ZnSO4 + Pb = Zn + PbSO4

ZnSO_4 zinc sulfate + Pb lead ⟶ Zn zinc + PbSO_4 lead(II) sulfate

Balance the chemical equation algebraically: ZnSO_4 + Pb ⟶ Zn + PbSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 ZnSO_4 + c_2 Pb ⟶ c_3 Zn + c_4 PbSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for O, S, Zn and Pb: O: | 4 c_1 = 4 c_4 S: | c_1 = c_4 Zn: | c_1 = c_3 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: | | ZnSO_4 + Pb ⟶ Zn + PbSO_4

+ ⟶ +

zinc sulfate + lead ⟶ zinc + lead(II) sulfate

Construct the equilibrium constant, K, expression for: ZnSO_4 + Pb ⟶ Zn + 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: ZnSO_4 + Pb ⟶ Zn + 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 ZnSO_4 | 1 | -1 Pb | 1 | -1 Zn | 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 ZnSO_4 | 1 | -1 | ([ZnSO4])^(-1) Pb | 1 | -1 | ([Pb])^(-1) Zn | 1 | 1 | [Zn] 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 = ([ZnSO4])^(-1) ([Pb])^(-1) [Zn] [PbSO4] = ([Zn] [PbSO4])/([ZnSO4] [Pb])

Construct the rate of reaction expression for: ZnSO_4 + Pb ⟶ Zn + 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: ZnSO_4 + Pb ⟶ Zn + 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 ZnSO_4 | 1 | -1 Pb | 1 | -1 Zn | 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 ZnSO_4 | 1 | -1 | -(Δ[ZnSO4])/(Δt) Pb | 1 | -1 | -(Δ[Pb])/(Δt) Zn | 1 | 1 | (Δ[Zn])/(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[ZnSO4])/(Δt) = -(Δ[Pb])/(Δt) = (Δ[Zn])/(Δt) = (Δ[PbSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| zinc sulfate | lead | zinc | lead(II) sulfate formula | ZnSO_4 | Pb | Zn | PbSO_4 Hill formula | O_4SZn | Pb | Zn | O_4PbS name | zinc sulfate | lead | zinc | lead(II) sulfate

| zinc sulfate | lead | zinc | lead(II) sulfate molar mass | 161.4 g/mol | 207.2 g/mol | 65.38 g/mol | 303.3 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 327.4 °C | 420 °C | 1087 °C boiling point | | 1740 °C | 907 °C | density | 1.005 g/cm^3 | 11.34 g/cm^3 | 7.14 g/cm^3 | 6.29 g/cm^3 solubility in water | soluble | insoluble | insoluble | slightly soluble dynamic viscosity | | 0.00183 Pa s (at 38 °C) | | odor | odorless | | odorless |