Zn + FeSO4 = Fe + Zn2(SO4)3

Zn zinc + FeSO_4 duretter ⟶ Fe iron + Zn2(SO4)3

Balance the chemical equation algebraically: Zn + FeSO_4 ⟶ Fe + Zn2(SO4)3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Zn + c_2 FeSO_4 ⟶ c_3 Fe + c_4 Zn2(SO4)3 Set the number of atoms in the reactants equal to the number of atoms in the products for Zn, Fe, O and S: Zn: | c_1 = 2 c_4 Fe: | c_2 = c_3 O: | 4 c_2 = 12 c_4 S: | c_2 = 3 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Zn + 3 FeSO_4 ⟶ 3 Fe + Zn2(SO4)3

+ ⟶ + Zn2(SO4)3

zinc + duretter ⟶ iron + Zn2(SO4)3

Construct the equilibrium constant, K, expression for: Zn + FeSO_4 ⟶ Fe + Zn2(SO4)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: 2 Zn + 3 FeSO_4 ⟶ 3 Fe + Zn2(SO4)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 Zn | 2 | -2 FeSO_4 | 3 | -3 Fe | 3 | 3 Zn2(SO4)3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Zn | 2 | -2 | ([Zn])^(-2) FeSO_4 | 3 | -3 | ([FeSO4])^(-3) Fe | 3 | 3 | ([Fe])^3 Zn2(SO4)3 | 1 | 1 | [Zn2(SO4)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 = ([Zn])^(-2) ([FeSO4])^(-3) ([Fe])^3 [Zn2(SO4)3] = (([Fe])^3 [Zn2(SO4)3])/(([Zn])^2 ([FeSO4])^3)

Construct the rate of reaction expression for: Zn + FeSO_4 ⟶ Fe + Zn2(SO4)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: 2 Zn + 3 FeSO_4 ⟶ 3 Fe + Zn2(SO4)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 Zn | 2 | -2 FeSO_4 | 3 | -3 Fe | 3 | 3 Zn2(SO4)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 Zn | 2 | -2 | -1/2 (Δ[Zn])/(Δt) FeSO_4 | 3 | -3 | -1/3 (Δ[FeSO4])/(Δt) Fe | 3 | 3 | 1/3 (Δ[Fe])/(Δt) Zn2(SO4)3 | 1 | 1 | (Δ[Zn2(SO4)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 = -1/2 (Δ[Zn])/(Δt) = -1/3 (Δ[FeSO4])/(Δt) = 1/3 (Δ[Fe])/(Δt) = (Δ[Zn2(SO4)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| zinc | duretter | iron | Zn2(SO4)3 formula | Zn | FeSO_4 | Fe | Zn2(SO4)3 Hill formula | Zn | FeO_4S | Fe | O12S3Zn2 name | zinc | duretter | iron | IUPAC name | zinc | iron(+2) cation sulfate | iron |

| zinc | duretter | iron | Zn2(SO4)3 molar mass | 65.38 g/mol | 151.9 g/mol | 55.845 g/mol | 418.9 g/mol phase | solid (at STP) | | solid (at STP) | melting point | 420 °C | | 1535 °C | boiling point | 907 °C | | 2750 °C | density | 7.14 g/cm^3 | 2.841 g/cm^3 | 7.874 g/cm^3 | solubility in water | insoluble | | insoluble | odor | odorless | | |