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KOH + I2 + K2SO3 = H2O + K2SO4 + KI

Input interpretation

KOH (potassium hydroxide) + I_2 (iodine) + K_2SO_3 (potassium sulfite) ⟶ H_2O (water) + K_2SO_4 (potassium sulfate) + KI (potassium iodide)
KOH (potassium hydroxide) + I_2 (iodine) + K_2SO_3 (potassium sulfite) ⟶ H_2O (water) + K_2SO_4 (potassium sulfate) + KI (potassium iodide)

Balanced equation

Balance the chemical equation algebraically: KOH + I_2 + K_2SO_3 ⟶ H_2O + K_2SO_4 + KI Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 I_2 + c_3 K_2SO_3 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 KI Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, I and S: H: | c_1 = 2 c_4 K: | c_1 + 2 c_3 = 2 c_5 + c_6 O: | c_1 + 3 c_3 = c_4 + 4 c_5 I: | 2 c_2 = c_6 S: | c_3 = 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_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 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + I_2 + K_2SO_3 ⟶ H_2O + K_2SO_4 + 2 KI
Balance the chemical equation algebraically: KOH + I_2 + K_2SO_3 ⟶ H_2O + K_2SO_4 + KI Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 I_2 + c_3 K_2SO_3 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 KI Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, I and S: H: | c_1 = 2 c_4 K: | c_1 + 2 c_3 = 2 c_5 + c_6 O: | c_1 + 3 c_3 = c_4 + 4 c_5 I: | 2 c_2 = c_6 S: | c_3 = 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_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 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + I_2 + K_2SO_3 ⟶ H_2O + K_2SO_4 + 2 KI

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

potassium hydroxide + iodine + potassium sulfite ⟶ water + potassium sulfate + potassium iodide
potassium hydroxide + iodine + potassium sulfite ⟶ water + potassium sulfate + potassium iodide

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + I_2 + K_2SO_3 ⟶ H_2O + K_2SO_4 + KI 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 KOH + I_2 + K_2SO_3 ⟶ H_2O + K_2SO_4 + 2 KI 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 | 2 | -2 I_2 | 1 | -1 K_2SO_3 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 KI | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 2 | -2 | ([KOH])^(-2) I_2 | 1 | -1 | ([I2])^(-1) K_2SO_3 | 1 | -1 | ([K2SO3])^(-1) H_2O | 1 | 1 | [H2O] K_2SO_4 | 1 | 1 | [K2SO4] KI | 2 | 2 | ([KI])^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])^(-2) ([I2])^(-1) ([K2SO3])^(-1) [H2O] [K2SO4] ([KI])^2 = ([H2O] [K2SO4] ([KI])^2)/(([KOH])^2 [I2] [K2SO3])
Construct the equilibrium constant, K, expression for: KOH + I_2 + K_2SO_3 ⟶ H_2O + K_2SO_4 + KI 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 KOH + I_2 + K_2SO_3 ⟶ H_2O + K_2SO_4 + 2 KI 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 | 2 | -2 I_2 | 1 | -1 K_2SO_3 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 KI | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 2 | -2 | ([KOH])^(-2) I_2 | 1 | -1 | ([I2])^(-1) K_2SO_3 | 1 | -1 | ([K2SO3])^(-1) H_2O | 1 | 1 | [H2O] K_2SO_4 | 1 | 1 | [K2SO4] KI | 2 | 2 | ([KI])^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])^(-2) ([I2])^(-1) ([K2SO3])^(-1) [H2O] [K2SO4] ([KI])^2 = ([H2O] [K2SO4] ([KI])^2)/(([KOH])^2 [I2] [K2SO3])

Rate of reaction

Construct the rate of reaction expression for: KOH + I_2 + K_2SO_3 ⟶ H_2O + K_2SO_4 + KI 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 KOH + I_2 + K_2SO_3 ⟶ H_2O + K_2SO_4 + 2 KI 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 | 2 | -2 I_2 | 1 | -1 K_2SO_3 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 KI | 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 | 2 | -2 | -1/2 (Δ[KOH])/(Δt) I_2 | 1 | -1 | -(Δ[I2])/(Δt) K_2SO_3 | 1 | -1 | -(Δ[K2SO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) KI | 2 | 2 | 1/2 (Δ[KI])/(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[KOH])/(Δt) = -(Δ[I2])/(Δt) = -(Δ[K2SO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[KI])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + I_2 + K_2SO_3 ⟶ H_2O + K_2SO_4 + KI 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 KOH + I_2 + K_2SO_3 ⟶ H_2O + K_2SO_4 + 2 KI 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 | 2 | -2 I_2 | 1 | -1 K_2SO_3 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 KI | 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 | 2 | -2 | -1/2 (Δ[KOH])/(Δt) I_2 | 1 | -1 | -(Δ[I2])/(Δt) K_2SO_3 | 1 | -1 | -(Δ[K2SO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) KI | 2 | 2 | 1/2 (Δ[KI])/(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[KOH])/(Δt) = -(Δ[I2])/(Δt) = -(Δ[K2SO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[KI])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | iodine | potassium sulfite | water | potassium sulfate | potassium iodide formula | KOH | I_2 | K_2SO_3 | H_2O | K_2SO_4 | KI Hill formula | HKO | I_2 | K_2O_3S | H_2O | K_2O_4S | IK name | potassium hydroxide | iodine | potassium sulfite | water | potassium sulfate | potassium iodide IUPAC name | potassium hydroxide | molecular iodine | dipotassium sulfite | water | dipotassium sulfate | potassium iodide
| potassium hydroxide | iodine | potassium sulfite | water | potassium sulfate | potassium iodide formula | KOH | I_2 | K_2SO_3 | H_2O | K_2SO_4 | KI Hill formula | HKO | I_2 | K_2O_3S | H_2O | K_2O_4S | IK name | potassium hydroxide | iodine | potassium sulfite | water | potassium sulfate | potassium iodide IUPAC name | potassium hydroxide | molecular iodine | dipotassium sulfite | water | dipotassium sulfate | potassium iodide

Substance properties

| potassium hydroxide | iodine | potassium sulfite | water | potassium sulfate | potassium iodide molar mass | 56.105 g/mol | 253.80894 g/mol | 158.25 g/mol | 18.015 g/mol | 174.25 g/mol | 166.0028 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 | | | | 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 | potassium sulfite | water | potassium sulfate | potassium iodide molar mass | 56.105 g/mol | 253.80894 g/mol | 158.25 g/mol | 18.015 g/mol | 174.25 g/mol | 166.0028 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 | | | | 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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