KClO3 = O2 + KClO2

KClO_3 potassium chlorate ⟶ O_2 oxygen + KClO2

Balance the chemical equation algebraically: KClO_3 ⟶ O_2 + KClO2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KClO_3 ⟶ c_2 O_2 + c_3 KClO2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, K and O: Cl: | c_1 = c_3 K: | c_1 = c_3 O: | 3 c_1 = 2 c_2 + 2 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 = 2 c_2 = 1 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KClO_3 ⟶ O_2 + 2 KClO2

⟶ + KClO2

potassium chlorate ⟶ oxygen + KClO2

Construct the equilibrium constant, K, expression for: KClO_3 ⟶ O_2 + KClO2 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 KClO_3 ⟶ O_2 + 2 KClO2 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 KClO_3 | 2 | -2 O_2 | 1 | 1 KClO2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KClO_3 | 2 | -2 | ([KClO3])^(-2) O_2 | 1 | 1 | [O2] KClO2 | 2 | 2 | ([KClO2])^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 = ([KClO3])^(-2) [O2] ([KClO2])^2 = ([O2] ([KClO2])^2)/([KClO3])^2

Construct the rate of reaction expression for: KClO_3 ⟶ O_2 + KClO2 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 KClO_3 ⟶ O_2 + 2 KClO2 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 KClO_3 | 2 | -2 O_2 | 1 | 1 KClO2 | 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 KClO_3 | 2 | -2 | -1/2 (Δ[KClO3])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) KClO2 | 2 | 2 | 1/2 (Δ[KClO2])/(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[KClO3])/(Δt) = (Δ[O2])/(Δt) = 1/2 (Δ[KClO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium chlorate | oxygen | KClO2 formula | KClO_3 | O_2 | KClO2 Hill formula | ClKO_3 | O_2 | ClKO2 name | potassium chlorate | oxygen | IUPAC name | potassium chlorate | molecular oxygen |

| potassium chlorate | oxygen | KClO2 molar mass | 122.5 g/mol | 31.998 g/mol | 106.5 g/mol phase | solid (at STP) | gas (at STP) | melting point | 356 °C | -218 °C | boiling point | | -183 °C | density | 2.34 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | solubility in water | soluble | | surface tension | | 0.01347 N/m | dynamic viscosity | | 2.055×10^-5 Pa s (at 25 °C) | odor | | odorless |