CO2 + ZnO = ZnCO3

CO_2 carbon dioxide + ZnO zinc oxide ⟶ ZnCO_3 zinc carbonate

Balance the chemical equation algebraically: CO_2 + ZnO ⟶ ZnCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CO_2 + c_2 ZnO ⟶ c_3 ZnCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for C, O and Zn: C: | c_1 = c_3 O: | 2 c_1 + c_2 = 3 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: | | CO_2 + ZnO ⟶ ZnCO_3

+ ⟶

carbon dioxide + zinc oxide ⟶ zinc carbonate

Construct the equilibrium constant, K, expression for: CO_2 + ZnO ⟶ 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: CO_2 + ZnO ⟶ 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 CO_2 | 1 | -1 ZnO | 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 CO_2 | 1 | -1 | ([CO2])^(-1) ZnO | 1 | -1 | ([ZnO])^(-1) 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 = ([CO2])^(-1) ([ZnO])^(-1) [ZnCO3] = ([ZnCO3])/([CO2] [ZnO])

Construct the rate of reaction expression for: CO_2 + ZnO ⟶ 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: CO_2 + ZnO ⟶ 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 CO_2 | 1 | -1 ZnO | 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 CO_2 | 1 | -1 | -(Δ[CO2])/(Δt) ZnO | 1 | -1 | -(Δ[ZnO])/(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[CO2])/(Δt) = -(Δ[ZnO])/(Δt) = (Δ[ZnCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| carbon dioxide | zinc oxide | zinc carbonate formula | CO_2 | ZnO | ZnCO_3 Hill formula | CO_2 | OZn | CO_3Zn name | carbon dioxide | zinc oxide | zinc carbonate IUPAC name | carbon dioxide | oxozinc | zinc carbonate

| carbon dioxide | zinc oxide | zinc carbonate molar mass | 44.009 g/mol | 81.38 g/mol | 125.4 g/mol phase | gas (at STP) | solid (at STP) | melting point | -56.56 °C (at triple point) | 1975 °C | boiling point | -78.5 °C (at sublimation point) | 2360 °C | density | 0.00184212 g/cm^3 (at 20 °C) | 5.6 g/cm^3 | 4.3476 g/cm^3 solubility in water | | | insoluble dynamic viscosity | 1.491×10^-5 Pa s (at 25 °C) | | odor | odorless | odorless |