Hg + XeF4 = Xe + HgF2

Hg mercury + F_4Xe_1 xenon tetrafluoride ⟶ Xe xenon + HgF_2 mercury(II) fluoride

Balance the chemical equation algebraically: Hg + F_4Xe_1 ⟶ Xe + HgF_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Hg + c_2 F_4Xe_1 ⟶ c_3 Xe + c_4 HgF_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Hg, F and Xe: Hg: | c_1 = c_4 F: | 4 c_2 = 2 c_4 Xe: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Hg + F_4Xe_1 ⟶ Xe + 2 HgF_2

+ ⟶ +

mercury + xenon tetrafluoride ⟶ xenon + mercury(II) fluoride

Construct the equilibrium constant, K, expression for: Hg + F_4Xe_1 ⟶ Xe + HgF_2 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: 2 Hg + F_4Xe_1 ⟶ Xe + 2 HgF_2 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 Hg | 2 | -2 F_4Xe_1 | 1 | -1 Xe | 1 | 1 HgF_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Hg | 2 | -2 | ([Hg])^(-2) F_4Xe_1 | 1 | -1 | ([F4Xe1])^(-1) Xe | 1 | 1 | [Xe] HgF_2 | 2 | 2 | ([HgF2])^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 = ([Hg])^(-2) ([F4Xe1])^(-1) [Xe] ([HgF2])^2 = ([Xe] ([HgF2])^2)/(([Hg])^2 [F4Xe1])

Construct the rate of reaction expression for: Hg + F_4Xe_1 ⟶ Xe + HgF_2 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: 2 Hg + F_4Xe_1 ⟶ Xe + 2 HgF_2 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 Hg | 2 | -2 F_4Xe_1 | 1 | -1 Xe | 1 | 1 HgF_2 | 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 Hg | 2 | -2 | -1/2 (Δ[Hg])/(Δt) F_4Xe_1 | 1 | -1 | -(Δ[F4Xe1])/(Δt) Xe | 1 | 1 | (Δ[Xe])/(Δt) HgF_2 | 2 | 2 | 1/2 (Δ[HgF2])/(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 = -1/2 (Δ[Hg])/(Δt) = -(Δ[F4Xe1])/(Δt) = (Δ[Xe])/(Δt) = 1/2 (Δ[HgF2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| mercury | xenon tetrafluoride | xenon | mercury(II) fluoride formula | Hg | F_4Xe_1 | Xe | HgF_2 Hill formula | Hg | F_4Xe | Xe | F_2Hg name | mercury | xenon tetrafluoride | xenon | mercury(II) fluoride IUPAC name | mercury | tetrafluoroxenon | xenon | mercury(2+) difluoride

| mercury | xenon tetrafluoride | xenon | mercury(II) fluoride molar mass | 200.592 g/mol | 207.287 g/mol | 131.293 g/mol | 238.589 g/mol phase | liquid (at STP) | | gas (at STP) | solid (at STP) melting point | -38.87 °C | | -111.8 °C | 645 °C boiling point | 356.6 °C | | -108 °C | 650 °C density | 13.534 g/cm^3 | | 0.0059 g/cm^3 (at 0 °C) | 8.95 g/cm^3 solubility in water | slightly soluble | | slightly soluble | reacts surface tension | 0.47 N/m | | | dynamic viscosity | 0.001526 Pa s (at 25 °C) | | 2.306×10^-5 Pa s (at 25 °C) | odor | odorless | | odorless |