CuO + C16H34 = H2O + CO2 + Cu

CuO cupric oxide + CH_3(CH_2)_14CH_3 N-hexadecane ⟶ H_2O water + CO_2 carbon dioxide + Cu copper

Balance the chemical equation algebraically: CuO + CH_3(CH_2)_14CH_3 ⟶ H_2O + CO_2 + Cu Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CuO + c_2 CH_3(CH_2)_14CH_3 ⟶ c_3 H_2O + c_4 CO_2 + c_5 Cu Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, O, C and H: Cu: | c_1 = c_5 O: | c_1 = c_3 + 2 c_4 C: | 16 c_2 = c_4 H: | 34 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_1 = 49 c_2 = 1 c_3 = 17 c_4 = 16 c_5 = 49 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 49 CuO + CH_3(CH_2)_14CH_3 ⟶ 17 H_2O + 16 CO_2 + 49 Cu

+ ⟶ + +

cupric oxide + N-hexadecane ⟶ water + carbon dioxide + copper

Construct the equilibrium constant, K, expression for: CuO + CH_3(CH_2)_14CH_3 ⟶ H_2O + CO_2 + Cu 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: 49 CuO + CH_3(CH_2)_14CH_3 ⟶ 17 H_2O + 16 CO_2 + 49 Cu 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 CuO | 49 | -49 CH_3(CH_2)_14CH_3 | 1 | -1 H_2O | 17 | 17 CO_2 | 16 | 16 Cu | 49 | 49 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CuO | 49 | -49 | ([CuO])^(-49) CH_3(CH_2)_14CH_3 | 1 | -1 | ([CH3(CH2)14CH3])^(-1) H_2O | 17 | 17 | ([H2O])^17 CO_2 | 16 | 16 | ([CO2])^16 Cu | 49 | 49 | ([Cu])^49 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 = ([CuO])^(-49) ([CH3(CH2)14CH3])^(-1) ([H2O])^17 ([CO2])^16 ([Cu])^49 = (([H2O])^17 ([CO2])^16 ([Cu])^49)/(([CuO])^49 [CH3(CH2)14CH3])

Construct the rate of reaction expression for: CuO + CH_3(CH_2)_14CH_3 ⟶ H_2O + CO_2 + Cu 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: 49 CuO + CH_3(CH_2)_14CH_3 ⟶ 17 H_2O + 16 CO_2 + 49 Cu 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 CuO | 49 | -49 CH_3(CH_2)_14CH_3 | 1 | -1 H_2O | 17 | 17 CO_2 | 16 | 16 Cu | 49 | 49 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 CuO | 49 | -49 | -1/49 (Δ[CuO])/(Δt) CH_3(CH_2)_14CH_3 | 1 | -1 | -(Δ[CH3(CH2)14CH3])/(Δt) H_2O | 17 | 17 | 1/17 (Δ[H2O])/(Δt) CO_2 | 16 | 16 | 1/16 (Δ[CO2])/(Δt) Cu | 49 | 49 | 1/49 (Δ[Cu])/(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 = -1/49 (Δ[CuO])/(Δt) = -(Δ[CH3(CH2)14CH3])/(Δt) = 1/17 (Δ[H2O])/(Δt) = 1/16 (Δ[CO2])/(Δt) = 1/49 (Δ[Cu])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| cupric oxide | N-hexadecane | water | carbon dioxide | copper formula | CuO | CH_3(CH_2)_14CH_3 | H_2O | CO_2 | Cu Hill formula | CuO | C_16H_34 | H_2O | CO_2 | Cu name | cupric oxide | N-hexadecane | water | carbon dioxide | copper IUPAC name | | hexadecane | water | carbon dioxide | copper