Zn + Cu2SO4 = Cu + ZnSO4

Zn zinc + Cu2SO4 ⟶ Cu copper + ZnSO_4 zinc sulfate

Balance the chemical equation algebraically: Zn + Cu2SO4 ⟶ Cu + ZnSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Zn + c_2 Cu2SO4 ⟶ c_3 Cu + c_4 ZnSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Zn, Cu, S and O: Zn: | c_1 = c_4 Cu: | 2 c_2 = c_3 S: | c_2 = c_4 O: | 4 c_2 = 4 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 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Zn + Cu2SO4 ⟶ 2 Cu + ZnSO_4

+ Cu2SO4 ⟶ +

zinc + Cu2SO4 ⟶ copper + zinc sulfate

Construct the equilibrium constant, K, expression for: Zn + Cu2SO4 ⟶ Cu + ZnSO_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: Zn + Cu2SO4 ⟶ 2 Cu + ZnSO_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 Zn | 1 | -1 Cu2SO4 | 1 | -1 Cu | 2 | 2 ZnSO_4 | 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) Cu2SO4 | 1 | -1 | ([Cu2SO4])^(-1) Cu | 2 | 2 | ([Cu])^2 ZnSO_4 | 1 | 1 | [ZnSO4] 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) ([Cu2SO4])^(-1) ([Cu])^2 [ZnSO4] = (([Cu])^2 [ZnSO4])/([Zn] [Cu2SO4])

Construct the rate of reaction expression for: Zn + Cu2SO4 ⟶ Cu + ZnSO_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: Zn + Cu2SO4 ⟶ 2 Cu + ZnSO_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 Zn | 1 | -1 Cu2SO4 | 1 | -1 Cu | 2 | 2 ZnSO_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 Zn | 1 | -1 | -(Δ[Zn])/(Δt) Cu2SO4 | 1 | -1 | -(Δ[Cu2SO4])/(Δt) Cu | 2 | 2 | 1/2 (Δ[Cu])/(Δt) ZnSO_4 | 1 | 1 | (Δ[ZnSO4])/(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) = -(Δ[Cu2SO4])/(Δt) = 1/2 (Δ[Cu])/(Δt) = (Δ[ZnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| zinc | Cu2SO4 | copper | zinc sulfate formula | Zn | Cu2SO4 | Cu | ZnSO_4 Hill formula | Zn | Cu2O4S | Cu | O_4SZn name | zinc | | copper | zinc sulfate

| zinc | Cu2SO4 | copper | zinc sulfate molar mass | 65.38 g/mol | 223.15 g/mol | 63.546 g/mol | 161.4 g/mol phase | solid (at STP) | | solid (at STP) | melting point | 420 °C | | 1083 °C | boiling point | 907 °C | | 2567 °C | density | 7.14 g/cm^3 | | 8.96 g/cm^3 | 1.005 g/cm^3 solubility in water | insoluble | | insoluble | soluble odor | odorless | | odorless | odorless