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O2 + Cl2 + C4H10 = H2O + CO2 + CCl4

Input interpretation

O_2 oxygen + Cl_2 chlorine + CH_3CH_2CH_2CH_3 butane ⟶ H_2O water + CO_2 carbon dioxide + CCl_4 carbon tetrachloride
O_2 oxygen + Cl_2 chlorine + CH_3CH_2CH_2CH_3 butane ⟶ H_2O water + CO_2 carbon dioxide + CCl_4 carbon tetrachloride

Balanced equation

Balance the chemical equation algebraically: O_2 + Cl_2 + CH_3CH_2CH_2CH_3 ⟶ H_2O + CO_2 + CCl_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 Cl_2 + c_3 CH_3CH_2CH_2CH_3 ⟶ c_4 H_2O + c_5 CO_2 + c_6 CCl_4 Set the number of atoms in the reactants equal to the number of atoms in the products for O, Cl, C and H: O: | 2 c_1 = c_4 + 2 c_5 Cl: | 2 c_2 = 4 c_6 C: | 4 c_3 = c_5 + c_6 H: | 10 c_3 = 2 c_4 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_3 = 1 and solve the system of equations for the remaining coefficients: c_2 = 13 - 2 c_1 c_3 = 1 c_4 = 5 c_5 = c_1 - 5/2 c_6 = 13/2 - c_1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_2 = 26 - 2 c_1 c_3 = 2 c_4 = 10 c_5 = c_1 - 5 c_6 = 13 - c_1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 9 and solve for the remaining coefficients: c_1 = 9 c_2 = 8 c_3 = 2 c_4 = 10 c_5 = 4 c_6 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 9 O_2 + 8 Cl_2 + 2 CH_3CH_2CH_2CH_3 ⟶ 10 H_2O + 4 CO_2 + 4 CCl_4
Balance the chemical equation algebraically: O_2 + Cl_2 + CH_3CH_2CH_2CH_3 ⟶ H_2O + CO_2 + CCl_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 Cl_2 + c_3 CH_3CH_2CH_2CH_3 ⟶ c_4 H_2O + c_5 CO_2 + c_6 CCl_4 Set the number of atoms in the reactants equal to the number of atoms in the products for O, Cl, C and H: O: | 2 c_1 = c_4 + 2 c_5 Cl: | 2 c_2 = 4 c_6 C: | 4 c_3 = c_5 + c_6 H: | 10 c_3 = 2 c_4 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_3 = 1 and solve the system of equations for the remaining coefficients: c_2 = 13 - 2 c_1 c_3 = 1 c_4 = 5 c_5 = c_1 - 5/2 c_6 = 13/2 - c_1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_2 = 26 - 2 c_1 c_3 = 2 c_4 = 10 c_5 = c_1 - 5 c_6 = 13 - c_1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 9 and solve for the remaining coefficients: c_1 = 9 c_2 = 8 c_3 = 2 c_4 = 10 c_5 = 4 c_6 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 9 O_2 + 8 Cl_2 + 2 CH_3CH_2CH_2CH_3 ⟶ 10 H_2O + 4 CO_2 + 4 CCl_4

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

oxygen + chlorine + butane ⟶ water + carbon dioxide + carbon tetrachloride
oxygen + chlorine + butane ⟶ water + carbon dioxide + carbon tetrachloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: O_2 + Cl_2 + CH_3CH_2CH_2CH_3 ⟶ H_2O + CO_2 + CCl_4 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: 9 O_2 + 8 Cl_2 + 2 CH_3CH_2CH_2CH_3 ⟶ 10 H_2O + 4 CO_2 + 4 CCl_4 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 | 9 | -9 Cl_2 | 8 | -8 CH_3CH_2CH_2CH_3 | 2 | -2 H_2O | 10 | 10 CO_2 | 4 | 4 CCl_4 | 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 | 9 | -9 | ([O2])^(-9) Cl_2 | 8 | -8 | ([Cl2])^(-8) CH_3CH_2CH_2CH_3 | 2 | -2 | ([CH3CH2CH2CH3])^(-2) H_2O | 10 | 10 | ([H2O])^10 CO_2 | 4 | 4 | ([CO2])^4 CCl_4 | 4 | 4 | ([CCl4])^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])^(-9) ([Cl2])^(-8) ([CH3CH2CH2CH3])^(-2) ([H2O])^10 ([CO2])^4 ([CCl4])^4 = (([H2O])^10 ([CO2])^4 ([CCl4])^4)/(([O2])^9 ([Cl2])^8 ([CH3CH2CH2CH3])^2)
Construct the equilibrium constant, K, expression for: O_2 + Cl_2 + CH_3CH_2CH_2CH_3 ⟶ H_2O + CO_2 + CCl_4 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: 9 O_2 + 8 Cl_2 + 2 CH_3CH_2CH_2CH_3 ⟶ 10 H_2O + 4 CO_2 + 4 CCl_4 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 | 9 | -9 Cl_2 | 8 | -8 CH_3CH_2CH_2CH_3 | 2 | -2 H_2O | 10 | 10 CO_2 | 4 | 4 CCl_4 | 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 | 9 | -9 | ([O2])^(-9) Cl_2 | 8 | -8 | ([Cl2])^(-8) CH_3CH_2CH_2CH_3 | 2 | -2 | ([CH3CH2CH2CH3])^(-2) H_2O | 10 | 10 | ([H2O])^10 CO_2 | 4 | 4 | ([CO2])^4 CCl_4 | 4 | 4 | ([CCl4])^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])^(-9) ([Cl2])^(-8) ([CH3CH2CH2CH3])^(-2) ([H2O])^10 ([CO2])^4 ([CCl4])^4 = (([H2O])^10 ([CO2])^4 ([CCl4])^4)/(([O2])^9 ([Cl2])^8 ([CH3CH2CH2CH3])^2)

Rate of reaction

Construct the rate of reaction expression for: O_2 + Cl_2 + CH_3CH_2CH_2CH_3 ⟶ H_2O + CO_2 + CCl_4 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: 9 O_2 + 8 Cl_2 + 2 CH_3CH_2CH_2CH_3 ⟶ 10 H_2O + 4 CO_2 + 4 CCl_4 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 | 9 | -9 Cl_2 | 8 | -8 CH_3CH_2CH_2CH_3 | 2 | -2 H_2O | 10 | 10 CO_2 | 4 | 4 CCl_4 | 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 | 9 | -9 | -1/9 (Δ[O2])/(Δt) Cl_2 | 8 | -8 | -1/8 (Δ[Cl2])/(Δt) CH_3CH_2CH_2CH_3 | 2 | -2 | -1/2 (Δ[CH3CH2CH2CH3])/(Δt) H_2O | 10 | 10 | 1/10 (Δ[H2O])/(Δt) CO_2 | 4 | 4 | 1/4 (Δ[CO2])/(Δt) CCl_4 | 4 | 4 | 1/4 (Δ[CCl4])/(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 = -1/9 (Δ[O2])/(Δt) = -1/8 (Δ[Cl2])/(Δt) = -1/2 (Δ[CH3CH2CH2CH3])/(Δt) = 1/10 (Δ[H2O])/(Δt) = 1/4 (Δ[CO2])/(Δt) = 1/4 (Δ[CCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: O_2 + Cl_2 + CH_3CH_2CH_2CH_3 ⟶ H_2O + CO_2 + CCl_4 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: 9 O_2 + 8 Cl_2 + 2 CH_3CH_2CH_2CH_3 ⟶ 10 H_2O + 4 CO_2 + 4 CCl_4 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 | 9 | -9 Cl_2 | 8 | -8 CH_3CH_2CH_2CH_3 | 2 | -2 H_2O | 10 | 10 CO_2 | 4 | 4 CCl_4 | 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 | 9 | -9 | -1/9 (Δ[O2])/(Δt) Cl_2 | 8 | -8 | -1/8 (Δ[Cl2])/(Δt) CH_3CH_2CH_2CH_3 | 2 | -2 | -1/2 (Δ[CH3CH2CH2CH3])/(Δt) H_2O | 10 | 10 | 1/10 (Δ[H2O])/(Δt) CO_2 | 4 | 4 | 1/4 (Δ[CO2])/(Δt) CCl_4 | 4 | 4 | 1/4 (Δ[CCl4])/(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 = -1/9 (Δ[O2])/(Δt) = -1/8 (Δ[Cl2])/(Δt) = -1/2 (Δ[CH3CH2CH2CH3])/(Δt) = 1/10 (Δ[H2O])/(Δt) = 1/4 (Δ[CO2])/(Δt) = 1/4 (Δ[CCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| oxygen | chlorine | butane | water | carbon dioxide | carbon tetrachloride formula | O_2 | Cl_2 | CH_3CH_2CH_2CH_3 | H_2O | CO_2 | CCl_4 Hill formula | O_2 | Cl_2 | C_4H_10 | H_2O | CO_2 | CCl_4 name | oxygen | chlorine | butane | water | carbon dioxide | carbon tetrachloride IUPAC name | molecular oxygen | molecular chlorine | butane | water | carbon dioxide | carbon tetrachloride
| oxygen | chlorine | butane | water | carbon dioxide | carbon tetrachloride formula | O_2 | Cl_2 | CH_3CH_2CH_2CH_3 | H_2O | CO_2 | CCl_4 Hill formula | O_2 | Cl_2 | C_4H_10 | H_2O | CO_2 | CCl_4 name | oxygen | chlorine | butane | water | carbon dioxide | carbon tetrachloride IUPAC name | molecular oxygen | molecular chlorine | butane | water | carbon dioxide | carbon tetrachloride

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