Input interpretation
![Al aluminum + O_3 ozone ⟶ Al_2O_3 aluminum oxide](../image_source/6724c09e5ce05c2c3c414e6847a7cacb.png)
Al aluminum + O_3 ozone ⟶ Al_2O_3 aluminum oxide
Balanced equation
![Balance the chemical equation algebraically: Al + O_3 ⟶ Al_2O_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Al + c_2 O_3 ⟶ c_3 Al_2O_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Al and O: Al: | c_1 = 2 c_3 O: | 3 c_2 = 3 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 Al + O_3 ⟶ Al_2O_3](../image_source/ab115d756811a3ff0aad8c86a4c89303.png)
Balance the chemical equation algebraically: Al + O_3 ⟶ Al_2O_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Al + c_2 O_3 ⟶ c_3 Al_2O_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Al and O: Al: | c_1 = 2 c_3 O: | 3 c_2 = 3 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 Al + O_3 ⟶ Al_2O_3
Structures
![+ ⟶](../image_source/cfdeb4877b539a38b3dc04c8e34afd1b.png)
+ ⟶
Names
![aluminum + ozone ⟶ aluminum oxide](../image_source/76d191606eb533d27e62106751b0a512.png)
aluminum + ozone ⟶ aluminum oxide
Reaction thermodynamics
Enthalpy
![| aluminum | ozone | aluminum oxide molecular enthalpy | 0 kJ/mol | 142.7 kJ/mol | -1676 kJ/mol total enthalpy | 0 kJ/mol | 142.7 kJ/mol | -1676 kJ/mol | H_initial = 142.7 kJ/mol | | H_final = -1676 kJ/mol ΔH_rxn^0 | -1676 kJ/mol - 142.7 kJ/mol = -1819 kJ/mol (exothermic) | |](../image_source/c26fb4fcfe13d11674da53e9986ceb8b.png)
| aluminum | ozone | aluminum oxide molecular enthalpy | 0 kJ/mol | 142.7 kJ/mol | -1676 kJ/mol total enthalpy | 0 kJ/mol | 142.7 kJ/mol | -1676 kJ/mol | H_initial = 142.7 kJ/mol | | H_final = -1676 kJ/mol ΔH_rxn^0 | -1676 kJ/mol - 142.7 kJ/mol = -1819 kJ/mol (exothermic) | |
Entropy
![| aluminum | ozone | aluminum oxide molecular entropy | 28.3 J/(mol K) | 239 J/(mol K) | 51 J/(mol K) total entropy | 56.6 J/(mol K) | 239 J/(mol K) | 51 J/(mol K) | S_initial = 295.6 J/(mol K) | | S_final = 51 J/(mol K) ΔS_rxn^0 | 51 J/(mol K) - 295.6 J/(mol K) = -244.6 J/(mol K) (exoentropic) | |](../image_source/47de8e2f5a283fc38ee981fa52c0f9a3.png)
| aluminum | ozone | aluminum oxide molecular entropy | 28.3 J/(mol K) | 239 J/(mol K) | 51 J/(mol K) total entropy | 56.6 J/(mol K) | 239 J/(mol K) | 51 J/(mol K) | S_initial = 295.6 J/(mol K) | | S_final = 51 J/(mol K) ΔS_rxn^0 | 51 J/(mol K) - 295.6 J/(mol K) = -244.6 J/(mol K) (exoentropic) | |
Equilibrium constant
![Construct the equilibrium constant, K, expression for: Al + O_3 ⟶ Al_2O_3 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 Al + O_3 ⟶ Al_2O_3 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 Al | 2 | -2 O_3 | 1 | -1 Al_2O_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Al | 2 | -2 | ([Al])^(-2) O_3 | 1 | -1 | ([O3])^(-1) Al_2O_3 | 1 | 1 | [Al2O3] 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 = ([Al])^(-2) ([O3])^(-1) [Al2O3] = ([Al2O3])/(([Al])^2 [O3])](../image_source/7f0163bcd5ef4729ba23da1a0036bc91.png)
Construct the equilibrium constant, K, expression for: Al + O_3 ⟶ Al_2O_3 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 Al + O_3 ⟶ Al_2O_3 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 Al | 2 | -2 O_3 | 1 | -1 Al_2O_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Al | 2 | -2 | ([Al])^(-2) O_3 | 1 | -1 | ([O3])^(-1) Al_2O_3 | 1 | 1 | [Al2O3] 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 = ([Al])^(-2) ([O3])^(-1) [Al2O3] = ([Al2O3])/(([Al])^2 [O3])
Rate of reaction
![Construct the rate of reaction expression for: Al + O_3 ⟶ Al_2O_3 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 Al + O_3 ⟶ Al_2O_3 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 Al | 2 | -2 O_3 | 1 | -1 Al_2O_3 | 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 Al | 2 | -2 | -1/2 (Δ[Al])/(Δt) O_3 | 1 | -1 | -(Δ[O3])/(Δt) Al_2O_3 | 1 | 1 | (Δ[Al2O3])/(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[Al])/(Δt) = -(Δ[O3])/(Δt) = (Δ[Al2O3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/d7757c9beccf802016adb782366ad709.png)
Construct the rate of reaction expression for: Al + O_3 ⟶ Al_2O_3 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 Al + O_3 ⟶ Al_2O_3 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 Al | 2 | -2 O_3 | 1 | -1 Al_2O_3 | 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 Al | 2 | -2 | -1/2 (Δ[Al])/(Δt) O_3 | 1 | -1 | -(Δ[O3])/(Δt) Al_2O_3 | 1 | 1 | (Δ[Al2O3])/(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[Al])/(Δt) = -(Δ[O3])/(Δt) = (Δ[Al2O3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| aluminum | ozone | aluminum oxide formula | Al | O_3 | Al_2O_3 name | aluminum | ozone | aluminum oxide IUPAC name | aluminum | ozone | dialuminum;oxygen(2-)](../image_source/e5aa00b7126b125502533ce5460535e5.png)
| aluminum | ozone | aluminum oxide formula | Al | O_3 | Al_2O_3 name | aluminum | ozone | aluminum oxide IUPAC name | aluminum | ozone | dialuminum;oxygen(2-)
Substance properties
![| aluminum | ozone | aluminum oxide molar mass | 26.9815385 g/mol | 47.997 g/mol | 101.96 g/mol phase | solid (at STP) | gas (at STP) | solid (at STP) melting point | 660.4 °C | -192.2 °C | 2040 °C boiling point | 2460 °C | -111.9 °C | density | 2.7 g/cm^3 | 0.001962 g/cm^3 (at 25 °C) | solubility in water | insoluble | | surface tension | 0.817 N/m | | dynamic viscosity | 1.5×10^-4 Pa s (at 760 °C) | | odor | odorless | | odorless](../image_source/13fe39b9df350c72ddf3ac2054d092e4.png)
| aluminum | ozone | aluminum oxide molar mass | 26.9815385 g/mol | 47.997 g/mol | 101.96 g/mol phase | solid (at STP) | gas (at STP) | solid (at STP) melting point | 660.4 °C | -192.2 °C | 2040 °C boiling point | 2460 °C | -111.9 °C | density | 2.7 g/cm^3 | 0.001962 g/cm^3 (at 25 °C) | solubility in water | insoluble | | surface tension | 0.817 N/m | | dynamic viscosity | 1.5×10^-4 Pa s (at 760 °C) | | odor | odorless | | odorless
Units