O2 + C4H9OH = H2O + C + CO

O_2 oxygen + CH_3(CH_2)_3OH 1-butanol ⟶ H_2O water + C activated charcoal + CO carbon monoxide

Balance the chemical equation algebraically: O_2 + CH_3(CH_2)_3OH ⟶ H_2O + C + CO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 CH_3(CH_2)_3OH ⟶ c_3 H_2O + c_4 C + c_5 CO Set the number of atoms in the reactants equal to the number of atoms in the products for O, C and H: O: | 2 c_1 + c_2 = c_3 + c_5 C: | 4 c_2 = c_4 + c_5 H: | 10 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_2 = 1 and solve the system of equations for the remaining coefficients: c_2 = 1 c_3 = 5 c_4 = 8 - 2 c_1 c_5 = 2 c_1 - 4 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 3 and solve for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 5 c_4 = 2 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 O_2 + CH_3(CH_2)_3OH ⟶ 5 H_2O + 2 C + 2 CO

+ ⟶ + +

oxygen + 1-butanol ⟶ water + activated charcoal + carbon monoxide

Construct the equilibrium constant, K, expression for: O_2 + CH_3(CH_2)_3OH ⟶ H_2O + C + CO 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: 3 O_2 + CH_3(CH_2)_3OH ⟶ 5 H_2O + 2 C + 2 CO 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 O_2 | 3 | -3 CH_3(CH_2)_3OH | 1 | -1 H_2O | 5 | 5 C | 2 | 2 CO | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 3 | -3 | ([O2])^(-3) CH_3(CH_2)_3OH | 1 | -1 | ([CH3(CH2)3OH])^(-1) H_2O | 5 | 5 | ([H2O])^5 C | 2 | 2 | ([C])^2 CO | 2 | 2 | ([CO])^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 = ([O2])^(-3) ([CH3(CH2)3OH])^(-1) ([H2O])^5 ([C])^2 ([CO])^2 = (([H2O])^5 ([C])^2 ([CO])^2)/(([O2])^3 [CH3(CH2)3OH])

Construct the rate of reaction expression for: O_2 + CH_3(CH_2)_3OH ⟶ H_2O + C + CO 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: 3 O_2 + CH_3(CH_2)_3OH ⟶ 5 H_2O + 2 C + 2 CO 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 O_2 | 3 | -3 CH_3(CH_2)_3OH | 1 | -1 H_2O | 5 | 5 C | 2 | 2 CO | 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 O_2 | 3 | -3 | -1/3 (Δ[O2])/(Δt) CH_3(CH_2)_3OH | 1 | -1 | -(Δ[CH3(CH2)3OH])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) C | 2 | 2 | 1/2 (Δ[C])/(Δt) CO | 2 | 2 | 1/2 (Δ[CO])/(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 = -1/3 (Δ[O2])/(Δt) = -(Δ[CH3(CH2)3OH])/(Δt) = 1/5 (Δ[H2O])/(Δt) = 1/2 (Δ[C])/(Δt) = 1/2 (Δ[CO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| oxygen | 1-butanol | water | activated charcoal | carbon monoxide formula | O_2 | CH_3(CH_2)_3OH | H_2O | C | CO Hill formula | O_2 | C_4H_10O | H_2O | C | CO name | oxygen | 1-butanol | water | activated charcoal | carbon monoxide IUPAC name | molecular oxygen | butan-1-ol | water | carbon | carbon monoxide