KClO2 = KCl + KClO3

KClO2 ⟶ KCl potassium chloride + KClO_3 potassium chlorate

Balance the chemical equation algebraically: KClO2 ⟶ KCl + KClO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KClO2 ⟶ c_2 KCl + c_3 KClO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for K, Cl and O: K: | c_1 = c_2 + c_3 Cl: | c_1 = c_2 + c_3 O: | 2 c_1 = 3 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 KClO2 ⟶ KCl + 2 KClO_3

KClO2 ⟶ +

KClO2 ⟶ potassium chloride + potassium chlorate

Construct the equilibrium constant, K, expression for: KClO2 ⟶ KCl + KClO_3 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: 3 KClO2 ⟶ KCl + 2 KClO_3 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 KClO2 | 3 | -3 KCl | 1 | 1 KClO_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KClO2 | 3 | -3 | ([KClO2])^(-3) KCl | 1 | 1 | [KCl] KClO_3 | 2 | 2 | ([KClO3])^2 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 = ([KClO2])^(-3) [KCl] ([KClO3])^2 = ([KCl] ([KClO3])^2)/([KClO2])^3

Construct the rate of reaction expression for: KClO2 ⟶ KCl + KClO_3 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: 3 KClO2 ⟶ KCl + 2 KClO_3 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 KClO2 | 3 | -3 KCl | 1 | 1 KClO_3 | 2 | 2 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 KClO2 | 3 | -3 | -1/3 (Δ[KClO2])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(Δt) KClO_3 | 2 | 2 | 1/2 (Δ[KClO3])/(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 = -1/3 (Δ[KClO2])/(Δt) = (Δ[KCl])/(Δt) = 1/2 (Δ[KClO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| KClO2 | potassium chloride | potassium chlorate formula | KClO2 | KCl | KClO_3 Hill formula | ClKO2 | ClK | ClKO_3 name | | potassium chloride | potassium chlorate

| KClO2 | potassium chloride | potassium chlorate molar mass | 106.5 g/mol | 74.55 g/mol | 122.5 g/mol phase | | solid (at STP) | solid (at STP) melting point | | 770 °C | 356 °C boiling point | | 1420 °C | density | | 1.98 g/cm^3 | 2.34 g/cm^3 solubility in water | | soluble | soluble odor | | odorless |