KMnO4 = K2MnO4MnO2O2

KMnO_4 potassium permanganate ⟶ K2MnO4MnO2O2

Balance the chemical equation algebraically: KMnO_4 ⟶ K2MnO4MnO2O2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KMnO_4 ⟶ c_2 K2MnO4MnO2O2 Set the number of atoms in the reactants equal to the number of atoms in the products for K, Mn and O: K: | c_1 = 2 c_2 Mn: | c_1 = 2 c_2 O: | 4 c_1 = 8 c_2 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KMnO_4 ⟶ K2MnO4MnO2O2

⟶ K2MnO4MnO2O2

potassium permanganate ⟶ K2MnO4MnO2O2

Construct the equilibrium constant, K, expression for: KMnO_4 ⟶ K2MnO4MnO2O2 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 KMnO_4 ⟶ K2MnO4MnO2O2 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 KMnO_4 | 2 | -2 K2MnO4MnO2O2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KMnO_4 | 2 | -2 | ([KMnO4])^(-2) K2MnO4MnO2O2 | 1 | 1 | [K2MnO4MnO2O2] 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 = ([KMnO4])^(-2) [K2MnO4MnO2O2] = ([K2MnO4MnO2O2])/([KMnO4])^2

Construct the rate of reaction expression for: KMnO_4 ⟶ K2MnO4MnO2O2 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 KMnO_4 ⟶ K2MnO4MnO2O2 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 KMnO_4 | 2 | -2 K2MnO4MnO2O2 | 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 KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) K2MnO4MnO2O2 | 1 | 1 | (Δ[K2MnO4MnO2O2])/(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[KMnO4])/(Δt) = (Δ[K2MnO4MnO2O2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium permanganate | K2MnO4MnO2O2 formula | KMnO_4 | K2MnO4MnO2O2 Hill formula | KMnO_4 | K2Mn2O8 name | potassium permanganate |

| potassium permanganate | K2MnO4MnO2O2 molar mass | 158.03 g/mol | 316.06 g/mol phase | solid (at STP) | melting point | 240 °C | density | 1 g/cm^3 | odor | odorless |