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KI + FeCl3 = I2 + KCl + FeI2

Input interpretation

KI potassium iodide + FeCl_3 iron(III) chloride ⟶ I_2 iodine + KCl potassium chloride + FeI_2 ferrous iodide
KI potassium iodide + FeCl_3 iron(III) chloride ⟶ I_2 iodine + KCl potassium chloride + FeI_2 ferrous iodide

Balanced equation

Balance the chemical equation algebraically: KI + FeCl_3 ⟶ I_2 + KCl + FeI_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KI + c_2 FeCl_3 ⟶ c_3 I_2 + c_4 KCl + c_5 FeI_2 Set the number of atoms in the reactants equal to the number of atoms in the products for I, K, Cl and Fe: I: | c_1 = 2 c_3 + 2 c_5 K: | c_1 = c_4 Cl: | 3 c_2 = c_4 Fe: | c_2 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 2 c_3 = 1 c_4 = 6 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 KI + 2 FeCl_3 ⟶ I_2 + 6 KCl + 2 FeI_2
Balance the chemical equation algebraically: KI + FeCl_3 ⟶ I_2 + KCl + FeI_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KI + c_2 FeCl_3 ⟶ c_3 I_2 + c_4 KCl + c_5 FeI_2 Set the number of atoms in the reactants equal to the number of atoms in the products for I, K, Cl and Fe: I: | c_1 = 2 c_3 + 2 c_5 K: | c_1 = c_4 Cl: | 3 c_2 = c_4 Fe: | c_2 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 2 c_3 = 1 c_4 = 6 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 KI + 2 FeCl_3 ⟶ I_2 + 6 KCl + 2 FeI_2

Structures

+ ⟶ + +
+ ⟶ + +

Names

potassium iodide + iron(III) chloride ⟶ iodine + potassium chloride + ferrous iodide
potassium iodide + iron(III) chloride ⟶ iodine + potassium chloride + ferrous iodide

Equilibrium constant

Construct the equilibrium constant, K, expression for: KI + FeCl_3 ⟶ I_2 + KCl + FeI_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: 6 KI + 2 FeCl_3 ⟶ I_2 + 6 KCl + 2 FeI_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 KI | 6 | -6 FeCl_3 | 2 | -2 I_2 | 1 | 1 KCl | 6 | 6 FeI_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KI | 6 | -6 | ([KI])^(-6) FeCl_3 | 2 | -2 | ([FeCl3])^(-2) I_2 | 1 | 1 | [I2] KCl | 6 | 6 | ([KCl])^6 FeI_2 | 2 | 2 | ([FeI2])^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 = ([KI])^(-6) ([FeCl3])^(-2) [I2] ([KCl])^6 ([FeI2])^2 = ([I2] ([KCl])^6 ([FeI2])^2)/(([KI])^6 ([FeCl3])^2)
Construct the equilibrium constant, K, expression for: KI + FeCl_3 ⟶ I_2 + KCl + FeI_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: 6 KI + 2 FeCl_3 ⟶ I_2 + 6 KCl + 2 FeI_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 KI | 6 | -6 FeCl_3 | 2 | -2 I_2 | 1 | 1 KCl | 6 | 6 FeI_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KI | 6 | -6 | ([KI])^(-6) FeCl_3 | 2 | -2 | ([FeCl3])^(-2) I_2 | 1 | 1 | [I2] KCl | 6 | 6 | ([KCl])^6 FeI_2 | 2 | 2 | ([FeI2])^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 = ([KI])^(-6) ([FeCl3])^(-2) [I2] ([KCl])^6 ([FeI2])^2 = ([I2] ([KCl])^6 ([FeI2])^2)/(([KI])^6 ([FeCl3])^2)

Rate of reaction

Construct the rate of reaction expression for: KI + FeCl_3 ⟶ I_2 + KCl + FeI_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: 6 KI + 2 FeCl_3 ⟶ I_2 + 6 KCl + 2 FeI_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 KI | 6 | -6 FeCl_3 | 2 | -2 I_2 | 1 | 1 KCl | 6 | 6 FeI_2 | 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 KI | 6 | -6 | -1/6 (Δ[KI])/(Δt) FeCl_3 | 2 | -2 | -1/2 (Δ[FeCl3])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) KCl | 6 | 6 | 1/6 (Δ[KCl])/(Δt) FeI_2 | 2 | 2 | 1/2 (Δ[FeI2])/(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 = -1/6 (Δ[KI])/(Δt) = -1/2 (Δ[FeCl3])/(Δt) = (Δ[I2])/(Δt) = 1/6 (Δ[KCl])/(Δt) = 1/2 (Δ[FeI2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KI + FeCl_3 ⟶ I_2 + KCl + FeI_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: 6 KI + 2 FeCl_3 ⟶ I_2 + 6 KCl + 2 FeI_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 KI | 6 | -6 FeCl_3 | 2 | -2 I_2 | 1 | 1 KCl | 6 | 6 FeI_2 | 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 KI | 6 | -6 | -1/6 (Δ[KI])/(Δt) FeCl_3 | 2 | -2 | -1/2 (Δ[FeCl3])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) KCl | 6 | 6 | 1/6 (Δ[KCl])/(Δt) FeI_2 | 2 | 2 | 1/2 (Δ[FeI2])/(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 = -1/6 (Δ[KI])/(Δt) = -1/2 (Δ[FeCl3])/(Δt) = (Δ[I2])/(Δt) = 1/6 (Δ[KCl])/(Δt) = 1/2 (Δ[FeI2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium iodide | iron(III) chloride | iodine | potassium chloride | ferrous iodide formula | KI | FeCl_3 | I_2 | KCl | FeI_2 Hill formula | IK | Cl_3Fe | I_2 | ClK | FeI_2 name | potassium iodide | iron(III) chloride | iodine | potassium chloride | ferrous iodide IUPAC name | potassium iodide | trichloroiron | molecular iodine | potassium chloride | diiodoiron
| potassium iodide | iron(III) chloride | iodine | potassium chloride | ferrous iodide formula | KI | FeCl_3 | I_2 | KCl | FeI_2 Hill formula | IK | Cl_3Fe | I_2 | ClK | FeI_2 name | potassium iodide | iron(III) chloride | iodine | potassium chloride | ferrous iodide IUPAC name | potassium iodide | trichloroiron | molecular iodine | potassium chloride | diiodoiron

Substance properties

| potassium iodide | iron(III) chloride | iodine | potassium chloride | ferrous iodide molar mass | 166.0028 g/mol | 162.2 g/mol | 253.80894 g/mol | 74.55 g/mol | 309.654 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 681 °C | 304 °C | 113 °C | 770 °C | boiling point | 1330 °C | | 184 °C | 1420 °C | density | 3.123 g/cm^3 | | 4.94 g/cm^3 | 1.98 g/cm^3 | 5.32 g/cm^3 solubility in water | | | | soluble | slightly soluble dynamic viscosity | 0.0010227 Pa s (at 732.9 °C) | | 0.00227 Pa s (at 116 °C) | | odor | | | | odorless |
| potassium iodide | iron(III) chloride | iodine | potassium chloride | ferrous iodide molar mass | 166.0028 g/mol | 162.2 g/mol | 253.80894 g/mol | 74.55 g/mol | 309.654 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 681 °C | 304 °C | 113 °C | 770 °C | boiling point | 1330 °C | | 184 °C | 1420 °C | density | 3.123 g/cm^3 | | 4.94 g/cm^3 | 1.98 g/cm^3 | 5.32 g/cm^3 solubility in water | | | | soluble | slightly soluble dynamic viscosity | 0.0010227 Pa s (at 732.9 °C) | | 0.00227 Pa s (at 116 °C) | | odor | | | | odorless |

Units

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