HNO3 + CuI = H2O + I2 + NO + CuNO3

HNO_3 nitric acid + CuI cuprous iodide ⟶ H_2O water + I_2 iodine + NO nitric oxide + CuNO3

Balance the chemical equation algebraically: HNO_3 + CuI ⟶ H_2O + I_2 + NO + CuNO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 CuI ⟶ c_3 H_2O + c_4 I_2 + c_5 NO + c_6 CuNO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, Cu and I: H: | c_1 = 2 c_3 N: | c_1 = c_5 + c_6 O: | 3 c_1 = c_3 + c_5 + 3 c_6 Cu: | c_2 = c_6 I: | c_2 = 2 c_4 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 = 4 c_2 = 3 c_3 = 2 c_4 = 3/2 c_5 = 1 c_6 = 3 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 8 c_2 = 6 c_3 = 4 c_4 = 3 c_5 = 2 c_6 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HNO_3 + 6 CuI ⟶ 4 H_2O + 3 I_2 + 2 NO + 6 CuNO3

+ ⟶ + + + CuNO3

nitric acid + cuprous iodide ⟶ water + iodine + nitric oxide + CuNO3

Construct the equilibrium constant, K, expression for: HNO_3 + CuI ⟶ H_2O + I_2 + NO + CuNO3 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: 8 HNO_3 + 6 CuI ⟶ 4 H_2O + 3 I_2 + 2 NO + 6 CuNO3 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 | 8 | -8 CuI | 6 | -6 H_2O | 4 | 4 I_2 | 3 | 3 NO | 2 | 2 CuNO3 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 8 | -8 | ([HNO3])^(-8) CuI | 6 | -6 | ([CuI])^(-6) H_2O | 4 | 4 | ([H2O])^4 I_2 | 3 | 3 | ([I2])^3 NO | 2 | 2 | ([NO])^2 CuNO3 | 6 | 6 | ([CuNO3])^6 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])^(-8) ([CuI])^(-6) ([H2O])^4 ([I2])^3 ([NO])^2 ([CuNO3])^6 = (([H2O])^4 ([I2])^3 ([NO])^2 ([CuNO3])^6)/(([HNO3])^8 ([CuI])^6)

Construct the rate of reaction expression for: HNO_3 + CuI ⟶ H_2O + I_2 + NO + CuNO3 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: 8 HNO_3 + 6 CuI ⟶ 4 H_2O + 3 I_2 + 2 NO + 6 CuNO3 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 | 8 | -8 CuI | 6 | -6 H_2O | 4 | 4 I_2 | 3 | 3 NO | 2 | 2 CuNO3 | 6 | 6 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 | 8 | -8 | -1/8 (Δ[HNO3])/(Δt) CuI | 6 | -6 | -1/6 (Δ[CuI])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) I_2 | 3 | 3 | 1/3 (Δ[I2])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) CuNO3 | 6 | 6 | 1/6 (Δ[CuNO3])/(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 = -1/8 (Δ[HNO3])/(Δt) = -1/6 (Δ[CuI])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/3 (Δ[I2])/(Δt) = 1/2 (Δ[NO])/(Δt) = 1/6 (Δ[CuNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| nitric acid | cuprous iodide | water | iodine | nitric oxide | CuNO3 formula | HNO_3 | CuI | H_2O | I_2 | NO | CuNO3 name | nitric acid | cuprous iodide | water | iodine | nitric oxide | IUPAC name | nitric acid | cuprous iodide | water | molecular iodine | nitric oxide |