HNO3 + KI = H2O + I2 + NO2 + KNO3

HNO_3 nitric acid + KI potassium iodide ⟶ H_2O water + I_2 iodine + NO_2 nitrogen dioxide + KNO_3 potassium nitrate

Balance the chemical equation algebraically: HNO_3 + KI ⟶ H_2O + I_2 + NO_2 + KNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 KI ⟶ c_3 H_2O + c_4 I_2 + c_5 NO_2 + c_6 KNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, I and K: H: | c_1 = 2 c_3 N: | c_1 = c_5 + c_6 O: | 3 c_1 = c_3 + 2 c_5 + 3 c_6 I: | c_2 = 2 c_4 K: | c_2 = 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 2 c_3 = 2 c_4 = 1 c_5 = 2 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 HNO_3 + 2 KI ⟶ 2 H_2O + I_2 + 2 NO_2 + 2 KNO_3

+ ⟶ + + +

nitric acid + potassium iodide ⟶ water + iodine + nitrogen dioxide + potassium nitrate

| nitric acid | potassium iodide | water | iodine | nitrogen dioxide | potassium nitrate molecular free energy | -80.7 kJ/mol | -324.9 kJ/mol | -237.1 kJ/mol | 0 kJ/mol | 51.3 kJ/mol | -394.9 kJ/mol total free energy | -322.8 kJ/mol | -649.8 kJ/mol | -474.2 kJ/mol | 0 kJ/mol | 102.6 kJ/mol | -789.8 kJ/mol | G_initial = -972.6 kJ/mol | | G_final = -1161 kJ/mol | | | ΔG_rxn^0 | -1161 kJ/mol - -972.6 kJ/mol = -188.8 kJ/mol (exergonic) | | | | |

Construct the equilibrium constant, K, expression for: HNO_3 + KI ⟶ H_2O + I_2 + NO_2 + KNO_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: 4 HNO_3 + 2 KI ⟶ 2 H_2O + I_2 + 2 NO_2 + 2 KNO_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 HNO_3 | 4 | -4 KI | 2 | -2 H_2O | 2 | 2 I_2 | 1 | 1 NO_2 | 2 | 2 KNO_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 4 | -4 | ([HNO3])^(-4) KI | 2 | -2 | ([KI])^(-2) H_2O | 2 | 2 | ([H2O])^2 I_2 | 1 | 1 | [I2] NO_2 | 2 | 2 | ([NO2])^2 KNO_3 | 2 | 2 | ([KNO3])^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 = ([HNO3])^(-4) ([KI])^(-2) ([H2O])^2 [I2] ([NO2])^2 ([KNO3])^2 = (([H2O])^2 [I2] ([NO2])^2 ([KNO3])^2)/(([HNO3])^4 ([KI])^2)

Construct the rate of reaction expression for: HNO_3 + KI ⟶ H_2O + I_2 + NO_2 + KNO_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: 4 HNO_3 + 2 KI ⟶ 2 H_2O + I_2 + 2 NO_2 + 2 KNO_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 HNO_3 | 4 | -4 KI | 2 | -2 H_2O | 2 | 2 I_2 | 1 | 1 NO_2 | 2 | 2 KNO_3 | 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 HNO_3 | 4 | -4 | -1/4 (Δ[HNO3])/(Δt) KI | 2 | -2 | -1/2 (Δ[KI])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) NO_2 | 2 | 2 | 1/2 (Δ[NO2])/(Δt) KNO_3 | 2 | 2 | 1/2 (Δ[KNO3])/(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 = -1/4 (Δ[HNO3])/(Δt) = -1/2 (Δ[KI])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[I2])/(Δt) = 1/2 (Δ[NO2])/(Δt) = 1/2 (Δ[KNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| nitric acid | potassium iodide | water | iodine | nitrogen dioxide | potassium nitrate formula | HNO_3 | KI | H_2O | I_2 | NO_2 | KNO_3 Hill formula | HNO_3 | IK | H_2O | I_2 | NO_2 | KNO_3 name | nitric acid | potassium iodide | water | iodine | nitrogen dioxide | potassium nitrate IUPAC name | nitric acid | potassium iodide | water | molecular iodine | Nitrogen dioxide | potassium nitrate