Zn + CuCO3 = Cu + ZnCO3

Zn zinc + CuCO_3 copper(II) carbonate ⟶ Cu copper + ZnCO_3 zinc carbonate

Balance the chemical equation algebraically: Zn + CuCO_3 ⟶ Cu + ZnCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Zn + c_2 CuCO_3 ⟶ c_3 Cu + c_4 ZnCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Zn, C, Cu and O: Zn: | c_1 = c_4 C: | c_2 = c_4 Cu: | c_2 = c_3 O: | 3 c_2 = 3 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: | | Zn + CuCO_3 ⟶ Cu + ZnCO_3

+ ⟶ +

zinc + copper(II) carbonate ⟶ copper + zinc carbonate

Construct the equilibrium constant, K, expression for: Zn + CuCO_3 ⟶ Cu + ZnCO_3 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 + CuCO_3 ⟶ Cu + ZnCO_3 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 CuCO_3 | 1 | -1 Cu | 1 | 1 ZnCO_3 | 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) CuCO_3 | 1 | -1 | ([CuCO3])^(-1) Cu | 1 | 1 | [Cu] ZnCO_3 | 1 | 1 | [ZnCO3] 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) ([CuCO3])^(-1) [Cu] [ZnCO3] = ([Cu] [ZnCO3])/([Zn] [CuCO3])

Construct the rate of reaction expression for: Zn + CuCO_3 ⟶ Cu + ZnCO_3 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 + CuCO_3 ⟶ Cu + ZnCO_3 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 CuCO_3 | 1 | -1 Cu | 1 | 1 ZnCO_3 | 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) CuCO_3 | 1 | -1 | -(Δ[CuCO3])/(Δt) Cu | 1 | 1 | (Δ[Cu])/(Δt) ZnCO_3 | 1 | 1 | (Δ[ZnCO3])/(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[CuCO3])/(Δt) = (Δ[Cu])/(Δt) = (Δ[ZnCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| zinc | copper(II) carbonate | copper | zinc carbonate formula | Zn | CuCO_3 | Cu | ZnCO_3 Hill formula | Zn | CCuO_3 | Cu | CO_3Zn name | zinc | copper(II) carbonate | copper | zinc carbonate IUPAC name | zinc | copper carbonate | copper | zinc carbonate

| zinc | copper(II) carbonate | copper | zinc carbonate molar mass | 65.38 g/mol | 123.55 g/mol | 63.546 g/mol | 125.4 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 420 °C | 200 °C | 1083 °C | boiling point | 907 °C | | 2567 °C | density | 7.14 g/cm^3 | | 8.96 g/cm^3 | 4.3476 g/cm^3 solubility in water | insoluble | | insoluble | insoluble odor | odorless | | odorless |