O2 + Hg = Hg2O

O_2 oxygen + Hg mercury ⟶ O_1Hg_2 mercury(I) oxide

Balance the chemical equation algebraically: O_2 + Hg ⟶ O_1Hg_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 Hg ⟶ c_3 O_1Hg_2 Set the number of atoms in the reactants equal to the number of atoms in the products for O and Hg: O: | 2 c_1 = c_3 Hg: | c_2 = 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 = 4 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | O_2 + 4 Hg ⟶ 2 O_1Hg_2

+ ⟶

oxygen + mercury ⟶ mercury(I) oxide

Construct the equilibrium constant, K, expression for: O_2 + Hg ⟶ O_1Hg_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: O_2 + 4 Hg ⟶ 2 O_1Hg_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 O_2 | 1 | -1 Hg | 4 | -4 O_1Hg_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 1 | -1 | ([O2])^(-1) Hg | 4 | -4 | ([Hg])^(-4) O_1Hg_2 | 2 | 2 | ([O1Hg2])^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 = ([O2])^(-1) ([Hg])^(-4) ([O1Hg2])^2 = ([O1Hg2])^2/([O2] ([Hg])^4)

Construct the rate of reaction expression for: O_2 + Hg ⟶ O_1Hg_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: O_2 + 4 Hg ⟶ 2 O_1Hg_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 O_2 | 1 | -1 Hg | 4 | -4 O_1Hg_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 O_2 | 1 | -1 | -(Δ[O2])/(Δt) Hg | 4 | -4 | -1/4 (Δ[Hg])/(Δt) O_1Hg_2 | 2 | 2 | 1/2 (Δ[O1Hg2])/(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[O2])/(Δt) = -1/4 (Δ[Hg])/(Δt) = 1/2 (Δ[O1Hg2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| oxygen | mercury | mercury(I) oxide formula | O_2 | Hg | O_1Hg_2 Hill formula | O_2 | Hg | Hg_2O name | oxygen | mercury | mercury(I) oxide IUPAC name | molecular oxygen | mercury | mercuriooxymercury

| oxygen | mercury | mercury(I) oxide molar mass | 31.998 g/mol | 200.592 g/mol | 417.183 g/mol phase | gas (at STP) | liquid (at STP) | melting point | -218 °C | -38.87 °C | boiling point | -183 °C | 356.6 °C | density | 0.001429 g/cm^3 (at 0 °C) | 13.534 g/cm^3 | solubility in water | | slightly soluble | surface tension | 0.01347 N/m | 0.47 N/m | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | 0.001526 Pa s (at 25 °C) | odor | odorless | odorless |