Br2 + F2 = BrF

Br_2 bromine + F_2 fluorine ⟶ BrF

Balance the chemical equation algebraically: Br_2 + F_2 ⟶ BrF Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Br_2 + c_2 F_2 ⟶ c_3 BrF Set the number of atoms in the reactants equal to the number of atoms in the products for Br and F: Br: | 2 c_1 = c_3 F: | 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Br_2 + F_2 ⟶ 2 BrF

+ ⟶

bromine + fluorine ⟶ BrF

Construct the equilibrium constant, K, expression for: Br_2 + F_2 ⟶ BrF 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: Br_2 + F_2 ⟶ 2 BrF 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 Br_2 | 1 | -1 F_2 | 1 | -1 BrF | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Br_2 | 1 | -1 | ([Br2])^(-1) F_2 | 1 | -1 | ([F2])^(-1) BrF | 2 | 2 | ([BrF])^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 = ([Br2])^(-1) ([F2])^(-1) ([BrF])^2 = ([BrF])^2/([Br2] [F2])

Construct the rate of reaction expression for: Br_2 + F_2 ⟶ BrF 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: Br_2 + F_2 ⟶ 2 BrF 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 Br_2 | 1 | -1 F_2 | 1 | -1 BrF | 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 Br_2 | 1 | -1 | -(Δ[Br2])/(Δt) F_2 | 1 | -1 | -(Δ[F2])/(Δt) BrF | 2 | 2 | 1/2 (Δ[BrF])/(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[Br2])/(Δt) = -(Δ[F2])/(Δt) = 1/2 (Δ[BrF])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| bromine | fluorine | SMILES | BrF formula | Br_2 | F_2 | BrF name | bromine | fluorine | IUPAC name | molecular bromine | molecular fluorine |

| bromine | fluorine | SMILES | BrF molar mass | 159.81 g/mol | 37.996806326 g/mol | 98.9 g/mol phase | liquid (at STP) | gas (at STP) | melting point | -7.2 °C | -219.6 °C | -123 °C boiling point | 58.8 °C | -188.12 °C | -8.32 °C density | 3.119 g/cm^3 | 0.001696 g/cm^3 (at 0 °C) | solubility in water | insoluble | reacts | surface tension | 0.0409 N/m | | dynamic viscosity | 9.44×10^-4 Pa s (at 25 °C) | 2.344×10^-5 Pa s (at 25 °C) |