ClO2NaOH = NaClO3NaClO2H2O

ClO2NaOH ⟶ NaClO3NaClO2H2O

Balance the chemical equation algebraically: ClO2NaOH ⟶ NaClO3NaClO2H2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 ClO2NaOH ⟶ c_2 NaClO3NaClO2H2O Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, O, Na and H: Cl: | c_1 = 2 c_2 O: | 3 c_1 = 6 c_2 Na: | c_1 = 2 c_2 H: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 ClO2NaOH ⟶ NaClO3NaClO2H2O

ClO2NaOH ⟶ NaClO3NaClO2H2O

ClO2NaOH ⟶ NaClO3NaClO2H2O

Construct the equilibrium constant, K, expression for: ClO2NaOH ⟶ NaClO3NaClO2H2O 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 ClO2NaOH ⟶ NaClO3NaClO2H2O 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 ClO2NaOH | 2 | -2 NaClO3NaClO2H2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression ClO2NaOH | 2 | -2 | ([ClO2NaOH])^(-2) NaClO3NaClO2H2O | 1 | 1 | [NaClO3NaClO2H2O] 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 = ([ClO2NaOH])^(-2) [NaClO3NaClO2H2O] = ([NaClO3NaClO2H2O])/([ClO2NaOH])^2

Construct the rate of reaction expression for: ClO2NaOH ⟶ NaClO3NaClO2H2O 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 ClO2NaOH ⟶ NaClO3NaClO2H2O 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 ClO2NaOH | 2 | -2 NaClO3NaClO2H2O | 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 ClO2NaOH | 2 | -2 | -1/2 (Δ[ClO2NaOH])/(Δt) NaClO3NaClO2H2O | 1 | 1 | (Δ[NaClO3NaClO2H2O])/(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[ClO2NaOH])/(Δt) = (Δ[NaClO3NaClO2H2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| ClO2NaOH | NaClO3NaClO2H2O formula | ClO2NaOH | NaClO3NaClO2H2O Hill formula | HClNaO3 | H2Cl2Na2O6

| ClO2NaOH | NaClO3NaClO2H2O molar mass | 107.4 g/mol | 214.9 g/mol