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H2O + I2 + HClO = HCl + HIO3

Input interpretation

H_2O water + I_2 iodine + HOCl hypochlorous acid ⟶ HCl hydrogen chloride + HIO_3 iodic acid
H_2O water + I_2 iodine + HOCl hypochlorous acid ⟶ HCl hydrogen chloride + HIO_3 iodic acid

Balanced equation

Balance the chemical equation algebraically: H_2O + I_2 + HOCl ⟶ HCl + HIO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 I_2 + c_3 HOCl ⟶ c_4 HCl + c_5 HIO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, I and Cl: H: | 2 c_1 + c_3 = c_4 + c_5 O: | c_1 + c_3 = 3 c_5 I: | 2 c_2 = c_5 Cl: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 5 c_4 = 5 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + I_2 + 5 HOCl ⟶ 5 HCl + 2 HIO_3
Balance the chemical equation algebraically: H_2O + I_2 + HOCl ⟶ HCl + HIO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 I_2 + c_3 HOCl ⟶ c_4 HCl + c_5 HIO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, I and Cl: H: | 2 c_1 + c_3 = c_4 + c_5 O: | c_1 + c_3 = 3 c_5 I: | 2 c_2 = c_5 Cl: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 5 c_4 = 5 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + I_2 + 5 HOCl ⟶ 5 HCl + 2 HIO_3

Structures

+ + ⟶ +
+ + ⟶ +

Names

water + iodine + hypochlorous acid ⟶ hydrogen chloride + iodic acid
water + iodine + hypochlorous acid ⟶ hydrogen chloride + iodic acid

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + I_2 + HOCl ⟶ HCl + HIO_3 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: H_2O + I_2 + 5 HOCl ⟶ 5 HCl + 2 HIO_3 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 H_2O | 1 | -1 I_2 | 1 | -1 HOCl | 5 | -5 HCl | 5 | 5 HIO_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) I_2 | 1 | -1 | ([I2])^(-1) HOCl | 5 | -5 | ([HOCl])^(-5) HCl | 5 | 5 | ([HCl])^5 HIO_3 | 2 | 2 | ([HIO3])^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 = ([H2O])^(-1) ([I2])^(-1) ([HOCl])^(-5) ([HCl])^5 ([HIO3])^2 = (([HCl])^5 ([HIO3])^2)/([H2O] [I2] ([HOCl])^5)
Construct the equilibrium constant, K, expression for: H_2O + I_2 + HOCl ⟶ HCl + HIO_3 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: H_2O + I_2 + 5 HOCl ⟶ 5 HCl + 2 HIO_3 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 H_2O | 1 | -1 I_2 | 1 | -1 HOCl | 5 | -5 HCl | 5 | 5 HIO_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) I_2 | 1 | -1 | ([I2])^(-1) HOCl | 5 | -5 | ([HOCl])^(-5) HCl | 5 | 5 | ([HCl])^5 HIO_3 | 2 | 2 | ([HIO3])^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 = ([H2O])^(-1) ([I2])^(-1) ([HOCl])^(-5) ([HCl])^5 ([HIO3])^2 = (([HCl])^5 ([HIO3])^2)/([H2O] [I2] ([HOCl])^5)

Rate of reaction

Construct the rate of reaction expression for: H_2O + I_2 + HOCl ⟶ HCl + HIO_3 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: H_2O + I_2 + 5 HOCl ⟶ 5 HCl + 2 HIO_3 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 H_2O | 1 | -1 I_2 | 1 | -1 HOCl | 5 | -5 HCl | 5 | 5 HIO_3 | 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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) I_2 | 1 | -1 | -(Δ[I2])/(Δt) HOCl | 5 | -5 | -1/5 (Δ[HOCl])/(Δt) HCl | 5 | 5 | 1/5 (Δ[HCl])/(Δt) HIO_3 | 2 | 2 | 1/2 (Δ[HIO3])/(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[H2O])/(Δt) = -(Δ[I2])/(Δt) = -1/5 (Δ[HOCl])/(Δt) = 1/5 (Δ[HCl])/(Δt) = 1/2 (Δ[HIO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + I_2 + HOCl ⟶ HCl + HIO_3 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: H_2O + I_2 + 5 HOCl ⟶ 5 HCl + 2 HIO_3 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 H_2O | 1 | -1 I_2 | 1 | -1 HOCl | 5 | -5 HCl | 5 | 5 HIO_3 | 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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) I_2 | 1 | -1 | -(Δ[I2])/(Δt) HOCl | 5 | -5 | -1/5 (Δ[HOCl])/(Δt) HCl | 5 | 5 | 1/5 (Δ[HCl])/(Δt) HIO_3 | 2 | 2 | 1/2 (Δ[HIO3])/(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[H2O])/(Δt) = -(Δ[I2])/(Δt) = -1/5 (Δ[HOCl])/(Δt) = 1/5 (Δ[HCl])/(Δt) = 1/2 (Δ[HIO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | iodine | hypochlorous acid | hydrogen chloride | iodic acid formula | H_2O | I_2 | HOCl | HCl | HIO_3 Hill formula | H_2O | I_2 | ClHO | ClH | HIO_3 name | water | iodine | hypochlorous acid | hydrogen chloride | iodic acid IUPAC name | water | molecular iodine | hypochlorous acid | hydrogen chloride | iodic acid
| water | iodine | hypochlorous acid | hydrogen chloride | iodic acid formula | H_2O | I_2 | HOCl | HCl | HIO_3 Hill formula | H_2O | I_2 | ClHO | ClH | HIO_3 name | water | iodine | hypochlorous acid | hydrogen chloride | iodic acid IUPAC name | water | molecular iodine | hypochlorous acid | hydrogen chloride | iodic acid

Substance properties

| water | iodine | hypochlorous acid | hydrogen chloride | iodic acid molar mass | 18.015 g/mol | 253.80894 g/mol | 52.46 g/mol | 36.46 g/mol | 175.91 g/mol phase | liquid (at STP) | solid (at STP) | | gas (at STP) | solid (at STP) melting point | 0 °C | 113 °C | | -114.17 °C | 110 °C boiling point | 99.9839 °C | 184 °C | | -85 °C | density | 1 g/cm^3 | 4.94 g/cm^3 | | 0.00149 g/cm^3 (at 25 °C) | 4.629 g/cm^3 solubility in water | | | soluble | miscible | very soluble surface tension | 0.0728 N/m | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 0.00227 Pa s (at 116 °C) | | | odor | odorless | | | |
| water | iodine | hypochlorous acid | hydrogen chloride | iodic acid molar mass | 18.015 g/mol | 253.80894 g/mol | 52.46 g/mol | 36.46 g/mol | 175.91 g/mol phase | liquid (at STP) | solid (at STP) | | gas (at STP) | solid (at STP) melting point | 0 °C | 113 °C | | -114.17 °C | 110 °C boiling point | 99.9839 °C | 184 °C | | -85 °C | density | 1 g/cm^3 | 4.94 g/cm^3 | | 0.00149 g/cm^3 (at 25 °C) | 4.629 g/cm^3 solubility in water | | | soluble | miscible | very soluble surface tension | 0.0728 N/m | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 0.00227 Pa s (at 116 °C) | | | odor | odorless | | | |

Units

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