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HI + HClO = H2O + HCl + I2

Input interpretation

HI hydrogen iodide + HOCl hypochlorous acid ⟶ H_2O water + HCl hydrogen chloride + I_2 iodine
HI hydrogen iodide + HOCl hypochlorous acid ⟶ H_2O water + HCl hydrogen chloride + I_2 iodine

Balanced equation

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

Structures

+ ⟶ + +
+ ⟶ + +

Names

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

Equilibrium constant

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

Rate of reaction

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

Chemical names and formulas

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

Substance properties

| hydrogen iodide | hypochlorous acid | water | hydrogen chloride | iodine molar mass | 127.912 g/mol | 52.46 g/mol | 18.015 g/mol | 36.46 g/mol | 253.80894 g/mol phase | gas (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -50.76 °C | | 0 °C | -114.17 °C | 113 °C boiling point | -35.55 °C | | 99.9839 °C | -85 °C | 184 °C density | 0.005228 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 4.94 g/cm^3 solubility in water | very soluble | soluble | | miscible | surface tension | | | 0.0728 N/m | | dynamic viscosity | 0.001321 Pa s (at -39 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | 0.00227 Pa s (at 116 °C) odor | | | odorless | |
| hydrogen iodide | hypochlorous acid | water | hydrogen chloride | iodine molar mass | 127.912 g/mol | 52.46 g/mol | 18.015 g/mol | 36.46 g/mol | 253.80894 g/mol phase | gas (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -50.76 °C | | 0 °C | -114.17 °C | 113 °C boiling point | -35.55 °C | | 99.9839 °C | -85 °C | 184 °C density | 0.005228 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 4.94 g/cm^3 solubility in water | very soluble | soluble | | miscible | surface tension | | | 0.0728 N/m | | dynamic viscosity | 0.001321 Pa s (at -39 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | 0.00227 Pa s (at 116 °C) odor | | | odorless | |

Units

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