Fe + AgNO3 = Ag + Fe(NO3)3

Fe iron + AgNO_3 silver nitrate ⟶ Ag silver + Fe(NO_3)_3 ferric nitrate

Balance the chemical equation algebraically: Fe + AgNO_3 ⟶ Ag + Fe(NO_3)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe + c_2 AgNO_3 ⟶ c_3 Ag + c_4 Fe(NO_3)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, Ag, N and O: Fe: | c_1 = c_4 Ag: | c_2 = c_3 N: | c_2 = 3 c_4 O: | 3 c_2 = 9 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 = 3 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe + 3 AgNO_3 ⟶ 3 Ag + Fe(NO_3)_3

+ ⟶ +

iron + silver nitrate ⟶ silver + ferric nitrate

Construct the equilibrium constant, K, expression for: Fe + AgNO_3 ⟶ Ag + Fe(NO_3)_3 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 + 3 AgNO_3 ⟶ 3 Ag + Fe(NO_3)_3 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 AgNO_3 | 3 | -3 Ag | 3 | 3 Fe(NO_3)_3 | 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) AgNO_3 | 3 | -3 | ([AgNO3])^(-3) Ag | 3 | 3 | ([Ag])^3 Fe(NO_3)_3 | 1 | 1 | [Fe(NO3)3] 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) ([AgNO3])^(-3) ([Ag])^3 [Fe(NO3)3] = (([Ag])^3 [Fe(NO3)3])/([Fe] ([AgNO3])^3)

Construct the rate of reaction expression for: Fe + AgNO_3 ⟶ Ag + Fe(NO_3)_3 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 + 3 AgNO_3 ⟶ 3 Ag + Fe(NO_3)_3 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 AgNO_3 | 3 | -3 Ag | 3 | 3 Fe(NO_3)_3 | 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) AgNO_3 | 3 | -3 | -1/3 (Δ[AgNO3])/(Δt) Ag | 3 | 3 | 1/3 (Δ[Ag])/(Δt) Fe(NO_3)_3 | 1 | 1 | (Δ[Fe(NO3)3])/(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) = -1/3 (Δ[AgNO3])/(Δt) = 1/3 (Δ[Ag])/(Δt) = (Δ[Fe(NO3)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| iron | silver nitrate | silver | ferric nitrate formula | Fe | AgNO_3 | Ag | Fe(NO_3)_3 Hill formula | Fe | AgNO_3 | Ag | FeN_3O_9 name | iron | silver nitrate | silver | ferric nitrate IUPAC name | iron | silver nitrate | silver | iron(+3) cation trinitrate

| iron | silver nitrate | silver | ferric nitrate molar mass | 55.845 g/mol | 169.87 g/mol | 107.8682 g/mol | 241.86 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 1535 °C | 212 °C | 960 °C | 35 °C boiling point | 2750 °C | | 2212 °C | density | 7.874 g/cm^3 | | 10.49 g/cm^3 | 1.7 g/cm^3 solubility in water | insoluble | soluble | insoluble | very soluble odor | | odorless | |