KClO3 = KClO + O3

KClO_3 potassium chlorate ⟶ KClO + O_3 ozone

Balance the chemical equation algebraically: KClO_3 ⟶ KClO + O_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KClO_3 ⟶ c_2 KClO + c_3 O_3 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_2 K: | c_1 = c_2 O: | 3 c_1 = c_2 + 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3/2 c_2 = 3/2 c_3 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 3 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 KClO_3 ⟶ 3 KClO + 2 O_3

⟶ KClO +

potassium chlorate ⟶ KClO + ozone

Construct the equilibrium constant, K, expression for: KClO_3 ⟶ KClO + O_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 KClO_3 ⟶ 3 KClO + 2 O_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 KClO_3 | 3 | -3 KClO | 3 | 3 O_3 | 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 | 3 | -3 | ([KClO3])^(-3) KClO | 3 | 3 | ([KClO])^3 O_3 | 2 | 2 | ([O3])^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])^(-3) ([KClO])^3 ([O3])^2 = (([KClO])^3 ([O3])^2)/([KClO3])^3

Construct the rate of reaction expression for: KClO_3 ⟶ KClO + O_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 KClO_3 ⟶ 3 KClO + 2 O_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 KClO_3 | 3 | -3 KClO | 3 | 3 O_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 KClO_3 | 3 | -3 | -1/3 (Δ[KClO3])/(Δt) KClO | 3 | 3 | 1/3 (Δ[KClO])/(Δt) O_3 | 2 | 2 | 1/2 (Δ[O3])/(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[KClO3])/(Δt) = 1/3 (Δ[KClO])/(Δt) = 1/2 (Δ[O3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium chlorate | KClO | ozone formula | KClO_3 | KClO | O_3 Hill formula | ClKO_3 | ClKO | O_3 name | potassium chlorate | | ozone

| potassium chlorate | KClO | ozone molar mass | 122.5 g/mol | 90.55 g/mol | 47.997 g/mol phase | solid (at STP) | | gas (at STP) melting point | 356 °C | | -192.2 °C boiling point | | | -111.9 °C density | 2.34 g/cm^3 | | 0.001962 g/cm^3 (at 25 °C) solubility in water | soluble | |