FeSO4 + Pb = Fe + PbSO4

FeSO_4 duretter + Pb lead ⟶ Fe iron + PbSO_4 lead(II) sulfate

Balance the chemical equation algebraically: FeSO_4 + Pb ⟶ Fe + PbSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 FeSO_4 + c_2 Pb ⟶ c_3 Fe + c_4 PbSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S and Pb: Fe: | c_1 = c_3 O: | 4 c_1 = 4 c_4 S: | c_1 = c_4 Pb: | c_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 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | FeSO_4 + Pb ⟶ Fe + PbSO_4

+ ⟶ +

duretter + lead ⟶ iron + lead(II) sulfate

Construct the equilibrium constant, K, expression for: FeSO_4 + Pb ⟶ Fe + PbSO_4 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: FeSO_4 + Pb ⟶ Fe + PbSO_4 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 FeSO_4 | 1 | -1 Pb | 1 | -1 Fe | 1 | 1 PbSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression FeSO_4 | 1 | -1 | ([FeSO4])^(-1) Pb | 1 | -1 | ([Pb])^(-1) Fe | 1 | 1 | [Fe] PbSO_4 | 1 | 1 | [PbSO4] 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 = ([FeSO4])^(-1) ([Pb])^(-1) [Fe] [PbSO4] = ([Fe] [PbSO4])/([FeSO4] [Pb])

Construct the rate of reaction expression for: FeSO_4 + Pb ⟶ Fe + PbSO_4 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: FeSO_4 + Pb ⟶ Fe + PbSO_4 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 FeSO_4 | 1 | -1 Pb | 1 | -1 Fe | 1 | 1 PbSO_4 | 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 FeSO_4 | 1 | -1 | -(Δ[FeSO4])/(Δt) Pb | 1 | -1 | -(Δ[Pb])/(Δt) Fe | 1 | 1 | (Δ[Fe])/(Δt) PbSO_4 | 1 | 1 | (Δ[PbSO4])/(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[FeSO4])/(Δt) = -(Δ[Pb])/(Δt) = (Δ[Fe])/(Δt) = (Δ[PbSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| duretter | lead | iron | lead(II) sulfate formula | FeSO_4 | Pb | Fe | PbSO_4 Hill formula | FeO_4S | Pb | Fe | O_4PbS name | duretter | lead | iron | lead(II) sulfate IUPAC name | iron(+2) cation sulfate | lead | iron |

| duretter | lead | iron | lead(II) sulfate molar mass | 151.9 g/mol | 207.2 g/mol | 55.845 g/mol | 303.3 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 327.4 °C | 1535 °C | 1087 °C boiling point | | 1740 °C | 2750 °C | density | 2.841 g/cm^3 | 11.34 g/cm^3 | 7.874 g/cm^3 | 6.29 g/cm^3 solubility in water | | insoluble | insoluble | slightly soluble dynamic viscosity | | 0.00183 Pa s (at 38 °C) | |