Cl2 + KOH + KI = H2O + KCl + KIO3

Cl_2 chlorine + KOH potassium hydroxide + KI potassium iodide ⟶ H_2O water + KCl potassium chloride + KIO_3 potassium iodate

Balance the chemical equation algebraically: Cl_2 + KOH + KI ⟶ H_2O + KCl + KIO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 KOH + c_3 KI ⟶ c_4 H_2O + c_5 KCl + c_6 KIO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, K, O and I: Cl: | 2 c_1 = c_5 H: | c_2 = 2 c_4 K: | c_2 + c_3 = c_5 + c_6 O: | c_2 = c_4 + 3 c_6 I: | c_3 = c_6 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 = 3 c_2 = 6 c_3 = 1 c_4 = 3 c_5 = 6 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Cl_2 + 6 KOH + KI ⟶ 3 H_2O + 6 KCl + KIO_3

+ + ⟶ + +

chlorine + potassium hydroxide + potassium iodide ⟶ water + potassium chloride + potassium iodate

| chlorine | potassium hydroxide | potassium iodide | water | potassium chloride | potassium iodate molecular enthalpy | 0 kJ/mol | -424.6 kJ/mol | -327.9 kJ/mol | -285.8 kJ/mol | -436.5 kJ/mol | -501.4 kJ/mol total enthalpy | 0 kJ/mol | -2548 kJ/mol | -327.9 kJ/mol | -857.5 kJ/mol | -2619 kJ/mol | -501.4 kJ/mol | H_initial = -2876 kJ/mol | | | H_final = -3978 kJ/mol | | ΔH_rxn^0 | -3978 kJ/mol - -2876 kJ/mol = -1102 kJ/mol (exothermic) | | | | |

| chlorine | potassium hydroxide | potassium iodide | water | potassium chloride | potassium iodate molecular free energy | 0 kJ/mol | -379.4 kJ/mol | -324.9 kJ/mol | -237.1 kJ/mol | -408.5 kJ/mol | -418.4 kJ/mol total free energy | 0 kJ/mol | -2276 kJ/mol | -324.9 kJ/mol | -711.3 kJ/mol | -2451 kJ/mol | -418.4 kJ/mol | G_initial = -2601 kJ/mol | | | G_final = -3581 kJ/mol | | ΔG_rxn^0 | -3581 kJ/mol - -2601 kJ/mol = -979.4 kJ/mol (exergonic) | | | | |

Construct the equilibrium constant, K, expression for: Cl_2 + KOH + KI ⟶ H_2O + KCl + KIO_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 Cl_2 + 6 KOH + KI ⟶ 3 H_2O + 6 KCl + KIO_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 Cl_2 | 3 | -3 KOH | 6 | -6 KI | 1 | -1 H_2O | 3 | 3 KCl | 6 | 6 KIO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 3 | -3 | ([Cl2])^(-3) KOH | 6 | -6 | ([KOH])^(-6) KI | 1 | -1 | ([KI])^(-1) H_2O | 3 | 3 | ([H2O])^3 KCl | 6 | 6 | ([KCl])^6 KIO_3 | 1 | 1 | [KIO3] 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 = ([Cl2])^(-3) ([KOH])^(-6) ([KI])^(-1) ([H2O])^3 ([KCl])^6 [KIO3] = (([H2O])^3 ([KCl])^6 [KIO3])/(([Cl2])^3 ([KOH])^6 [KI])

Construct the rate of reaction expression for: Cl_2 + KOH + KI ⟶ H_2O + KCl + KIO_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 Cl_2 + 6 KOH + KI ⟶ 3 H_2O + 6 KCl + KIO_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 Cl_2 | 3 | -3 KOH | 6 | -6 KI | 1 | -1 H_2O | 3 | 3 KCl | 6 | 6 KIO_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 Cl_2 | 3 | -3 | -1/3 (Δ[Cl2])/(Δt) KOH | 6 | -6 | -1/6 (Δ[KOH])/(Δt) KI | 1 | -1 | -(Δ[KI])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) KCl | 6 | 6 | 1/6 (Δ[KCl])/(Δt) KIO_3 | 1 | 1 | (Δ[KIO3])/(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[Cl2])/(Δt) = -1/6 (Δ[KOH])/(Δt) = -(Δ[KI])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/6 (Δ[KCl])/(Δt) = (Δ[KIO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| chlorine | potassium hydroxide | potassium iodide | water | potassium chloride | potassium iodate formula | Cl_2 | KOH | KI | H_2O | KCl | KIO_3 Hill formula | Cl_2 | HKO | IK | H_2O | ClK | IKO_3 name | chlorine | potassium hydroxide | potassium iodide | water | potassium chloride | potassium iodate IUPAC name | molecular chlorine | potassium hydroxide | potassium iodide | water | potassium chloride | potassium iodate

| chlorine | potassium hydroxide | potassium iodide | water | potassium chloride | potassium iodate molar mass | 70.9 g/mol | 56.105 g/mol | 166.0028 g/mol | 18.015 g/mol | 74.55 g/mol | 214 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | solid (at STP) melting point | -101 °C | 406 °C | 681 °C | 0 °C | 770 °C | 560 °C boiling point | -34 °C | 1327 °C | 1330 °C | 99.9839 °C | 1420 °C | density | 0.003214 g/cm^3 (at 0 °C) | 2.044 g/cm^3 | 3.123 g/cm^3 | 1 g/cm^3 | 1.98 g/cm^3 | 1.005 g/cm^3 solubility in water | | soluble | | | soluble | surface tension | | | | 0.0728 N/m | | dynamic viscosity | | 0.001 Pa s (at 550 °C) | 0.0010227 Pa s (at 732.9 °C) | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | | odorless | odorless |