I2 + H2O2 = H2O + HIO4

I_2 iodine + H_2O_2 hydrogen peroxide ⟶ H_2O water + HIO4

Balance the chemical equation algebraically: I_2 + H_2O_2 ⟶ H_2O + HIO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 I_2 + c_2 H_2O_2 ⟶ c_3 H_2O + c_4 HIO4 Set the number of atoms in the reactants equal to the number of atoms in the products for I, H and O: I: | 2 c_1 = c_4 H: | 2 c_2 = 2 c_3 + c_4 O: | 2 c_2 = c_3 + 4 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 7 c_3 = 6 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | I_2 + 7 H_2O_2 ⟶ 6 H_2O + 2 HIO4

+ ⟶ + HIO4

iodine + hydrogen peroxide ⟶ water + HIO4

Construct the equilibrium constant, K, expression for: I_2 + H_2O_2 ⟶ H_2O + HIO4 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: I_2 + 7 H_2O_2 ⟶ 6 H_2O + 2 HIO4 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 I_2 | 1 | -1 H_2O_2 | 7 | -7 H_2O | 6 | 6 HIO4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression I_2 | 1 | -1 | ([I2])^(-1) H_2O_2 | 7 | -7 | ([H2O2])^(-7) H_2O | 6 | 6 | ([H2O])^6 HIO4 | 2 | 2 | ([HIO4])^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 = ([I2])^(-1) ([H2O2])^(-7) ([H2O])^6 ([HIO4])^2 = (([H2O])^6 ([HIO4])^2)/([I2] ([H2O2])^7)

Construct the rate of reaction expression for: I_2 + H_2O_2 ⟶ H_2O + HIO4 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: I_2 + 7 H_2O_2 ⟶ 6 H_2O + 2 HIO4 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 I_2 | 1 | -1 H_2O_2 | 7 | -7 H_2O | 6 | 6 HIO4 | 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 I_2 | 1 | -1 | -(Δ[I2])/(Δt) H_2O_2 | 7 | -7 | -1/7 (Δ[H2O2])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) HIO4 | 2 | 2 | 1/2 (Δ[HIO4])/(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[I2])/(Δt) = -1/7 (Δ[H2O2])/(Δt) = 1/6 (Δ[H2O])/(Δt) = 1/2 (Δ[HIO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| iodine | hydrogen peroxide | water | HIO4 formula | I_2 | H_2O_2 | H_2O | HIO4 name | iodine | hydrogen peroxide | water | IUPAC name | molecular iodine | hydrogen peroxide | water |

| iodine | hydrogen peroxide | water | HIO4 molar mass | 253.80894 g/mol | 34.014 g/mol | 18.015 g/mol | 191.91 g/mol phase | solid (at STP) | liquid (at STP) | liquid (at STP) | melting point | 113 °C | -0.43 °C | 0 °C | boiling point | 184 °C | 150.2 °C | 99.9839 °C | density | 4.94 g/cm^3 | 1.44 g/cm^3 | 1 g/cm^3 | solubility in water | | miscible | | surface tension | | 0.0804 N/m | 0.0728 N/m | dynamic viscosity | 0.00227 Pa s (at 116 °C) | 0.001249 Pa s (at 20 °C) | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless |