Fe + AgF = Ag + FeF2

Fe iron + AgF silver fluoride ⟶ Ag silver + FeF_2 ferrous fluoride

Balance the chemical equation algebraically: Fe + AgF ⟶ Ag + FeF_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe + c_2 AgF ⟶ c_3 Ag + c_4 FeF_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, Ag and F: Fe: | c_1 = c_4 Ag: | c_2 = c_3 F: | c_2 = 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 = 2 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe + 2 AgF ⟶ 2 Ag + FeF_2

+ ⟶ +

iron + silver fluoride ⟶ silver + ferrous fluoride

Construct the equilibrium constant, K, expression for: Fe + AgF ⟶ Ag + FeF_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: Fe + 2 AgF ⟶ 2 Ag + FeF_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 Fe | 1 | -1 AgF | 2 | -2 Ag | 2 | 2 FeF_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe | 1 | -1 | ([Fe])^(-1) AgF | 2 | -2 | ([AgF])^(-2) Ag | 2 | 2 | ([Ag])^2 FeF_2 | 1 | 1 | [FeF2] 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 = ([Fe])^(-1) ([AgF])^(-2) ([Ag])^2 [FeF2] = (([Ag])^2 [FeF2])/([Fe] ([AgF])^2)

Construct the rate of reaction expression for: Fe + AgF ⟶ Ag + FeF_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: Fe + 2 AgF ⟶ 2 Ag + FeF_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 Fe | 1 | -1 AgF | 2 | -2 Ag | 2 | 2 FeF_2 | 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 Fe | 1 | -1 | -(Δ[Fe])/(Δt) AgF | 2 | -2 | -1/2 (Δ[AgF])/(Δt) Ag | 2 | 2 | 1/2 (Δ[Ag])/(Δt) FeF_2 | 1 | 1 | (Δ[FeF2])/(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[Fe])/(Δt) = -1/2 (Δ[AgF])/(Δt) = 1/2 (Δ[Ag])/(Δt) = (Δ[FeF2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| iron | silver fluoride | silver | ferrous fluoride formula | Fe | AgF | Ag | FeF_2 Hill formula | Fe | AgF | Ag | F_2Fe name | iron | silver fluoride | silver | ferrous fluoride IUPAC name | iron | fluorosilver | silver | difluoroiron

| iron | silver fluoride | silver | ferrous fluoride molar mass | 55.845 g/mol | 126.8666 g/mol | 107.8682 g/mol | 93.842 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 1535 °C | 300 °C | 960 °C | 970 °C boiling point | 2750 °C | 1150 °C | 2212 °C | 1100 °C density | 7.874 g/cm^3 | 5.852 g/cm^3 | 10.49 g/cm^3 | 4.09 g/cm^3 solubility in water | insoluble | | insoluble |