Input interpretation
hydrogen chloride + sodium iodide + sodium iodate ⟶ water + iodine + sodium chloride
Balanced equation
Balance the chemical equation algebraically: + + ⟶ + + Add stoichiometric coefficients, c_i, to the reactants and products: c_1 + c_2 + c_3 ⟶ c_4 + c_5 + c_6 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, I, Na and O: Cl: | c_1 = c_6 H: | c_1 = 2 c_4 I: | c_2 + c_3 = 2 c_5 Na: | c_2 + c_3 = c_6 O: | 3 c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 5 c_3 = 1 c_4 = 3 c_5 = 3 c_6 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 + 5 + ⟶ 3 + 3 + 6
Structures
+ + ⟶ + +
Names
hydrogen chloride + sodium iodide + sodium iodate ⟶ water + iodine + sodium chloride
Reaction thermodynamics
Enthalpy
| hydrogen chloride | sodium iodide | sodium iodate | water | iodine | sodium chloride molecular enthalpy | -92.3 kJ/mol | -287.8 kJ/mol | -481.8 kJ/mol | -285.8 kJ/mol | 0 kJ/mol | -411.2 kJ/mol total enthalpy | -553.8 kJ/mol | -1439 kJ/mol | -481.8 kJ/mol | -857.5 kJ/mol | 0 kJ/mol | -2467 kJ/mol | H_initial = -2475 kJ/mol | | | H_final = -3325 kJ/mol | | ΔH_rxn^0 | -3325 kJ/mol - -2475 kJ/mol = -850.1 kJ/mol (exothermic) | | | | |
Chemical names and formulas
| hydrogen chloride | sodium iodide | sodium iodate | water | iodine | sodium chloride Hill formula | ClH | INa | INaO_3 | H_2O | I_2 | ClNa name | hydrogen chloride | sodium iodide | sodium iodate | water | iodine | sodium chloride IUPAC name | hydrogen chloride | sodium iodide | sodium iodate | water | molecular iodine | sodium chloride