Input interpretation
Al aluminum + Br_2 bromine ⟶ AlBr2
Balanced equation
Balance the chemical equation algebraically: Al + Br_2 ⟶ AlBr2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Al + c_2 Br_2 ⟶ c_3 AlBr2 Set the number of atoms in the reactants equal to the number of atoms in the products for Al and Br: Al: | c_1 = c_3 Br: | 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Al + Br_2 ⟶ AlBr2
Structures
+ ⟶ AlBr2
Names
aluminum + bromine ⟶ AlBr2
Equilibrium constant
![Construct the equilibrium constant, K, expression for: Al + Br_2 ⟶ AlBr2 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 + Br_2 ⟶ AlBr2 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 | 1 | -1 Br_2 | 1 | -1 AlBr2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Al | 1 | -1 | ([Al])^(-1) Br_2 | 1 | -1 | ([Br2])^(-1) AlBr2 | 1 | 1 | [AlBr2] 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])^(-1) ([Br2])^(-1) [AlBr2] = ([AlBr2])/([Al] [Br2])](../image_source/cfeecda5559c59e7921a355a2d571e13.png)
Construct the equilibrium constant, K, expression for: Al + Br_2 ⟶ AlBr2 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 + Br_2 ⟶ AlBr2 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 | 1 | -1 Br_2 | 1 | -1 AlBr2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Al | 1 | -1 | ([Al])^(-1) Br_2 | 1 | -1 | ([Br2])^(-1) AlBr2 | 1 | 1 | [AlBr2] 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])^(-1) ([Br2])^(-1) [AlBr2] = ([AlBr2])/([Al] [Br2])
Rate of reaction
![Construct the rate of reaction expression for: Al + Br_2 ⟶ AlBr2 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 + Br_2 ⟶ AlBr2 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 | 1 | -1 Br_2 | 1 | -1 AlBr2 | 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 | 1 | -1 | -(Δ[Al])/(Δt) Br_2 | 1 | -1 | -(Δ[Br2])/(Δt) AlBr2 | 1 | 1 | (Δ[AlBr2])/(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[Al])/(Δt) = -(Δ[Br2])/(Δt) = (Δ[AlBr2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/366abb26edacb11dd8fcacdba893a1fd.png)
Construct the rate of reaction expression for: Al + Br_2 ⟶ AlBr2 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 + Br_2 ⟶ AlBr2 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 | 1 | -1 Br_2 | 1 | -1 AlBr2 | 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 | 1 | -1 | -(Δ[Al])/(Δt) Br_2 | 1 | -1 | -(Δ[Br2])/(Δt) AlBr2 | 1 | 1 | (Δ[AlBr2])/(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[Al])/(Δt) = -(Δ[Br2])/(Δt) = (Δ[AlBr2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| aluminum | bromine | AlBr2 formula | Al | Br_2 | AlBr2 name | aluminum | bromine | IUPAC name | aluminum | molecular bromine |
Substance properties
| aluminum | bromine | AlBr2 molar mass | 26.9815385 g/mol | 159.81 g/mol | 186.79 g/mol phase | solid (at STP) | liquid (at STP) | melting point | 660.4 °C | -7.2 °C | boiling point | 2460 °C | 58.8 °C | density | 2.7 g/cm^3 | 3.119 g/cm^3 | solubility in water | insoluble | insoluble | surface tension | 0.817 N/m | 0.0409 N/m | dynamic viscosity | 1.5×10^-4 Pa s (at 760 °C) | 9.44×10^-4 Pa s (at 25 °C) | odor | odorless | |
Units
