Cu + ZnSO4 = ZnSO4Cu

Cu copper + ZnSO_4 zinc sulfate ⟶ ZnSO4Cu

Balance the chemical equation algebraically: Cu + ZnSO_4 ⟶ ZnSO4Cu Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cu + c_2 ZnSO_4 ⟶ c_3 ZnSO4Cu Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, O, S and Zn: Cu: | c_1 = c_3 O: | 4 c_2 = 4 c_3 S: | c_2 = c_3 Zn: | c_2 = c_3 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Cu + ZnSO_4 ⟶ ZnSO4Cu

+ ⟶ ZnSO4Cu

copper + zinc sulfate ⟶ ZnSO4Cu

Construct the equilibrium constant, K, expression for: Cu + ZnSO_4 ⟶ ZnSO4Cu 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: Cu + ZnSO_4 ⟶ ZnSO4Cu 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 Cu | 1 | -1 ZnSO_4 | 1 | -1 ZnSO4Cu | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cu | 1 | -1 | ([Cu])^(-1) ZnSO_4 | 1 | -1 | ([ZnSO4])^(-1) ZnSO4Cu | 1 | 1 | [ZnSO4Cu] 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 = ([Cu])^(-1) ([ZnSO4])^(-1) [ZnSO4Cu] = ([ZnSO4Cu])/([Cu] [ZnSO4])

Construct the rate of reaction expression for: Cu + ZnSO_4 ⟶ ZnSO4Cu 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: Cu + ZnSO_4 ⟶ ZnSO4Cu 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 Cu | 1 | -1 ZnSO_4 | 1 | -1 ZnSO4Cu | 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 Cu | 1 | -1 | -(Δ[Cu])/(Δt) ZnSO_4 | 1 | -1 | -(Δ[ZnSO4])/(Δt) ZnSO4Cu | 1 | 1 | (Δ[ZnSO4Cu])/(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[Cu])/(Δt) = -(Δ[ZnSO4])/(Δt) = (Δ[ZnSO4Cu])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| copper | zinc sulfate | ZnSO4Cu formula | Cu | ZnSO_4 | ZnSO4Cu Hill formula | Cu | O_4SZn | CuO4SZn name | copper | zinc sulfate |

| copper | zinc sulfate | ZnSO4Cu molar mass | 63.546 g/mol | 161.4 g/mol | 225 g/mol phase | solid (at STP) | | melting point | 1083 °C | | boiling point | 2567 °C | | density | 8.96 g/cm^3 | 1.005 g/cm^3 | solubility in water | insoluble | soluble | odor | odorless | odorless |