S + Ag = AgS

S mixed sulfur + Ag silver ⟶ AgS

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

+ ⟶ AgS

mixed sulfur + silver ⟶ AgS

Construct the equilibrium constant, K, expression for: S + Ag ⟶ 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: S + Ag ⟶ 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 S | 1 | -1 Ag | 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 S | 1 | -1 | ([S])^(-1) Ag | 1 | -1 | ([Ag])^(-1) 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 = ([S])^(-1) ([Ag])^(-1) [AgS] = ([AgS])/([S] [Ag])

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

| mixed sulfur | silver | AgS formula | S | Ag | AgS name | mixed sulfur | silver | IUPAC name | sulfur | silver |

| mixed sulfur | silver | AgS molar mass | 32.06 g/mol | 107.8682 g/mol | 139.93 g/mol phase | solid (at STP) | solid (at STP) | melting point | 112.8 °C | 960 °C | boiling point | 444.7 °C | 2212 °C | density | 2.07 g/cm^3 | 10.49 g/cm^3 | solubility in water | | insoluble |