HNO3 + Hg = HgHNO3

HNO_3 nitric acid + Hg mercury ⟶ HgHNO3

Balance the chemical equation algebraically: HNO_3 + Hg ⟶ HgHNO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Hg ⟶ c_3 HgHNO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Hg: H: | c_1 = c_3 N: | c_1 = c_3 O: | 3 c_1 = 3 c_3 Hg: | c_2 = c_3 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | HNO_3 + Hg ⟶ HgHNO3

+ ⟶ HgHNO3

nitric acid + mercury ⟶ HgHNO3

Construct the equilibrium constant, K, expression for: HNO_3 + Hg ⟶ HgHNO3 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: HNO_3 + Hg ⟶ HgHNO3 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 | 1 | -1 Hg | 1 | -1 HgHNO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 1 | -1 | ([HNO3])^(-1) Hg | 1 | -1 | ([Hg])^(-1) HgHNO3 | 1 | 1 | [HgHNO3] 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])^(-1) ([Hg])^(-1) [HgHNO3] = ([HgHNO3])/([HNO3] [Hg])

Construct the rate of reaction expression for: HNO_3 + Hg ⟶ HgHNO3 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: HNO_3 + Hg ⟶ HgHNO3 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 | 1 | -1 Hg | 1 | -1 HgHNO3 | 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 HNO_3 | 1 | -1 | -(Δ[HNO3])/(Δt) Hg | 1 | -1 | -(Δ[Hg])/(Δt) HgHNO3 | 1 | 1 | (Δ[HgHNO3])/(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 = -(Δ[HNO3])/(Δt) = -(Δ[Hg])/(Δt) = (Δ[HgHNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| nitric acid | mercury | HgHNO3 formula | HNO_3 | Hg | HgHNO3 Hill formula | HNO_3 | Hg | HHgNO3 name | nitric acid | mercury |

| nitric acid | mercury | HgHNO3 molar mass | 63.012 g/mol | 200.592 g/mol | 263.6 g/mol phase | liquid (at STP) | liquid (at STP) | melting point | -41.6 °C | -38.87 °C | boiling point | 83 °C | 356.6 °C | density | 1.5129 g/cm^3 | 13.534 g/cm^3 | solubility in water | miscible | slightly soluble | surface tension | | 0.47 N/m | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | 0.001526 Pa s (at 25 °C) | odor | | odorless |