H2O + NO + HClO4 = HCl + HNO3

H_2O water + NO nitric oxide + HClO_4 perchloric acid ⟶ HCl hydrogen chloride + HNO_3 nitric acid

Balance the chemical equation algebraically: H_2O + NO + HClO_4 ⟶ HCl + HNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 NO + c_3 HClO_4 ⟶ c_4 HCl + c_5 HNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, N and Cl: H: | 2 c_1 + c_3 = c_4 + c_5 O: | c_1 + c_2 + 4 c_3 = 3 c_5 N: | c_2 = c_5 Cl: | c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4/3 c_2 = 8/3 c_3 = 1 c_4 = 1 c_5 = 8/3 Multiply by the least common denominator, 3, to eliminate fractional coefficients: c_1 = 4 c_2 = 8 c_3 = 3 c_4 = 3 c_5 = 8 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2O + 8 NO + 3 HClO_4 ⟶ 3 HCl + 8 HNO_3

+ + ⟶ +

water + nitric oxide + perchloric acid ⟶ hydrogen chloride + nitric acid

Construct the equilibrium constant, K, expression for: H_2O + NO + HClO_4 ⟶ HCl + HNO_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 H_2O + 8 NO + 3 HClO_4 ⟶ 3 HCl + 8 HNO_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 H_2O | 4 | -4 NO | 8 | -8 HClO_4 | 3 | -3 HCl | 3 | 3 HNO_3 | 8 | 8 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 4 | -4 | ([H2O])^(-4) NO | 8 | -8 | ([NO])^(-8) HClO_4 | 3 | -3 | ([HClO4])^(-3) HCl | 3 | 3 | ([HCl])^3 HNO_3 | 8 | 8 | ([HNO3])^8 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 = ([H2O])^(-4) ([NO])^(-8) ([HClO4])^(-3) ([HCl])^3 ([HNO3])^8 = (([HCl])^3 ([HNO3])^8)/(([H2O])^4 ([NO])^8 ([HClO4])^3)

Construct the rate of reaction expression for: H_2O + NO + HClO_4 ⟶ HCl + HNO_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 H_2O + 8 NO + 3 HClO_4 ⟶ 3 HCl + 8 HNO_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 H_2O | 4 | -4 NO | 8 | -8 HClO_4 | 3 | -3 HCl | 3 | 3 HNO_3 | 8 | 8 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 H_2O | 4 | -4 | -1/4 (Δ[H2O])/(Δt) NO | 8 | -8 | -1/8 (Δ[NO])/(Δt) HClO_4 | 3 | -3 | -1/3 (Δ[HClO4])/(Δt) HCl | 3 | 3 | 1/3 (Δ[HCl])/(Δt) HNO_3 | 8 | 8 | 1/8 (Δ[HNO3])/(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[H2O])/(Δt) = -1/8 (Δ[NO])/(Δt) = -1/3 (Δ[HClO4])/(Δt) = 1/3 (Δ[HCl])/(Δt) = 1/8 (Δ[HNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| water | nitric oxide | perchloric acid | hydrogen chloride | nitric acid formula | H_2O | NO | HClO_4 | HCl | HNO_3 Hill formula | H_2O | NO | ClHO_4 | ClH | HNO_3 name | water | nitric oxide | perchloric acid | hydrogen chloride | nitric acid