CO + AgO = CO2 + Ag

CO carbon monoxide + AgO silver(II) oxide ⟶ CO_2 carbon dioxide + Ag silver

Balance the chemical equation algebraically: CO + AgO ⟶ CO_2 + Ag Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CO + c_2 AgO ⟶ c_3 CO_2 + c_4 Ag Set the number of atoms in the reactants equal to the number of atoms in the products for C, O and Ag: C: | c_1 = c_3 O: | c_1 + c_2 = 2 c_3 Ag: | 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_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: | | CO + AgO ⟶ CO_2 + Ag

+ ⟶ +

carbon monoxide + silver(II) oxide ⟶ carbon dioxide + silver

| carbon monoxide | silver(II) oxide | carbon dioxide | silver molecular enthalpy | -110.5 kJ/mol | -24.3 kJ/mol | -393.5 kJ/mol | 0 kJ/mol total enthalpy | -110.5 kJ/mol | -24.3 kJ/mol | -393.5 kJ/mol | 0 kJ/mol | H_initial = -134.8 kJ/mol | | H_final = -393.5 kJ/mol | ΔH_rxn^0 | -393.5 kJ/mol - -134.8 kJ/mol = -258.7 kJ/mol (exothermic) | | |

| carbon monoxide | silver(II) oxide | carbon dioxide | silver molecular entropy | 198 J/(mol K) | 117 J/(mol K) | 214 J/(mol K) | 42.6 J/(mol K) total entropy | 198 J/(mol K) | 117 J/(mol K) | 214 J/(mol K) | 42.6 J/(mol K) | S_initial = 315 J/(mol K) | | S_final = 256.6 J/(mol K) | ΔS_rxn^0 | 256.6 J/(mol K) - 315 J/(mol K) = -58.4 J/(mol K) (exoentropic) | | |

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

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

| carbon monoxide | silver(II) oxide | carbon dioxide | silver formula | CO | AgO | CO_2 | Ag name | carbon monoxide | silver(II) oxide | carbon dioxide | silver IUPAC name | carbon monoxide | oxosilver | carbon dioxide | silver