CH3CH2OH + Na2O2 = H2O + CO2 + Na2O

CH_3CH_2OH ethanol + Na_2O_2 sodium peroxide ⟶ H_2O water + CO_2 carbon dioxide + Na_2O sodium oxide

Balance the chemical equation algebraically: CH_3CH_2OH + Na_2O_2 ⟶ H_2O + CO_2 + Na_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CH_3CH_2OH + c_2 Na_2O_2 ⟶ c_3 H_2O + c_4 CO_2 + c_5 Na_2O Set the number of atoms in the reactants equal to the number of atoms in the products for C, H, O and Na: C: | 2 c_1 = c_4 H: | 6 c_1 = 2 c_3 O: | c_1 + 2 c_2 = c_3 + 2 c_4 + c_5 Na: | 2 c_2 = 2 c_5 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 = 6 c_3 = 3 c_4 = 2 c_5 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CH_3CH_2OH + 6 Na_2O_2 ⟶ 3 H_2O + 2 CO_2 + 6 Na_2O

+ ⟶ + +

ethanol + sodium peroxide ⟶ water + carbon dioxide + sodium oxide

Construct the equilibrium constant, K, expression for: CH_3CH_2OH + Na_2O_2 ⟶ H_2O + CO_2 + Na_2O 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: CH_3CH_2OH + 6 Na_2O_2 ⟶ 3 H_2O + 2 CO_2 + 6 Na_2O 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 CH_3CH_2OH | 1 | -1 Na_2O_2 | 6 | -6 H_2O | 3 | 3 CO_2 | 2 | 2 Na_2O | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CH_3CH_2OH | 1 | -1 | ([CH3CH2OH])^(-1) Na_2O_2 | 6 | -6 | ([Na2O2])^(-6) H_2O | 3 | 3 | ([H2O])^3 CO_2 | 2 | 2 | ([CO2])^2 Na_2O | 6 | 6 | ([Na2O])^6 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 = ([CH3CH2OH])^(-1) ([Na2O2])^(-6) ([H2O])^3 ([CO2])^2 ([Na2O])^6 = (([H2O])^3 ([CO2])^2 ([Na2O])^6)/([CH3CH2OH] ([Na2O2])^6)

Construct the rate of reaction expression for: CH_3CH_2OH + Na_2O_2 ⟶ H_2O + CO_2 + Na_2O 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: CH_3CH_2OH + 6 Na_2O_2 ⟶ 3 H_2O + 2 CO_2 + 6 Na_2O 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 CH_3CH_2OH | 1 | -1 Na_2O_2 | 6 | -6 H_2O | 3 | 3 CO_2 | 2 | 2 Na_2O | 6 | 6 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 CH_3CH_2OH | 1 | -1 | -(Δ[CH3CH2OH])/(Δt) Na_2O_2 | 6 | -6 | -1/6 (Δ[Na2O2])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) CO_2 | 2 | 2 | 1/2 (Δ[CO2])/(Δt) Na_2O | 6 | 6 | 1/6 (Δ[Na2O])/(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[CH3CH2OH])/(Δt) = -1/6 (Δ[Na2O2])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/2 (Δ[CO2])/(Δt) = 1/6 (Δ[Na2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| ethanol | sodium peroxide | water | carbon dioxide | sodium oxide formula | CH_3CH_2OH | Na_2O_2 | H_2O | CO_2 | Na_2O Hill formula | C_2H_6O | Na_2O_2 | H_2O | CO_2 | Na_2O name | ethanol | sodium peroxide | water | carbon dioxide | sodium oxide IUPAC name | ethanol | disodium peroxide | water | carbon dioxide | disodium oxygen(-2) anion