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Al2O3 + SO3 = Al2(SO4)3

Input interpretation

Al_2O_3 aluminum oxide + SO_3 sulfur trioxide ⟶ Al_2(SO_4)_3 aluminum sulfate
Al_2O_3 aluminum oxide + SO_3 sulfur trioxide ⟶ Al_2(SO_4)_3 aluminum sulfate

Balanced equation

Balance the chemical equation algebraically: Al_2O_3 + SO_3 ⟶ Al_2(SO_4)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Al_2O_3 + c_2 SO_3 ⟶ c_3 Al_2(SO_4)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Al, O and S: Al: | 2 c_1 = 2 c_3 O: | 3 c_1 + 3 c_2 = 12 c_3 S: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 3 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: |   | Al_2O_3 + 3 SO_3 ⟶ Al_2(SO_4)_3
Balance the chemical equation algebraically: Al_2O_3 + SO_3 ⟶ Al_2(SO_4)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Al_2O_3 + c_2 SO_3 ⟶ c_3 Al_2(SO_4)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Al, O and S: Al: | 2 c_1 = 2 c_3 O: | 3 c_1 + 3 c_2 = 12 c_3 S: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 3 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Al_2O_3 + 3 SO_3 ⟶ Al_2(SO_4)_3

Structures

 + ⟶
+ ⟶

Names

aluminum oxide + sulfur trioxide ⟶ aluminum sulfate
aluminum oxide + sulfur trioxide ⟶ aluminum sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: Al_2O_3 + SO_3 ⟶ Al_2(SO_4)_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: Al_2O_3 + 3 SO_3 ⟶ Al_2(SO_4)_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_2O_3 | 1 | -1 SO_3 | 3 | -3 Al_2(SO_4)_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_2O_3 | 1 | -1 | ([Al2O3])^(-1) SO_3 | 3 | -3 | ([SO3])^(-3) Al_2(SO_4)_3 | 1 | 1 | [Al2(SO4)3] 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 = ([Al2O3])^(-1) ([SO3])^(-3) [Al2(SO4)3] = ([Al2(SO4)3])/([Al2O3] ([SO3])^3)
Construct the equilibrium constant, K, expression for: Al_2O_3 + SO_3 ⟶ Al_2(SO_4)_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: Al_2O_3 + 3 SO_3 ⟶ Al_2(SO_4)_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_2O_3 | 1 | -1 SO_3 | 3 | -3 Al_2(SO_4)_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_2O_3 | 1 | -1 | ([Al2O3])^(-1) SO_3 | 3 | -3 | ([SO3])^(-3) Al_2(SO_4)_3 | 1 | 1 | [Al2(SO4)3] 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 = ([Al2O3])^(-1) ([SO3])^(-3) [Al2(SO4)3] = ([Al2(SO4)3])/([Al2O3] ([SO3])^3)

Rate of reaction

Construct the rate of reaction expression for: Al_2O_3 + SO_3 ⟶ Al_2(SO_4)_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: Al_2O_3 + 3 SO_3 ⟶ Al_2(SO_4)_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_2O_3 | 1 | -1 SO_3 | 3 | -3 Al_2(SO_4)_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_2O_3 | 1 | -1 | -(Δ[Al2O3])/(Δt) SO_3 | 3 | -3 | -1/3 (Δ[SO3])/(Δt) Al_2(SO_4)_3 | 1 | 1 | (Δ[Al2(SO4)3])/(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 = -(Δ[Al2O3])/(Δt) = -1/3 (Δ[SO3])/(Δt) = (Δ[Al2(SO4)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Al_2O_3 + SO_3 ⟶ Al_2(SO_4)_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: Al_2O_3 + 3 SO_3 ⟶ Al_2(SO_4)_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_2O_3 | 1 | -1 SO_3 | 3 | -3 Al_2(SO_4)_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_2O_3 | 1 | -1 | -(Δ[Al2O3])/(Δt) SO_3 | 3 | -3 | -1/3 (Δ[SO3])/(Δt) Al_2(SO_4)_3 | 1 | 1 | (Δ[Al2(SO4)3])/(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 = -(Δ[Al2O3])/(Δt) = -1/3 (Δ[SO3])/(Δt) = (Δ[Al2(SO4)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

 | aluminum oxide | sulfur trioxide | aluminum sulfate formula | Al_2O_3 | SO_3 | Al_2(SO_4)_3 Hill formula | Al_2O_3 | O_3S | Al_2O_12S_3 name | aluminum oxide | sulfur trioxide | aluminum sulfate IUPAC name | dialuminum;oxygen(2-) | sulfur trioxide | dialuminum trisulfate
| aluminum oxide | sulfur trioxide | aluminum sulfate formula | Al_2O_3 | SO_3 | Al_2(SO_4)_3 Hill formula | Al_2O_3 | O_3S | Al_2O_12S_3 name | aluminum oxide | sulfur trioxide | aluminum sulfate IUPAC name | dialuminum;oxygen(2-) | sulfur trioxide | dialuminum trisulfate

Substance properties

 | aluminum oxide | sulfur trioxide | aluminum sulfate molar mass | 101.96 g/mol | 80.06 g/mol | 342.1 g/mol phase | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 2040 °C | 16.8 °C | 770 °C boiling point | | 44.7 °C |  density | | 1.97 g/cm^3 | 2.71 g/cm^3 solubility in water | | reacts | soluble dynamic viscosity | | 0.00159 Pa s (at 30 °C) |  odor | odorless | |
| aluminum oxide | sulfur trioxide | aluminum sulfate molar mass | 101.96 g/mol | 80.06 g/mol | 342.1 g/mol phase | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 2040 °C | 16.8 °C | 770 °C boiling point | | 44.7 °C | density | | 1.97 g/cm^3 | 2.71 g/cm^3 solubility in water | | reacts | soluble dynamic viscosity | | 0.00159 Pa s (at 30 °C) | odor | odorless | |

Units