C) | odor | | odorless |