H2O + NO + HgNO32 = HNO3 + Hg

H_2O water + NO nitric oxide + HgNO32 ⟶ HNO_3 nitric acid + Hg mercury

Balance the chemical equation algebraically: H_2O + NO + HgNO32 ⟶ HNO_3 + Hg Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 NO + c_3 HgNO32 ⟶ c_4 HNO_3 + c_5 Hg Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, N and Hg: H: | 2 c_1 = c_4 O: | c_1 + c_2 + 32 c_3 = 3 c_4 N: | c_2 + c_3 = c_4 Hg: | c_3 = 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 = 31/3 c_2 = 59/3 c_3 = 1 c_4 = 62/3 c_5 = 1 Multiply by the least common denominator, 3, to eliminate fractional coefficients: c_1 = 31 c_2 = 59 c_3 = 3 c_4 = 62 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 31 H_2O + 59 NO + 3 HgNO32 ⟶ 62 HNO_3 + 3 Hg

+ + HgNO32 ⟶ +

water + nitric oxide + HgNO32 ⟶ nitric acid + mercury

Construct the equilibrium constant, K, expression for: H_2O + NO + HgNO32 ⟶ HNO_3 + Hg 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: 31 H_2O + 59 NO + 3 HgNO32 ⟶ 62 HNO_3 + 3 Hg 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 | 31 | -31 NO | 59 | -59 HgNO32 | 3 | -3 HNO_3 | 62 | 62 Hg | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 31 | -31 | ([H2O])^(-31) NO | 59 | -59 | ([NO])^(-59) HgNO32 | 3 | -3 | ([HgNO32])^(-3) HNO_3 | 62 | 62 | ([HNO3])^62 Hg | 3 | 3 | ([Hg])^3 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])^(-31) ([NO])^(-59) ([HgNO32])^(-3) ([HNO3])^62 ([Hg])^3 = (([HNO3])^62 ([Hg])^3)/(([H2O])^31 ([NO])^59 ([HgNO32])^3)

Construct the rate of reaction expression for: H_2O + NO + HgNO32 ⟶ HNO_3 + Hg 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: 31 H_2O + 59 NO + 3 HgNO32 ⟶ 62 HNO_3 + 3 Hg 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 | 31 | -31 NO | 59 | -59 HgNO32 | 3 | -3 HNO_3 | 62 | 62 Hg | 3 | 3 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 | 31 | -31 | -1/31 (Δ[H2O])/(Δt) NO | 59 | -59 | -1/59 (Δ[NO])/(Δt) HgNO32 | 3 | -3 | -1/3 (Δ[HgNO32])/(Δt) HNO_3 | 62 | 62 | 1/62 (Δ[HNO3])/(Δt) Hg | 3 | 3 | 1/3 (Δ[Hg])/(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 = -1/31 (Δ[H2O])/(Δt) = -1/59 (Δ[NO])/(Δt) = -1/3 (Δ[HgNO32])/(Δt) = 1/62 (Δ[HNO3])/(Δt) = 1/3 (Δ[Hg])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| water | nitric oxide | HgNO32 | nitric acid | mercury formula | H_2O | NO | HgNO32 | HNO_3 | Hg name | water | nitric oxide | | nitric acid | mercury

| water | nitric oxide | HgNO32 | nitric acid | mercury molar mass | 18.015 g/mol | 30.006 g/mol | 726.57 g/mol | 63.012 g/mol | 200.592 g/mol phase | liquid (at STP) | gas (at STP) | | liquid (at STP) | liquid (at STP) melting point | 0 °C | -163.6 °C | | -41.6 °C | -38.87 °C boiling point | 99.9839 °C | -151.7 °C | | 83 °C | 356.6 °C density | 1 g/cm^3 | 0.001226 g/cm^3 (at 25 °C) | | 1.5129 g/cm^3 | 13.534 g/cm^3 solubility in water | | | | miscible | slightly soluble surface tension | 0.0728 N/m | | | | 0.47 N/m dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 1.911×10^-5 Pa s (at 25 °C) | | 7.6×10^-4 Pa s (at 25 °C) | 0.001526 Pa s (at 25 °C) odor | odorless | | | | odorless