HClO3 = H2O + HClO4 + Cl2O

HClO3 ⟶ H_2O water + HClO_4 perchloric acid + Cl_2O chlorine monoxide

Balance the chemical equation algebraically: HClO3 ⟶ H_2O + HClO_4 + Cl_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HClO3 ⟶ c_2 H_2O + c_3 HClO_4 + c_4 Cl_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, Cl and O: H: | c_1 = 2 c_2 + c_3 Cl: | c_1 = c_3 + 2 c_4 O: | 3 c_1 = c_2 + 4 c_3 + c_4 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 = 6 c_2 = 1 c_3 = 4 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HClO3 ⟶ H_2O + 4 HClO_4 + Cl_2O

HClO3 ⟶ + +

HClO3 ⟶ water + perchloric acid + chlorine monoxide

Construct the equilibrium constant, K, expression for: HClO3 ⟶ H_2O + HClO_4 + Cl_2O 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: 6 HClO3 ⟶ H_2O + 4 HClO_4 + Cl_2O 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 HClO3 | 6 | -6 H_2O | 1 | 1 HClO_4 | 4 | 4 Cl_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HClO3 | 6 | -6 | ([HClO3])^(-6) H_2O | 1 | 1 | [H2O] HClO_4 | 4 | 4 | ([HClO4])^4 Cl_2O | 1 | 1 | [Cl2O] 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 = ([HClO3])^(-6) [H2O] ([HClO4])^4 [Cl2O] = ([H2O] ([HClO4])^4 [Cl2O])/([HClO3])^6

Construct the rate of reaction expression for: HClO3 ⟶ H_2O + HClO_4 + Cl_2O 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: 6 HClO3 ⟶ H_2O + 4 HClO_4 + Cl_2O 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 HClO3 | 6 | -6 H_2O | 1 | 1 HClO_4 | 4 | 4 Cl_2O | 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 HClO3 | 6 | -6 | -1/6 (Δ[HClO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) HClO_4 | 4 | 4 | 1/4 (Δ[HClO4])/(Δt) Cl_2O | 1 | 1 | (Δ[Cl2O])/(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 = -1/6 (Δ[HClO3])/(Δt) = (Δ[H2O])/(Δt) = 1/4 (Δ[HClO4])/(Δt) = (Δ[Cl2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| HClO3 | water | perchloric acid | chlorine monoxide formula | HClO3 | H_2O | HClO_4 | Cl_2O Hill formula | HClO3 | H_2O | ClHO_4 | Cl_2O name | | water | perchloric acid | chlorine monoxide IUPAC name | | water | perchloric acid | chloro hypochlorite

| HClO3 | water | perchloric acid | chlorine monoxide molar mass | 84.45 g/mol | 18.015 g/mol | 100.5 g/mol | 86.9 g/mol phase | | liquid (at STP) | liquid (at STP) | gas (at STP) melting point | | 0 °C | -112 °C | -120.6 °C boiling point | | 99.9839 °C | 90 °C | 2.2 °C density | | 1 g/cm^3 | 1.77 g/cm^3 | 0.003552 g/cm^3 (at 20 °C) solubility in water | | | very soluble | slightly soluble surface tension | | 0.0728 N/m | | dynamic viscosity | | 8.9×10^-4 Pa s (at 25 °C) | 8×10^-4 Pa s (at 25 °C) | odor | | odorless | odorless |