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KOH + I2 = H2O + KI + K2IO3

Input interpretation

KOH potassium hydroxide + I_2 iodine ⟶ H_2O water + KI potassium iodide + K2IO3
KOH potassium hydroxide + I_2 iodine ⟶ H_2O water + KI potassium iodide + K2IO3

Balanced equation

Balance the chemical equation algebraically: KOH + I_2 ⟶ H_2O + KI + K2IO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 I_2 ⟶ c_3 H_2O + c_4 KI + c_5 K2IO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O and I: H: | c_1 = 2 c_3 K: | c_1 = c_4 + 2 c_5 O: | c_1 = c_3 + 3 c_5 I: | 2 c_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 = 6 c_2 = 5/2 c_3 = 3 c_4 = 4 c_5 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 12 c_2 = 5 c_3 = 6 c_4 = 8 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 12 KOH + 5 I_2 ⟶ 6 H_2O + 8 KI + 2 K2IO3
Balance the chemical equation algebraically: KOH + I_2 ⟶ H_2O + KI + K2IO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 I_2 ⟶ c_3 H_2O + c_4 KI + c_5 K2IO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O and I: H: | c_1 = 2 c_3 K: | c_1 = c_4 + 2 c_5 O: | c_1 = c_3 + 3 c_5 I: | 2 c_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 = 6 c_2 = 5/2 c_3 = 3 c_4 = 4 c_5 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 12 c_2 = 5 c_3 = 6 c_4 = 8 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 12 KOH + 5 I_2 ⟶ 6 H_2O + 8 KI + 2 K2IO3

Structures

+ ⟶ + + K2IO3
+ ⟶ + + K2IO3

Names

potassium hydroxide + iodine ⟶ water + potassium iodide + K2IO3
potassium hydroxide + iodine ⟶ water + potassium iodide + K2IO3

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + I_2 ⟶ H_2O + KI + K2IO3 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: 12 KOH + 5 I_2 ⟶ 6 H_2O + 8 KI + 2 K2IO3 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 KOH | 12 | -12 I_2 | 5 | -5 H_2O | 6 | 6 KI | 8 | 8 K2IO3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 12 | -12 | ([KOH])^(-12) I_2 | 5 | -5 | ([I2])^(-5) H_2O | 6 | 6 | ([H2O])^6 KI | 8 | 8 | ([KI])^8 K2IO3 | 2 | 2 | ([K2IO3])^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 = ([KOH])^(-12) ([I2])^(-5) ([H2O])^6 ([KI])^8 ([K2IO3])^2 = (([H2O])^6 ([KI])^8 ([K2IO3])^2)/(([KOH])^12 ([I2])^5)
Construct the equilibrium constant, K, expression for: KOH + I_2 ⟶ H_2O + KI + K2IO3 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: 12 KOH + 5 I_2 ⟶ 6 H_2O + 8 KI + 2 K2IO3 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 KOH | 12 | -12 I_2 | 5 | -5 H_2O | 6 | 6 KI | 8 | 8 K2IO3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 12 | -12 | ([KOH])^(-12) I_2 | 5 | -5 | ([I2])^(-5) H_2O | 6 | 6 | ([H2O])^6 KI | 8 | 8 | ([KI])^8 K2IO3 | 2 | 2 | ([K2IO3])^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 = ([KOH])^(-12) ([I2])^(-5) ([H2O])^6 ([KI])^8 ([K2IO3])^2 = (([H2O])^6 ([KI])^8 ([K2IO3])^2)/(([KOH])^12 ([I2])^5)

Rate of reaction

Construct the rate of reaction expression for: KOH + I_2 ⟶ H_2O + KI + K2IO3 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: 12 KOH + 5 I_2 ⟶ 6 H_2O + 8 KI + 2 K2IO3 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 KOH | 12 | -12 I_2 | 5 | -5 H_2O | 6 | 6 KI | 8 | 8 K2IO3 | 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 KOH | 12 | -12 | -1/12 (Δ[KOH])/(Δt) I_2 | 5 | -5 | -1/5 (Δ[I2])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) KI | 8 | 8 | 1/8 (Δ[KI])/(Δt) K2IO3 | 2 | 2 | 1/2 (Δ[K2IO3])/(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 = -1/12 (Δ[KOH])/(Δt) = -1/5 (Δ[I2])/(Δt) = 1/6 (Δ[H2O])/(Δt) = 1/8 (Δ[KI])/(Δt) = 1/2 (Δ[K2IO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + I_2 ⟶ H_2O + KI + K2IO3 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: 12 KOH + 5 I_2 ⟶ 6 H_2O + 8 KI + 2 K2IO3 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 KOH | 12 | -12 I_2 | 5 | -5 H_2O | 6 | 6 KI | 8 | 8 K2IO3 | 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 KOH | 12 | -12 | -1/12 (Δ[KOH])/(Δt) I_2 | 5 | -5 | -1/5 (Δ[I2])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) KI | 8 | 8 | 1/8 (Δ[KI])/(Δt) K2IO3 | 2 | 2 | 1/2 (Δ[K2IO3])/(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 = -1/12 (Δ[KOH])/(Δt) = -1/5 (Δ[I2])/(Δt) = 1/6 (Δ[H2O])/(Δt) = 1/8 (Δ[KI])/(Δt) = 1/2 (Δ[K2IO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | iodine | water | potassium iodide | K2IO3 formula | KOH | I_2 | H_2O | KI | K2IO3 Hill formula | HKO | I_2 | H_2O | IK | IK2O3 name | potassium hydroxide | iodine | water | potassium iodide | IUPAC name | potassium hydroxide | molecular iodine | water | potassium iodide |
| potassium hydroxide | iodine | water | potassium iodide | K2IO3 formula | KOH | I_2 | H_2O | KI | K2IO3 Hill formula | HKO | I_2 | H_2O | IK | IK2O3 name | potassium hydroxide | iodine | water | potassium iodide | IUPAC name | potassium hydroxide | molecular iodine | water | potassium iodide |

Substance properties

| potassium hydroxide | iodine | water | potassium iodide | K2IO3 molar mass | 56.105 g/mol | 253.80894 g/mol | 18.015 g/mol | 166.0028 g/mol | 253.098 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | melting point | 406 °C | 113 °C | 0 °C | 681 °C | boiling point | 1327 °C | 184 °C | 99.9839 °C | 1330 °C | density | 2.044 g/cm^3 | 4.94 g/cm^3 | 1 g/cm^3 | 3.123 g/cm^3 | solubility in water | soluble | | | | surface tension | | | 0.0728 N/m | | dynamic viscosity | 0.001 Pa s (at 550 °C) | 0.00227 Pa s (at 116 °C) | 8.9×10^-4 Pa s (at 25 °C) | 0.0010227 Pa s (at 732.9 °C) | odor | | | odorless | |
| potassium hydroxide | iodine | water | potassium iodide | K2IO3 molar mass | 56.105 g/mol | 253.80894 g/mol | 18.015 g/mol | 166.0028 g/mol | 253.098 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | melting point | 406 °C | 113 °C | 0 °C | 681 °C | boiling point | 1327 °C | 184 °C | 99.9839 °C | 1330 °C | density | 2.044 g/cm^3 | 4.94 g/cm^3 | 1 g/cm^3 | 3.123 g/cm^3 | solubility in water | soluble | | | | surface tension | | | 0.0728 N/m | | dynamic viscosity | 0.001 Pa s (at 550 °C) | 0.00227 Pa s (at 116 °C) | 8.9×10^-4 Pa s (at 25 °C) | 0.0010227 Pa s (at 732.9 °C) | odor | | | odorless | |

Units

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