KClO2 = O2 + KCl

KClO2 ⟶ O_2 oxygen + KCl potassium chloride

Balance the chemical equation algebraically: KClO2 ⟶ O_2 + KCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KClO2 ⟶ c_2 O_2 + c_3 KCl 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_3 Cl: | c_1 = c_3 O: | 2 c_1 = 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | KClO2 ⟶ O_2 + KCl

KClO2 ⟶ +

KClO2 ⟶ oxygen + potassium chloride

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

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

| KClO2 | oxygen | potassium chloride formula | KClO2 | O_2 | KCl Hill formula | ClKO2 | O_2 | ClK name | | oxygen | potassium chloride IUPAC name | | molecular oxygen | potassium chloride

| KClO2 | oxygen | potassium chloride molar mass | 106.5 g/mol | 31.998 g/mol | 74.55 g/mol phase | | gas (at STP) | solid (at STP) melting point | | -218 °C | 770 °C boiling point | | -183 °C | 1420 °C density | | 0.001429 g/cm^3 (at 0 °C) | 1.98 g/cm^3 solubility in water | | | soluble surface tension | | 0.01347 N/m | dynamic viscosity | | 2.055×10^-5 Pa s (at 25 °C) | odor | | odorless | odorless