HgS = S + Hg

HgS mercury(II) sulfide ⟶ S mixed sulfur + Hg mercury

Balance the chemical equation algebraically: HgS ⟶ S + Hg Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HgS ⟶ c_2 S + c_3 Hg Set the number of atoms in the reactants equal to the number of atoms in the products for Hg and S: Hg: | c_1 = c_3 S: | c_1 = c_2 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: | | HgS ⟶ S + Hg

⟶ +

mercury(II) sulfide ⟶ mixed sulfur + mercury

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

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

| mercury(II) sulfide | mixed sulfur | mercury formula | HgS | S | Hg name | mercury(II) sulfide | mixed sulfur | mercury IUPAC name | thioxomercury | sulfur | mercury

| mercury(II) sulfide | mixed sulfur | mercury molar mass | 232.65 g/mol | 32.06 g/mol | 200.592 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) melting point | 583.5 °C | 112.8 °C | -38.87 °C boiling point | | 444.7 °C | 356.6 °C density | 8.1 g/cm^3 | 2.07 g/cm^3 | 13.534 g/cm^3 solubility in water | insoluble | | slightly soluble surface tension | | | 0.47 N/m dynamic viscosity | | | 0.001526 Pa s (at 25 °C) odor | | | odorless