Input interpretation
water + potassium superoxide ⟶ oxygen + potassium hydroxide + hydrogen peroxide
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 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and K: H: | 2 c_1 = c_4 + 2 c_5 O: | c_1 + 2 c_2 = 2 c_3 + c_4 + 2 c_5 K: | 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_3 = 1 and solve the system of equations for the remaining coefficients: c_2 = c_1/2 + 1 c_3 = 1 c_4 = c_1/2 + 1 c_5 = (3 c_1)/4 - 1/2 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 2 and solve for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 + 2 ⟶ + 2 +
Structures
+ ⟶ + +
Names
water + potassium superoxide ⟶ oxygen + potassium hydroxide + hydrogen peroxide
Reaction thermodynamics
Gibbs free energy
| water | potassium superoxide | oxygen | potassium hydroxide | hydrogen peroxide molecular free energy | -237.1 kJ/mol | -239.4 kJ/mol | 231.7 kJ/mol | -379.4 kJ/mol | -120.4 kJ/mol total free energy | -474.2 kJ/mol | -478.8 kJ/mol | 231.7 kJ/mol | -758.8 kJ/mol | -120.4 kJ/mol | G_initial = -953 kJ/mol | | G_final = -647.5 kJ/mol | | ΔG_rxn^0 | -647.5 kJ/mol - -953 kJ/mol = 305.5 kJ/mol (endergonic) | | | |
Chemical names and formulas
| water | potassium superoxide | oxygen | potassium hydroxide | hydrogen peroxide Hill formula | H_2O | KO_2 | O_2 | HKO | H_2O_2 name | water | potassium superoxide | oxygen | potassium hydroxide | hydrogen peroxide IUPAC name | water | potassium molecular oxygen | molecular oxygen | potassium hydroxide | hydrogen peroxide