O2 + C4H10 = H2O + C

O_2 oxygen + CH_3CH_2CH_2CH_3 butane ⟶ H_2O water + C activated charcoal

Balance the chemical equation algebraically: O_2 + CH_3CH_2CH_2CH_3 ⟶ H_2O + C Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 CH_3CH_2CH_2CH_3 ⟶ c_3 H_2O + c_4 C 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_3 C: | 4 c_2 = c_4 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_1 = 5/2 c_2 = 1 c_3 = 5 c_4 = 4 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 5 c_2 = 2 c_3 = 10 c_4 = 8 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 5 O_2 + 2 CH_3CH_2CH_2CH_3 ⟶ 10 H_2O + 8 C

+ ⟶ +

oxygen + butane ⟶ water + activated charcoal

Construct the equilibrium constant, K, expression for: O_2 + CH_3CH_2CH_2CH_3 ⟶ H_2O + C 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: 5 O_2 + 2 CH_3CH_2CH_2CH_3 ⟶ 10 H_2O + 8 C 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 | 5 | -5 CH_3CH_2CH_2CH_3 | 2 | -2 H_2O | 10 | 10 C | 8 | 8 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 5 | -5 | ([O2])^(-5) CH_3CH_2CH_2CH_3 | 2 | -2 | ([CH3CH2CH2CH3])^(-2) H_2O | 10 | 10 | ([H2O])^10 C | 8 | 8 | ([C])^8 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])^(-5) ([CH3CH2CH2CH3])^(-2) ([H2O])^10 ([C])^8 = (([H2O])^10 ([C])^8)/(([O2])^5 ([CH3CH2CH2CH3])^2)

Construct the rate of reaction expression for: O_2 + CH_3CH_2CH_2CH_3 ⟶ H_2O + C 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: 5 O_2 + 2 CH_3CH_2CH_2CH_3 ⟶ 10 H_2O + 8 C 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 | 5 | -5 CH_3CH_2CH_2CH_3 | 2 | -2 H_2O | 10 | 10 C | 8 | 8 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 | 5 | -5 | -1/5 (Δ[O2])/(Δt) CH_3CH_2CH_2CH_3 | 2 | -2 | -1/2 (Δ[CH3CH2CH2CH3])/(Δt) H_2O | 10 | 10 | 1/10 (Δ[H2O])/(Δt) C | 8 | 8 | 1/8 (Δ[C])/(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 = -1/5 (Δ[O2])/(Δt) = -1/2 (Δ[CH3CH2CH2CH3])/(Δt) = 1/10 (Δ[H2O])/(Δt) = 1/8 (Δ[C])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| oxygen | butane | water | activated charcoal formula | O_2 | CH_3CH_2CH_2CH_3 | H_2O | C Hill formula | O_2 | C_4H_10 | H_2O | C name | oxygen | butane | water | activated charcoal IUPAC name | molecular oxygen | butane | water | carbon