Zn + FeSO4 = Fe + Zn(SO4)2

Zn zinc + FeSO_4 duretter ⟶ Fe iron + Zn(SO4)2

Balance the chemical equation algebraically: Zn + FeSO_4 ⟶ Fe + Zn(SO4)2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Zn + c_2 FeSO_4 ⟶ c_3 Fe + c_4 Zn(SO4)2 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 = c_4 Fe: | c_2 = c_3 O: | 4 c_2 = 8 c_4 S: | 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: | | Zn + 2 FeSO_4 ⟶ 2 Fe + Zn(SO4)2

+ ⟶ + Zn(SO4)2

zinc + duretter ⟶ iron + Zn(SO4)2

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

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

| zinc | duretter | iron | Zn(SO4)2 formula | Zn | FeSO_4 | Fe | Zn(SO4)2 Hill formula | Zn | FeO_4S | Fe | O8S2Zn name | zinc | duretter | iron | IUPAC name | zinc | iron(+2) cation sulfate | iron |

| zinc | duretter | iron | Zn(SO4)2 molar mass | 65.38 g/mol | 151.9 g/mol | 55.845 g/mol | 257.5 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 | | |