Input interpretation
![O_2 oxygen + Co cobalt ⟶ O_3Co_2 cobalt(III) oxide](../image_source/9dfb7822f91669f19c4ace4f54fd33b3.png)
O_2 oxygen + Co cobalt ⟶ O_3Co_2 cobalt(III) oxide
Balanced equation
![Balance the chemical equation algebraically: O_2 + Co ⟶ O_3Co_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 Co ⟶ c_3 O_3Co_2 Set the number of atoms in the reactants equal to the number of atoms in the products for O and Co: O: | 2 c_1 = 3 c_3 Co: | 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3/2 c_2 = 2 c_3 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 4 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 O_2 + 4 Co ⟶ 2 O_3Co_2](../image_source/f10a985737fde233b27d63617ce7fc23.png)
Balance the chemical equation algebraically: O_2 + Co ⟶ O_3Co_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 Co ⟶ c_3 O_3Co_2 Set the number of atoms in the reactants equal to the number of atoms in the products for O and Co: O: | 2 c_1 = 3 c_3 Co: | 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3/2 c_2 = 2 c_3 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 4 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 O_2 + 4 Co ⟶ 2 O_3Co_2
Structures
![+ ⟶](../image_source/26db057894fbff1ace3127dc325d2446.png)
+ ⟶
Names
![oxygen + cobalt ⟶ cobalt(III) oxide](../image_source/36f225531594555bbc47a1ef36c46435.png)
oxygen + cobalt ⟶ cobalt(III) oxide
Equilibrium constant
![Construct the equilibrium constant, K, expression for: O_2 + Co ⟶ O_3Co_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: 3 O_2 + 4 Co ⟶ 2 O_3Co_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 | 3 | -3 Co | 4 | -4 O_3Co_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 3 | -3 | ([O2])^(-3) Co | 4 | -4 | ([Co])^(-4) O_3Co_2 | 2 | 2 | ([O3Co2])^2 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])^(-3) ([Co])^(-4) ([O3Co2])^2 = ([O3Co2])^2/(([O2])^3 ([Co])^4)](../image_source/de29d3567435513b3b83a36888ee4e5f.png)
Construct the equilibrium constant, K, expression for: O_2 + Co ⟶ O_3Co_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: 3 O_2 + 4 Co ⟶ 2 O_3Co_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 | 3 | -3 Co | 4 | -4 O_3Co_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 3 | -3 | ([O2])^(-3) Co | 4 | -4 | ([Co])^(-4) O_3Co_2 | 2 | 2 | ([O3Co2])^2 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])^(-3) ([Co])^(-4) ([O3Co2])^2 = ([O3Co2])^2/(([O2])^3 ([Co])^4)
Rate of reaction
![Construct the rate of reaction expression for: O_2 + Co ⟶ O_3Co_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: 3 O_2 + 4 Co ⟶ 2 O_3Co_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 | 3 | -3 Co | 4 | -4 O_3Co_2 | 2 | 2 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 | 3 | -3 | -1/3 (Δ[O2])/(Δt) Co | 4 | -4 | -1/4 (Δ[Co])/(Δt) O_3Co_2 | 2 | 2 | 1/2 (Δ[O3Co2])/(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 = -1/3 (Δ[O2])/(Δt) = -1/4 (Δ[Co])/(Δt) = 1/2 (Δ[O3Co2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/3ad2d42f35cb5ece8fc2ec77846a21b3.png)
Construct the rate of reaction expression for: O_2 + Co ⟶ O_3Co_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: 3 O_2 + 4 Co ⟶ 2 O_3Co_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 | 3 | -3 Co | 4 | -4 O_3Co_2 | 2 | 2 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 | 3 | -3 | -1/3 (Δ[O2])/(Δt) Co | 4 | -4 | -1/4 (Δ[Co])/(Δt) O_3Co_2 | 2 | 2 | 1/2 (Δ[O3Co2])/(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 = -1/3 (Δ[O2])/(Δt) = -1/4 (Δ[Co])/(Δt) = 1/2 (Δ[O3Co2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| oxygen | cobalt | cobalt(III) oxide formula | O_2 | Co | O_3Co_2 Hill formula | O_2 | Co | Co_2O_3 name | oxygen | cobalt | cobalt(III) oxide IUPAC name | molecular oxygen | cobalt | oxo(oxocobaltiooxy)cobalt](../image_source/decf39388e88560ebad854cd1e679c56.png)
| oxygen | cobalt | cobalt(III) oxide formula | O_2 | Co | O_3Co_2 Hill formula | O_2 | Co | Co_2O_3 name | oxygen | cobalt | cobalt(III) oxide IUPAC name | molecular oxygen | cobalt | oxo(oxocobaltiooxy)cobalt
Substance properties
![| oxygen | cobalt | cobalt(III) oxide molar mass | 31.998 g/mol | 58.933194 g/mol | 165.863 g/mol phase | gas (at STP) | solid (at STP) | melting point | -218 °C | 1495 °C | boiling point | -183 °C | 2900 °C | density | 0.001429 g/cm^3 (at 0 °C) | 8.9 g/cm^3 | solubility in water | | insoluble | surface tension | 0.01347 N/m | | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | | odor | odorless | |](../image_source/de1972a7817d773e75c5af6ba3c6643e.png)
| oxygen | cobalt | cobalt(III) oxide molar mass | 31.998 g/mol | 58.933194 g/mol | 165.863 g/mol phase | gas (at STP) | solid (at STP) | melting point | -218 °C | 1495 °C | boiling point | -183 °C | 2900 °C | density | 0.001429 g/cm^3 (at 0 °C) | 8.9 g/cm^3 | solubility in water | | insoluble | surface tension | 0.01347 N/m | | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | | odor | odorless | |
Units
Input interpretation
![O_2 oxygen + CO carbon monoxide ⟶ CO2O3](../image_source/48191ce54fd242faea5c91e9880c1ce0.png)
O_2 oxygen + CO carbon monoxide ⟶ CO2O3
Balanced equation
![Balance the chemical equation algebraically: O_2 + CO ⟶ CO2O3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 CO ⟶ c_3 CO2O3 Set the number of atoms in the reactants equal to the number of atoms in the products for O and C: O: | 2 c_1 + c_2 = 5 c_3 C: | c_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 = 2 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 O_2 + CO ⟶ CO2O3](../image_source/df9499317a0d09b650a8b069405e1be6.png)
Balance the chemical equation algebraically: O_2 + CO ⟶ CO2O3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 CO ⟶ c_3 CO2O3 Set the number of atoms in the reactants equal to the number of atoms in the products for O and C: O: | 2 c_1 + c_2 = 5 c_3 C: | c_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 = 2 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 O_2 + CO ⟶ CO2O3
Structures
![+ ⟶ CO2O3](../image_source/4431782760d4e560334ffa7ccd23e556.png)
+ ⟶ CO2O3
Names
![oxygen + carbon monoxide ⟶ CO2O3](../image_source/b9bcf48e84eeb98560524e31d05e61a6.png)
oxygen + carbon monoxide ⟶ CO2O3
Equilibrium constant
![Construct the equilibrium constant, K, expression for: O_2 + CO ⟶ CO2O3 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: 2 O_2 + CO ⟶ CO2O3 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 | 2 | -2 CO | 1 | -1 CO2O3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 2 | -2 | ([O2])^(-2) CO | 1 | -1 | ([CO])^(-1) CO2O3 | 1 | 1 | [CO2O3] 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])^(-2) ([CO])^(-1) [CO2O3] = ([CO2O3])/(([O2])^2 [CO])](../image_source/ed8893887867437b0bd0930b8c8010e0.png)
Construct the equilibrium constant, K, expression for: O_2 + CO ⟶ CO2O3 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: 2 O_2 + CO ⟶ CO2O3 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 | 2 | -2 CO | 1 | -1 CO2O3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 2 | -2 | ([O2])^(-2) CO | 1 | -1 | ([CO])^(-1) CO2O3 | 1 | 1 | [CO2O3] 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])^(-2) ([CO])^(-1) [CO2O3] = ([CO2O3])/(([O2])^2 [CO])
Rate of reaction
![Construct the rate of reaction expression for: O_2 + CO ⟶ CO2O3 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: 2 O_2 + CO ⟶ CO2O3 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 | 2 | -2 CO | 1 | -1 CO2O3 | 1 | 1 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 | 2 | -2 | -1/2 (Δ[O2])/(Δt) CO | 1 | -1 | -(Δ[CO])/(Δt) CO2O3 | 1 | 1 | (Δ[CO2O3])/(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 = -1/2 (Δ[O2])/(Δt) = -(Δ[CO])/(Δt) = (Δ[CO2O3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/6164d7b1c35d20abe508e3bad6ffc010.png)
Construct the rate of reaction expression for: O_2 + CO ⟶ CO2O3 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: 2 O_2 + CO ⟶ CO2O3 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 | 2 | -2 CO | 1 | -1 CO2O3 | 1 | 1 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 | 2 | -2 | -1/2 (Δ[O2])/(Δt) CO | 1 | -1 | -(Δ[CO])/(Δt) CO2O3 | 1 | 1 | (Δ[CO2O3])/(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 = -1/2 (Δ[O2])/(Δt) = -(Δ[CO])/(Δt) = (Δ[CO2O3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| oxygen | carbon monoxide | CO2O3 formula | O_2 | CO | CO2O3 Hill formula | O_2 | CO | CO5 name | oxygen | carbon monoxide | IUPAC name | molecular oxygen | carbon monoxide |](../image_source/54c1bd39330700e8572c5ab5fa6bfc29.png)
| oxygen | carbon monoxide | CO2O3 formula | O_2 | CO | CO2O3 Hill formula | O_2 | CO | CO5 name | oxygen | carbon monoxide | IUPAC name | molecular oxygen | carbon monoxide |
Substance properties
![| oxygen | carbon monoxide | CO2O3 molar mass | 31.998 g/mol | 28.01 g/mol | 92.006 g/mol phase | gas (at STP) | gas (at STP) | melting point | -218 °C | -205 °C | boiling point | -183 °C | -191.5 °C | density | 0.001429 g/cm^3 (at 0 °C) | 0.001145 g/cm^3 (at 25 °C) | surface tension | 0.01347 N/m | | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | 1.772×10^-5 Pa s (at 25 °C) | odor | odorless | odorless |](../image_source/37c3246da5ffd39542e522877b09a803.png)
| oxygen | carbon monoxide | CO2O3 molar mass | 31.998 g/mol | 28.01 g/mol | 92.006 g/mol phase | gas (at STP) | gas (at STP) | melting point | -218 °C | -205 °C | boiling point | -183 °C | -191.5 °C | density | 0.001429 g/cm^3 (at 0 °C) | 0.001145 g/cm^3 (at 25 °C) | surface tension | 0.01347 N/m | | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | 1.772×10^-5 Pa s (at 25 °C) | odor | odorless | odorless |
Units
Input interpretation
![O_2 oxygen + CO carbon monoxide ⟶ CO2O3](../image_source/768870abef297750b15257b18d5b3c31.png)
O_2 oxygen + CO carbon monoxide ⟶ CO2O3
Balanced equation
![Balance the chemical equation algebraically: O_2 + CO ⟶ CO2O3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 CO ⟶ c_3 CO2O3 Set the number of atoms in the reactants equal to the number of atoms in the products for O and C: O: | 2 c_1 + c_2 = 5 c_3 C: | c_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 = 2 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 O_2 + CO ⟶ CO2O3](../image_source/450c0d26dc793716be58c0ca0b7eff7d.png)
Balance the chemical equation algebraically: O_2 + CO ⟶ CO2O3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 CO ⟶ c_3 CO2O3 Set the number of atoms in the reactants equal to the number of atoms in the products for O and C: O: | 2 c_1 + c_2 = 5 c_3 C: | c_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 = 2 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 O_2 + CO ⟶ CO2O3
Structures
![+ ⟶ CO2O3](../image_source/e78c169944a5fea8772f22dd449f1569.png)
+ ⟶ CO2O3
Names
![oxygen + carbon monoxide ⟶ CO2O3](../image_source/4aa795296b4faaf0ed9a45220c60d830.png)
oxygen + carbon monoxide ⟶ CO2O3
Equilibrium constant
![Construct the equilibrium constant, K, expression for: O_2 + CO ⟶ CO2O3 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: 2 O_2 + CO ⟶ CO2O3 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 | 2 | -2 CO | 1 | -1 CO2O3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 2 | -2 | ([O2])^(-2) CO | 1 | -1 | ([CO])^(-1) CO2O3 | 1 | 1 | [CO2O3] 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])^(-2) ([CO])^(-1) [CO2O3] = ([CO2O3])/(([O2])^2 [CO])](../image_source/f29a357aa691910673614b879bbebb41.png)
Construct the equilibrium constant, K, expression for: O_2 + CO ⟶ CO2O3 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: 2 O_2 + CO ⟶ CO2O3 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 | 2 | -2 CO | 1 | -1 CO2O3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 2 | -2 | ([O2])^(-2) CO | 1 | -1 | ([CO])^(-1) CO2O3 | 1 | 1 | [CO2O3] 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])^(-2) ([CO])^(-1) [CO2O3] = ([CO2O3])/(([O2])^2 [CO])
Rate of reaction
![Construct the rate of reaction expression for: O_2 + CO ⟶ CO2O3 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: 2 O_2 + CO ⟶ CO2O3 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 | 2 | -2 CO | 1 | -1 CO2O3 | 1 | 1 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 | 2 | -2 | -1/2 (Δ[O2])/(Δt) CO | 1 | -1 | -(Δ[CO])/(Δt) CO2O3 | 1 | 1 | (Δ[CO2O3])/(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 = -1/2 (Δ[O2])/(Δt) = -(Δ[CO])/(Δt) = (Δ[CO2O3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/ca04b6ae7fb6aa4ae736ee0913be9e0f.png)
Construct the rate of reaction expression for: O_2 + CO ⟶ CO2O3 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: 2 O_2 + CO ⟶ CO2O3 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 | 2 | -2 CO | 1 | -1 CO2O3 | 1 | 1 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 | 2 | -2 | -1/2 (Δ[O2])/(Δt) CO | 1 | -1 | -(Δ[CO])/(Δt) CO2O3 | 1 | 1 | (Δ[CO2O3])/(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 = -1/2 (Δ[O2])/(Δt) = -(Δ[CO])/(Δt) = (Δ[CO2O3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| oxygen | carbon monoxide | CO2O3 formula | O_2 | CO | CO2O3 Hill formula | O_2 | CO | CO5 name | oxygen | carbon monoxide | IUPAC name | molecular oxygen | carbon monoxide |](../image_source/2ea823db15d4073dc2de43c46546f580.png)
| oxygen | carbon monoxide | CO2O3 formula | O_2 | CO | CO2O3 Hill formula | O_2 | CO | CO5 name | oxygen | carbon monoxide | IUPAC name | molecular oxygen | carbon monoxide |
Substance properties
![| oxygen | carbon monoxide | CO2O3 molar mass | 31.998 g/mol | 28.01 g/mol | 92.006 g/mol phase | gas (at STP) | gas (at STP) | melting point | -218 °C | -205 °C | boiling point | -183 °C | -191.5 °C | density | 0.001429 g/cm^3 (at 0 °C) | 0.001145 g/cm^3 (at 25 °C) | surface tension | 0.01347 N/m | | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | 1.772×10^-5 Pa s (at 25 °C) | odor | odorless | odorless |](../image_source/e70368bd5e8cf4a28d97d394beca71e8.png)
| oxygen | carbon monoxide | CO2O3 molar mass | 31.998 g/mol | 28.01 g/mol | 92.006 g/mol phase | gas (at STP) | gas (at STP) | melting point | -218 °C | -205 °C | boiling point | -183 °C | -191.5 °C | density | 0.001429 g/cm^3 (at 0 °C) | 0.001145 g/cm^3 (at 25 °C) | surface tension | 0.01347 N/m | | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | 1.772×10^-5 Pa s (at 25 °C) | odor | odorless | odorless |
Units