F2 + HCCl3 = Cl2 + HCF2Cl

F_2 fluorine + HCCl3 ⟶ Cl_2 chlorine + HCF2Cl

Balance the chemical equation algebraically: F_2 + HCCl3 ⟶ Cl_2 + HCF2Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 F_2 + c_2 HCCl3 ⟶ c_3 Cl_2 + c_4 HCF2Cl Set the number of atoms in the reactants equal to the number of atoms in the products for F, H, C and Cl: F: | 2 c_1 = 2 c_4 H: | c_2 = c_4 C: | c_2 = c_4 Cl: | 3 c_2 = 2 c_3 + c_4 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 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | F_2 + HCCl3 ⟶ Cl_2 + HCF2Cl

+ HCCl3 ⟶ + HCF2Cl

fluorine + HCCl3 ⟶ chlorine + HCF2Cl

Construct the equilibrium constant, K, expression for: F_2 + HCCl3 ⟶ Cl_2 + HCF2Cl 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: F_2 + HCCl3 ⟶ Cl_2 + HCF2Cl 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 F_2 | 1 | -1 HCCl3 | 1 | -1 Cl_2 | 1 | 1 HCF2Cl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression F_2 | 1 | -1 | ([F2])^(-1) HCCl3 | 1 | -1 | ([HCCl3])^(-1) Cl_2 | 1 | 1 | [Cl2] HCF2Cl | 1 | 1 | [HCF2Cl] 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 = ([F2])^(-1) ([HCCl3])^(-1) [Cl2] [HCF2Cl] = ([Cl2] [HCF2Cl])/([F2] [HCCl3])

Construct the rate of reaction expression for: F_2 + HCCl3 ⟶ Cl_2 + HCF2Cl 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: F_2 + HCCl3 ⟶ Cl_2 + HCF2Cl 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 F_2 | 1 | -1 HCCl3 | 1 | -1 Cl_2 | 1 | 1 HCF2Cl | 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 F_2 | 1 | -1 | -(Δ[F2])/(Δt) HCCl3 | 1 | -1 | -(Δ[HCCl3])/(Δt) Cl_2 | 1 | 1 | (Δ[Cl2])/(Δt) HCF2Cl | 1 | 1 | (Δ[HCF2Cl])/(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[F2])/(Δt) = -(Δ[HCCl3])/(Δt) = (Δ[Cl2])/(Δt) = (Δ[HCF2Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| fluorine | HCCl3 | chlorine | HCF2Cl formula | F_2 | HCCl3 | Cl_2 | HCF2Cl Hill formula | F_2 | CHCl3 | Cl_2 | CHClF2 name | fluorine | | chlorine | IUPAC name | molecular fluorine | | molecular chlorine |

| fluorine | HCCl3 | chlorine | HCF2Cl molar mass | 37.996806326 g/mol | 119.4 g/mol | 70.9 g/mol | 86.47 g/mol phase | gas (at STP) | | gas (at STP) | melting point | -219.6 °C | | -101 °C | boiling point | -188.12 °C | | -34 °C | density | 0.001696 g/cm^3 (at 0 °C) | | 0.003214 g/cm^3 (at 0 °C) | solubility in water | reacts | | | dynamic viscosity | 2.344×10^-5 Pa s (at 25 °C) | | |