CuO + Zn(NO3)2 = Cu(NO3)2 + ZnO

CuO cupric oxide + Zn(NO3)2 ⟶ Cu(NO_3)_2 copper(II) nitrate + ZnO zinc oxide

Balance the chemical equation algebraically: CuO + Zn(NO3)2 ⟶ Cu(NO_3)_2 + ZnO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CuO + c_2 Zn(NO3)2 ⟶ c_3 Cu(NO_3)_2 + c_4 ZnO Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, O, Zn and N: Cu: | c_1 = c_3 O: | c_1 + 6 c_2 = 6 c_3 + c_4 Zn: | c_2 = c_4 N: | 2 c_2 = 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 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CuO + Zn(NO3)2 ⟶ Cu(NO_3)_2 + ZnO

+ Zn(NO3)2 ⟶ +

cupric oxide + Zn(NO3)2 ⟶ copper(II) nitrate + zinc oxide

Construct the equilibrium constant, K, expression for: CuO + Zn(NO3)2 ⟶ Cu(NO_3)_2 + ZnO 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: CuO + Zn(NO3)2 ⟶ Cu(NO_3)_2 + ZnO 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 CuO | 1 | -1 Zn(NO3)2 | 1 | -1 Cu(NO_3)_2 | 1 | 1 ZnO | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CuO | 1 | -1 | ([CuO])^(-1) Zn(NO3)2 | 1 | -1 | ([Zn(NO3)2])^(-1) Cu(NO_3)_2 | 1 | 1 | [Cu(NO3)2] ZnO | 1 | 1 | [ZnO] 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 = ([CuO])^(-1) ([Zn(NO3)2])^(-1) [Cu(NO3)2] [ZnO] = ([Cu(NO3)2] [ZnO])/([CuO] [Zn(NO3)2])

Construct the rate of reaction expression for: CuO + Zn(NO3)2 ⟶ Cu(NO_3)_2 + ZnO 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: CuO + Zn(NO3)2 ⟶ Cu(NO_3)_2 + ZnO 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 CuO | 1 | -1 Zn(NO3)2 | 1 | -1 Cu(NO_3)_2 | 1 | 1 ZnO | 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 CuO | 1 | -1 | -(Δ[CuO])/(Δt) Zn(NO3)2 | 1 | -1 | -(Δ[Zn(NO3)2])/(Δt) Cu(NO_3)_2 | 1 | 1 | (Δ[Cu(NO3)2])/(Δt) ZnO | 1 | 1 | (Δ[ZnO])/(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[CuO])/(Δt) = -(Δ[Zn(NO3)2])/(Δt) = (Δ[Cu(NO3)2])/(Δt) = (Δ[ZnO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| cupric oxide | Zn(NO3)2 | copper(II) nitrate | zinc oxide formula | CuO | Zn(NO3)2 | Cu(NO_3)_2 | ZnO Hill formula | CuO | N2O6Zn | CuN_2O_6 | OZn name | cupric oxide | | copper(II) nitrate | zinc oxide IUPAC name | | | copper(II) nitrate | oxozinc

| cupric oxide | Zn(NO3)2 | copper(II) nitrate | zinc oxide molar mass | 79.545 g/mol | 189.4 g/mol | 187.55 g/mol | 81.38 g/mol phase | solid (at STP) | | | solid (at STP) melting point | 1326 °C | | | 1975 °C boiling point | 2000 °C | | | 2360 °C density | 6.315 g/cm^3 | | | 5.6 g/cm^3 solubility in water | insoluble | | | odor | | | | odorless