Input interpretation
![O_2 (oxygen) + CH_3(CH_2)_5CH_3 (N-heptane) ⟶ H_2O (water) + CO_2 (carbon dioxide)](../image_source/ae0fe89f9230f2948d42b337d7d7bb87.png)
O_2 (oxygen) + CH_3(CH_2)_5CH_3 (N-heptane) ⟶ H_2O (water) + CO_2 (carbon dioxide)
Balanced equation
![Balance the chemical equation algebraically: O_2 + CH_3(CH_2)_5CH_3 ⟶ H_2O + CO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 CH_3(CH_2)_5CH_3 ⟶ c_3 H_2O + c_4 CO_2 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 + 2 c_4 C: | 7 c_2 = c_4 H: | 16 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 = 11 c_2 = 1 c_3 = 8 c_4 = 7 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 11 O_2 + CH_3(CH_2)_5CH_3 ⟶ 8 H_2O + 7 CO_2](../image_source/b3b22ef0358220531870e40853191248.png)
Balance the chemical equation algebraically: O_2 + CH_3(CH_2)_5CH_3 ⟶ H_2O + CO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 CH_3(CH_2)_5CH_3 ⟶ c_3 H_2O + c_4 CO_2 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 + 2 c_4 C: | 7 c_2 = c_4 H: | 16 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 = 11 c_2 = 1 c_3 = 8 c_4 = 7 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 11 O_2 + CH_3(CH_2)_5CH_3 ⟶ 8 H_2O + 7 CO_2
Structures
![+ ⟶ +](../image_source/8ad512074a7ee68cce02af5eef5454d8.png)
+ ⟶ +
Names
![oxygen + N-heptane ⟶ water + carbon dioxide](../image_source/5396c43551a9ab4a4535deb1e493196f.png)
oxygen + N-heptane ⟶ water + carbon dioxide
Reaction thermodynamics
Enthalpy
![| oxygen | N-heptane | water | carbon dioxide molecular enthalpy | 0 kJ/mol | -17.63 kJ/mol | -285.8 kJ/mol | -393.5 kJ/mol total enthalpy | 0 kJ/mol | -17.63 kJ/mol | -2287 kJ/mol | -2755 kJ/mol | H_initial = -17.63 kJ/mol | | H_final = -5041 kJ/mol | ΔH_rxn^0 | -5041 kJ/mol - -17.63 kJ/mol = -5024 kJ/mol (exothermic) | | |](../image_source/795800a986e76983a1a40ba2fe1a7961.png)
| oxygen | N-heptane | water | carbon dioxide molecular enthalpy | 0 kJ/mol | -17.63 kJ/mol | -285.8 kJ/mol | -393.5 kJ/mol total enthalpy | 0 kJ/mol | -17.63 kJ/mol | -2287 kJ/mol | -2755 kJ/mol | H_initial = -17.63 kJ/mol | | H_final = -5041 kJ/mol | ΔH_rxn^0 | -5041 kJ/mol - -17.63 kJ/mol = -5024 kJ/mol (exothermic) | | |
Equilibrium constant
![Construct the equilibrium constant, K, expression for: O_2 + CH_3(CH_2)_5CH_3 ⟶ H_2O + CO_2 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: 11 O_2 + CH_3(CH_2)_5CH_3 ⟶ 8 H_2O + 7 CO_2 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 | 11 | -11 CH_3(CH_2)_5CH_3 | 1 | -1 H_2O | 8 | 8 CO_2 | 7 | 7 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 11 | -11 | ([O2])^(-11) CH_3(CH_2)_5CH_3 | 1 | -1 | ([CH3(CH2)5CH3])^(-1) H_2O | 8 | 8 | ([H2O])^8 CO_2 | 7 | 7 | ([CO2])^7 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])^(-11) ([CH3(CH2)5CH3])^(-1) ([H2O])^8 ([CO2])^7 = (([H2O])^8 ([CO2])^7)/(([O2])^11 [CH3(CH2)5CH3])](../image_source/4be78e59fc32e408d12318db6c5bb7a9.png)
Construct the equilibrium constant, K, expression for: O_2 + CH_3(CH_2)_5CH_3 ⟶ H_2O + CO_2 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: 11 O_2 + CH_3(CH_2)_5CH_3 ⟶ 8 H_2O + 7 CO_2 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 | 11 | -11 CH_3(CH_2)_5CH_3 | 1 | -1 H_2O | 8 | 8 CO_2 | 7 | 7 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 11 | -11 | ([O2])^(-11) CH_3(CH_2)_5CH_3 | 1 | -1 | ([CH3(CH2)5CH3])^(-1) H_2O | 8 | 8 | ([H2O])^8 CO_2 | 7 | 7 | ([CO2])^7 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])^(-11) ([CH3(CH2)5CH3])^(-1) ([H2O])^8 ([CO2])^7 = (([H2O])^8 ([CO2])^7)/(([O2])^11 [CH3(CH2)5CH3])
Rate of reaction
![Construct the rate of reaction expression for: O_2 + CH_3(CH_2)_5CH_3 ⟶ H_2O + CO_2 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: 11 O_2 + CH_3(CH_2)_5CH_3 ⟶ 8 H_2O + 7 CO_2 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 | 11 | -11 CH_3(CH_2)_5CH_3 | 1 | -1 H_2O | 8 | 8 CO_2 | 7 | 7 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 | 11 | -11 | -1/11 (Δ[O2])/(Δt) CH_3(CH_2)_5CH_3 | 1 | -1 | -(Δ[CH3(CH2)5CH3])/(Δt) H_2O | 8 | 8 | 1/8 (Δ[H2O])/(Δt) CO_2 | 7 | 7 | 1/7 (Δ[CO2])/(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 = -1/11 (Δ[O2])/(Δt) = -(Δ[CH3(CH2)5CH3])/(Δt) = 1/8 (Δ[H2O])/(Δt) = 1/7 (Δ[CO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/0bd90944a35f19938290495545d78d8f.png)
Construct the rate of reaction expression for: O_2 + CH_3(CH_2)_5CH_3 ⟶ H_2O + CO_2 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: 11 O_2 + CH_3(CH_2)_5CH_3 ⟶ 8 H_2O + 7 CO_2 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 | 11 | -11 CH_3(CH_2)_5CH_3 | 1 | -1 H_2O | 8 | 8 CO_2 | 7 | 7 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 | 11 | -11 | -1/11 (Δ[O2])/(Δt) CH_3(CH_2)_5CH_3 | 1 | -1 | -(Δ[CH3(CH2)5CH3])/(Δt) H_2O | 8 | 8 | 1/8 (Δ[H2O])/(Δt) CO_2 | 7 | 7 | 1/7 (Δ[CO2])/(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 = -1/11 (Δ[O2])/(Δt) = -(Δ[CH3(CH2)5CH3])/(Δt) = 1/8 (Δ[H2O])/(Δt) = 1/7 (Δ[CO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| oxygen | N-heptane | water | carbon dioxide formula | O_2 | CH_3(CH_2)_5CH_3 | H_2O | CO_2 Hill formula | O_2 | C_7H_16 | H_2O | CO_2 name | oxygen | N-heptane | water | carbon dioxide IUPAC name | molecular oxygen | heptane | water | carbon dioxide](../image_source/f461c7281e132577e1c11f3357fd11de.png)
| oxygen | N-heptane | water | carbon dioxide formula | O_2 | CH_3(CH_2)_5CH_3 | H_2O | CO_2 Hill formula | O_2 | C_7H_16 | H_2O | CO_2 name | oxygen | N-heptane | water | carbon dioxide IUPAC name | molecular oxygen | heptane | water | carbon dioxide
Substance properties
![| oxygen | N-heptane | water | carbon dioxide molar mass | 31.998 g/mol | 100.21 g/mol | 18.015 g/mol | 44.009 g/mol phase | gas (at STP) | liquid (at STP) | liquid (at STP) | gas (at STP) melting point | -218 °C | -91 °C | 0 °C | -56.56 °C (at triple point) boiling point | -183 °C | 98 °C | 99.9839 °C | -78.5 °C (at sublimation point) density | 0.001429 g/cm^3 (at 0 °C) | 0.684 g/cm^3 | 1 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) surface tension | 0.01347 N/m | 0.02021 N/m | 0.0728 N/m | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | 3.87×10^-4 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | 1.491×10^-5 Pa s (at 25 °C) odor | odorless | gasoline-like | odorless | odorless](../image_source/f4c68b83dbab4196b3c3d1a28474984b.png)
| oxygen | N-heptane | water | carbon dioxide molar mass | 31.998 g/mol | 100.21 g/mol | 18.015 g/mol | 44.009 g/mol phase | gas (at STP) | liquid (at STP) | liquid (at STP) | gas (at STP) melting point | -218 °C | -91 °C | 0 °C | -56.56 °C (at triple point) boiling point | -183 °C | 98 °C | 99.9839 °C | -78.5 °C (at sublimation point) density | 0.001429 g/cm^3 (at 0 °C) | 0.684 g/cm^3 | 1 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) surface tension | 0.01347 N/m | 0.02021 N/m | 0.0728 N/m | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | 3.87×10^-4 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | 1.491×10^-5 Pa s (at 25 °C) odor | odorless | gasoline-like | odorless | odorless
Units