KOH + H2O2 = H2O + K2O2

KOH potassium hydroxide + H_2O_2 hydrogen peroxide ⟶ H_2O water + K_2O_2 potassium peroxide

Balance the chemical equation algebraically: KOH + H_2O_2 ⟶ H_2O + K_2O_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 H_2O_2 ⟶ c_3 H_2O + c_4 K_2O_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K and O: H: | c_1 + 2 c_2 = 2 c_3 K: | c_1 = 2 c_4 O: | c_1 + 2 c_2 = c_3 + 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + H_2O_2 ⟶ 2 H_2O + K_2O_2

+ ⟶ +

potassium hydroxide + hydrogen peroxide ⟶ water + potassium peroxide

| potassium hydroxide | hydrogen peroxide | water | potassium peroxide molecular free energy | -379.4 kJ/mol | -120.4 kJ/mol | -237.1 kJ/mol | -425.1 kJ/mol total free energy | -758.8 kJ/mol | -120.4 kJ/mol | -474.2 kJ/mol | -425.1 kJ/mol | G_initial = -879.2 kJ/mol | | G_final = -899.3 kJ/mol | ΔG_rxn^0 | -899.3 kJ/mol - -879.2 kJ/mol = -20.1 kJ/mol (exergonic) | | |

Construct the equilibrium constant, K, expression for: KOH + H_2O_2 ⟶ H_2O + K_2O_2 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: 2 KOH + H_2O_2 ⟶ 2 H_2O + K_2O_2 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 KOH | 2 | -2 H_2O_2 | 1 | -1 H_2O | 2 | 2 K_2O_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 2 | -2 | ([KOH])^(-2) H_2O_2 | 1 | -1 | ([H2O2])^(-1) H_2O | 2 | 2 | ([H2O])^2 K_2O_2 | 1 | 1 | [K2O2] 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 = ([KOH])^(-2) ([H2O2])^(-1) ([H2O])^2 [K2O2] = (([H2O])^2 [K2O2])/(([KOH])^2 [H2O2])

Construct the rate of reaction expression for: KOH + H_2O_2 ⟶ H_2O + K_2O_2 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: 2 KOH + H_2O_2 ⟶ 2 H_2O + K_2O_2 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 KOH | 2 | -2 H_2O_2 | 1 | -1 H_2O | 2 | 2 K_2O_2 | 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 KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) K_2O_2 | 1 | 1 | (Δ[K2O2])/(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 = -1/2 (Δ[KOH])/(Δt) = -(Δ[H2O2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[K2O2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium hydroxide | hydrogen peroxide | water | potassium peroxide formula | KOH | H_2O_2 | H_2O | K_2O_2 Hill formula | HKO | H_2O_2 | H_2O | K_2O_2 name | potassium hydroxide | hydrogen peroxide | water | potassium peroxide IUPAC name | potassium hydroxide | hydrogen peroxide | water | dipotassium peroxide

| potassium hydroxide | hydrogen peroxide | water | potassium peroxide molar mass | 56.105 g/mol | 34.014 g/mol | 18.015 g/mol | 110.19 g/mol phase | solid (at STP) | liquid (at STP) | liquid (at STP) | solid (at STP) melting point | 406 °C | -0.43 °C | 0 °C | 490 °C boiling point | 1327 °C | 150.2 °C | 99.9839 °C | density | 2.044 g/cm^3 | 1.44 g/cm^3 | 1 g/cm^3 | 1 g/cm^3 solubility in water | soluble | miscible | | reacts surface tension | | 0.0804 N/m | 0.0728 N/m | dynamic viscosity | 0.001 Pa s (at 550 °C) | 0.001249 Pa s (at 20 °C) | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless |