O2 + C2H5N = H2O + CO2 + NO

O_2 oxygen + C_2H_5N aziridine ⟶ H_2O water + CO_2 carbon dioxide + NO nitric oxide

Balance the chemical equation algebraically: O_2 + C_2H_5N ⟶ H_2O + CO_2 + NO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 C_2H_5N ⟶ c_3 H_2O + c_4 CO_2 + c_5 NO Set the number of atoms in the reactants equal to the number of atoms in the products for O, C, H and N: O: | 2 c_1 = c_3 + 2 c_4 + c_5 C: | 2 c_2 = c_4 H: | 5 c_2 = 2 c_3 N: | c_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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 15/4 c_2 = 1 c_3 = 5/2 c_4 = 2 c_5 = 1 Multiply by the least common denominator, 4, to eliminate fractional coefficients: c_1 = 15 c_2 = 4 c_3 = 10 c_4 = 8 c_5 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 15 O_2 + 4 C_2H_5N ⟶ 10 H_2O + 8 CO_2 + 4 NO

+ ⟶ + +

oxygen + aziridine ⟶ water + carbon dioxide + nitric oxide

Construct the equilibrium constant, K, expression for: O_2 + C_2H_5N ⟶ H_2O + CO_2 + NO 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: 15 O_2 + 4 C_2H_5N ⟶ 10 H_2O + 8 CO_2 + 4 NO 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 | 15 | -15 C_2H_5N | 4 | -4 H_2O | 10 | 10 CO_2 | 8 | 8 NO | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 15 | -15 | ([O2])^(-15) C_2H_5N | 4 | -4 | ([C2H5N])^(-4) H_2O | 10 | 10 | ([H2O])^10 CO_2 | 8 | 8 | ([CO2])^8 NO | 4 | 4 | ([NO])^4 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])^(-15) ([C2H5N])^(-4) ([H2O])^10 ([CO2])^8 ([NO])^4 = (([H2O])^10 ([CO2])^8 ([NO])^4)/(([O2])^15 ([C2H5N])^4)

Construct the rate of reaction expression for: O_2 + C_2H_5N ⟶ H_2O + CO_2 + NO 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: 15 O_2 + 4 C_2H_5N ⟶ 10 H_2O + 8 CO_2 + 4 NO 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 | 15 | -15 C_2H_5N | 4 | -4 H_2O | 10 | 10 CO_2 | 8 | 8 NO | 4 | 4 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 | 15 | -15 | -1/15 (Δ[O2])/(Δt) C_2H_5N | 4 | -4 | -1/4 (Δ[C2H5N])/(Δt) H_2O | 10 | 10 | 1/10 (Δ[H2O])/(Δt) CO_2 | 8 | 8 | 1/8 (Δ[CO2])/(Δt) NO | 4 | 4 | 1/4 (Δ[NO])/(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 = -1/15 (Δ[O2])/(Δt) = -1/4 (Δ[C2H5N])/(Δt) = 1/10 (Δ[H2O])/(Δt) = 1/8 (Δ[CO2])/(Δt) = 1/4 (Δ[NO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| oxygen | aziridine | water | carbon dioxide | nitric oxide formula | O_2 | C_2H_5N | H_2O | CO_2 | NO name | oxygen | aziridine | water | carbon dioxide | nitric oxide IUPAC name | molecular oxygen | aziridine | water | carbon dioxide | nitric oxide