H2S + Ag = H2 + AgS

H_2S hydrogen sulfide + Ag silver ⟶ H_2 hydrogen + AgS

Balance the chemical equation algebraically: H_2S + Ag ⟶ H_2 + AgS Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2S + c_2 Ag ⟶ c_3 H_2 + c_4 AgS Set the number of atoms in the reactants equal to the number of atoms in the products for H, S and Ag: H: | 2 c_1 = 2 c_3 S: | c_1 = c_4 Ag: | c_2 = c_4 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 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2S + Ag ⟶ H_2 + AgS

+ ⟶ + AgS

hydrogen sulfide + silver ⟶ hydrogen + AgS

Construct the equilibrium constant, K, expression for: H_2S + Ag ⟶ H_2 + AgS 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: H_2S + Ag ⟶ H_2 + AgS 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_2S | 1 | -1 Ag | 1 | -1 H_2 | 1 | 1 AgS | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2S | 1 | -1 | ([H2S])^(-1) Ag | 1 | -1 | ([Ag])^(-1) H_2 | 1 | 1 | [H2] AgS | 1 | 1 | [AgS] 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 = ([H2S])^(-1) ([Ag])^(-1) [H2] [AgS] = ([H2] [AgS])/([H2S] [Ag])

Construct the rate of reaction expression for: H_2S + Ag ⟶ H_2 + AgS 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: H_2S + Ag ⟶ H_2 + AgS 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_2S | 1 | -1 Ag | 1 | -1 H_2 | 1 | 1 AgS | 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 H_2S | 1 | -1 | -(Δ[H2S])/(Δt) Ag | 1 | -1 | -(Δ[Ag])/(Δt) H_2 | 1 | 1 | (Δ[H2])/(Δt) AgS | 1 | 1 | (Δ[AgS])/(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[H2S])/(Δt) = -(Δ[Ag])/(Δt) = (Δ[H2])/(Δt) = (Δ[AgS])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen sulfide | silver | hydrogen | AgS formula | H_2S | Ag | H_2 | AgS name | hydrogen sulfide | silver | hydrogen | IUPAC name | hydrogen sulfide | silver | molecular hydrogen |

| hydrogen sulfide | silver | hydrogen | AgS molar mass | 34.08 g/mol | 107.8682 g/mol | 2.016 g/mol | 139.93 g/mol phase | gas (at STP) | solid (at STP) | gas (at STP) | melting point | -85 °C | 960 °C | -259.2 °C | boiling point | -60 °C | 2212 °C | -252.8 °C | density | 0.001393 g/cm^3 (at 25 °C) | 10.49 g/cm^3 | 8.99×10^-5 g/cm^3 (at 0 °C) | solubility in water | | insoluble | | dynamic viscosity | 1.239×10^-5 Pa s (at 25 °C) | | 8.9×10^-6 Pa s (at 25 °C) | odor | | | odorless |