H2SeO3H2O2 = H2SeO4H2O

H2SeO3H2O2 ⟶ H2SeO4H2O

Balance the chemical equation algebraically: H2SeO3H2O2 ⟶ H2SeO4H2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H2SeO3H2O2 ⟶ c_2 H2SeO4H2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, Se and O: H: | 4 c_1 = 4 c_2 Se: | c_1 = c_2 O: | 5 c_1 = 5 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H2SeO3H2O2 ⟶ H2SeO4H2O

H2SeO3H2O2 ⟶ H2SeO4H2O

H2SeO3H2O2 ⟶ H2SeO4H2O

Construct the equilibrium constant, K, expression for: H2SeO3H2O2 ⟶ H2SeO4H2O 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: H2SeO3H2O2 ⟶ H2SeO4H2O 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 H2SeO3H2O2 | 1 | -1 H2SeO4H2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H2SeO3H2O2 | 1 | -1 | ([H2SeO3H2O2])^(-1) H2SeO4H2O | 1 | 1 | [H2SeO4H2O] 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 = ([H2SeO3H2O2])^(-1) [H2SeO4H2O] = ([H2SeO4H2O])/([H2SeO3H2O2])

Construct the rate of reaction expression for: H2SeO3H2O2 ⟶ H2SeO4H2O 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: H2SeO3H2O2 ⟶ H2SeO4H2O 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 H2SeO3H2O2 | 1 | -1 H2SeO4H2O | 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 H2SeO3H2O2 | 1 | -1 | -(Δ[H2SeO3H2O2])/(Δt) H2SeO4H2O | 1 | 1 | (Δ[H2SeO4H2O])/(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[H2SeO3H2O2])/(Δt) = (Δ[H2SeO4H2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| H2SeO3H2O2 | H2SeO4H2O formula | H2SeO3H2O2 | H2SeO4H2O Hill formula | H4O5Se | H4O5Se

| H2SeO3H2O2 | H2SeO4H2O molar mass | 163 g/mol | 163 g/mol