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H2O + ICl = HCl + I2 + HIO3

Input interpretation

H_2O water + ICl iodine monochloride ⟶ HCl hydrogen chloride + I_2 iodine + HIO_3 iodic acid
H_2O water + ICl iodine monochloride ⟶ HCl hydrogen chloride + I_2 iodine + HIO_3 iodic acid

Balanced equation

Balance the chemical equation algebraically: H_2O + ICl ⟶ HCl + I_2 + HIO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 ICl ⟶ c_3 HCl + c_4 I_2 + c_5 HIO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl and I: H: | 2 c_1 = c_3 + c_5 O: | c_1 = 3 c_5 Cl: | c_2 = c_3 I: | c_2 = 2 c_4 + c_5 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 5 c_3 = 5 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2O + 5 ICl ⟶ 5 HCl + 2 I_2 + HIO_3
Balance the chemical equation algebraically: H_2O + ICl ⟶ HCl + I_2 + HIO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 ICl ⟶ c_3 HCl + c_4 I_2 + c_5 HIO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl and I: H: | 2 c_1 = c_3 + c_5 O: | c_1 = 3 c_5 Cl: | c_2 = c_3 I: | c_2 = 2 c_4 + c_5 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 5 c_3 = 5 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2O + 5 ICl ⟶ 5 HCl + 2 I_2 + HIO_3

Structures

+ ⟶ + +
+ ⟶ + +

Names

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

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + ICl ⟶ HCl + I_2 + 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: 3 H_2O + 5 ICl ⟶ 5 HCl + 2 I_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 | 3 | -3 ICl | 5 | -5 HCl | 5 | 5 I_2 | 2 | 2 HIO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 3 | -3 | ([H2O])^(-3) ICl | 5 | -5 | ([ICl])^(-5) HCl | 5 | 5 | ([HCl])^5 I_2 | 2 | 2 | ([I2])^2 HIO_3 | 1 | 1 | [HIO3] 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])^(-3) ([ICl])^(-5) ([HCl])^5 ([I2])^2 [HIO3] = (([HCl])^5 ([I2])^2 [HIO3])/(([H2O])^3 ([ICl])^5)
Construct the equilibrium constant, K, expression for: H_2O + ICl ⟶ HCl + I_2 + 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: 3 H_2O + 5 ICl ⟶ 5 HCl + 2 I_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 | 3 | -3 ICl | 5 | -5 HCl | 5 | 5 I_2 | 2 | 2 HIO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 3 | -3 | ([H2O])^(-3) ICl | 5 | -5 | ([ICl])^(-5) HCl | 5 | 5 | ([HCl])^5 I_2 | 2 | 2 | ([I2])^2 HIO_3 | 1 | 1 | [HIO3] 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])^(-3) ([ICl])^(-5) ([HCl])^5 ([I2])^2 [HIO3] = (([HCl])^5 ([I2])^2 [HIO3])/(([H2O])^3 ([ICl])^5)

Rate of reaction

Construct the rate of reaction expression for: H_2O + ICl ⟶ HCl + I_2 + 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: 3 H_2O + 5 ICl ⟶ 5 HCl + 2 I_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 | 3 | -3 ICl | 5 | -5 HCl | 5 | 5 I_2 | 2 | 2 HIO_3 | 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 H_2O | 3 | -3 | -1/3 (Δ[H2O])/(Δt) ICl | 5 | -5 | -1/5 (Δ[ICl])/(Δt) HCl | 5 | 5 | 1/5 (Δ[HCl])/(Δt) I_2 | 2 | 2 | 1/2 (Δ[I2])/(Δt) HIO_3 | 1 | 1 | (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 = -1/3 (Δ[H2O])/(Δt) = -1/5 (Δ[ICl])/(Δt) = 1/5 (Δ[HCl])/(Δt) = 1/2 (Δ[I2])/(Δt) = (Δ[HIO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + ICl ⟶ HCl + I_2 + 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: 3 H_2O + 5 ICl ⟶ 5 HCl + 2 I_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 | 3 | -3 ICl | 5 | -5 HCl | 5 | 5 I_2 | 2 | 2 HIO_3 | 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 H_2O | 3 | -3 | -1/3 (Δ[H2O])/(Δt) ICl | 5 | -5 | -1/5 (Δ[ICl])/(Δt) HCl | 5 | 5 | 1/5 (Δ[HCl])/(Δt) I_2 | 2 | 2 | 1/2 (Δ[I2])/(Δt) HIO_3 | 1 | 1 | (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 = -1/3 (Δ[H2O])/(Δt) = -1/5 (Δ[ICl])/(Δt) = 1/5 (Δ[HCl])/(Δt) = 1/2 (Δ[I2])/(Δt) = (Δ[HIO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | iodine monochloride | hydrogen chloride | iodine | iodic acid formula | H_2O | ICl | HCl | I_2 | HIO_3 Hill formula | H_2O | ClI | ClH | I_2 | HIO_3 name | water | iodine monochloride | hydrogen chloride | iodine | iodic acid IUPAC name | water | | hydrogen chloride | molecular iodine | iodic acid
| water | iodine monochloride | hydrogen chloride | iodine | iodic acid formula | H_2O | ICl | HCl | I_2 | HIO_3 Hill formula | H_2O | ClI | ClH | I_2 | HIO_3 name | water | iodine monochloride | hydrogen chloride | iodine | iodic acid IUPAC name | water | | hydrogen chloride | molecular iodine | iodic acid

Substance properties

| water | iodine monochloride | hydrogen chloride | iodine | iodic acid molar mass | 18.015 g/mol | 162.35 g/mol | 36.46 g/mol | 253.80894 g/mol | 175.91 g/mol phase | liquid (at STP) | solid (at STP) | gas (at STP) | solid (at STP) | solid (at STP) melting point | 0 °C | 26 °C | -114.17 °C | 113 °C | 110 °C boiling point | 99.9839 °C | 97.4 °C | -85 °C | 184 °C | density | 1 g/cm^3 | 3.24 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 4.94 g/cm^3 | 4.629 g/cm^3 solubility in water | | decomposes | 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 monochloride | hydrogen chloride | iodine | iodic acid molar mass | 18.015 g/mol | 162.35 g/mol | 36.46 g/mol | 253.80894 g/mol | 175.91 g/mol phase | liquid (at STP) | solid (at STP) | gas (at STP) | solid (at STP) | solid (at STP) melting point | 0 °C | 26 °C | -114.17 °C | 113 °C | 110 °C boiling point | 99.9839 °C | 97.4 °C | -85 °C | 184 °C | density | 1 g/cm^3 | 3.24 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 4.94 g/cm^3 | 4.629 g/cm^3 solubility in water | | decomposes | 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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