CO2 + Pb2O2 = O2 + PbCO2

CO_2 carbon dioxide + Pb2O2 ⟶ O_2 oxygen + PbCO2

Balance the chemical equation algebraically: CO_2 + Pb2O2 ⟶ O_2 + PbCO2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CO_2 + c_2 Pb2O2 ⟶ c_3 O_2 + c_4 PbCO2 Set the number of atoms in the reactants equal to the number of atoms in the products for C, O and Pb: C: | c_1 = c_4 O: | 2 c_1 + 2 c_2 = 2 c_3 + 2 c_4 Pb: | 2 c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 CO_2 + Pb2O2 ⟶ O_2 + 2 PbCO2

+ Pb2O2 ⟶ + PbCO2

carbon dioxide + Pb2O2 ⟶ oxygen + PbCO2

Construct the equilibrium constant, K, expression for: CO_2 + Pb2O2 ⟶ O_2 + PbCO2 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: 2 CO_2 + Pb2O2 ⟶ O_2 + 2 PbCO2 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 | 2 | -2 Pb2O2 | 1 | -1 O_2 | 1 | 1 PbCO2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CO_2 | 2 | -2 | ([CO2])^(-2) Pb2O2 | 1 | -1 | ([Pb2O2])^(-1) O_2 | 1 | 1 | [O2] PbCO2 | 2 | 2 | ([PbCO2])^2 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])^(-2) ([Pb2O2])^(-1) [O2] ([PbCO2])^2 = ([O2] ([PbCO2])^2)/(([CO2])^2 [Pb2O2])

Construct the rate of reaction expression for: CO_2 + Pb2O2 ⟶ O_2 + PbCO2 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: 2 CO_2 + Pb2O2 ⟶ O_2 + 2 PbCO2 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 | 2 | -2 Pb2O2 | 1 | -1 O_2 | 1 | 1 PbCO2 | 2 | 2 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 | 2 | -2 | -1/2 (Δ[CO2])/(Δt) Pb2O2 | 1 | -1 | -(Δ[Pb2O2])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) PbCO2 | 2 | 2 | 1/2 (Δ[PbCO2])/(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 = -1/2 (Δ[CO2])/(Δt) = -(Δ[Pb2O2])/(Δt) = (Δ[O2])/(Δt) = 1/2 (Δ[PbCO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| carbon dioxide | Pb2O2 | oxygen | PbCO2 formula | CO_2 | Pb2O2 | O_2 | PbCO2 Hill formula | CO_2 | O2Pb2 | O_2 | CO2Pb name | carbon dioxide | | oxygen | IUPAC name | carbon dioxide | | molecular oxygen |

| carbon dioxide | Pb2O2 | oxygen | PbCO2 molar mass | 44.009 g/mol | 446.4 g/mol | 31.998 g/mol | 251.2 g/mol phase | gas (at STP) | | gas (at STP) | melting point | -56.56 °C (at triple point) | | -218 °C | boiling point | -78.5 °C (at sublimation point) | | -183 °C | density | 0.00184212 g/cm^3 (at 20 °C) | | 0.001429 g/cm^3 (at 0 °C) | surface tension | | | 0.01347 N/m | dynamic viscosity | 1.491×10^-5 Pa s (at 25 °C) | | 2.055×10^-5 Pa s (at 25 °C) | odor | odorless | | odorless |