CoF3 = F2 + CoF2

CoF_3 cobalt trifluoride ⟶ F_2 fluorine + CoF_2 cobalt difluoride

Balance the chemical equation algebraically: CoF_3 ⟶ F_2 + CoF_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CoF_3 ⟶ c_2 F_2 + c_3 CoF_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Co and F: Co: | c_1 = c_3 F: | 3 c_1 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 CoF_3 ⟶ F_2 + 2 CoF_2

⟶ +

cobalt trifluoride ⟶ fluorine + cobalt difluoride

Construct the equilibrium constant, K, expression for: CoF_3 ⟶ F_2 + CoF_2 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 CoF_3 ⟶ F_2 + 2 CoF_2 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 CoF_3 | 2 | -2 F_2 | 1 | 1 CoF_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CoF_3 | 2 | -2 | ([CoF3])^(-2) F_2 | 1 | 1 | [F2] CoF_2 | 2 | 2 | ([CoF2])^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 = ([CoF3])^(-2) [F2] ([CoF2])^2 = ([F2] ([CoF2])^2)/([CoF3])^2

Construct the rate of reaction expression for: CoF_3 ⟶ F_2 + CoF_2 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 CoF_3 ⟶ F_2 + 2 CoF_2 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 CoF_3 | 2 | -2 F_2 | 1 | 1 CoF_2 | 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 CoF_3 | 2 | -2 | -1/2 (Δ[CoF3])/(Δt) F_2 | 1 | 1 | (Δ[F2])/(Δt) CoF_2 | 2 | 2 | 1/2 (Δ[CoF2])/(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[CoF3])/(Δt) = (Δ[F2])/(Δt) = 1/2 (Δ[CoF2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| cobalt trifluoride | fluorine | cobalt difluoride formula | CoF_3 | F_2 | CoF_2 name | cobalt trifluoride | fluorine | cobalt difluoride IUPAC name | trifluorocobalt | molecular fluorine | difluorocobalt

| cobalt trifluoride | fluorine | cobalt difluoride molar mass | 115.9284 g/mol | 37.996806326 g/mol | 96.93 g/mol phase | solid (at STP) | gas (at STP) | solid (at STP) melting point | 927 °C | -219.6 °C | 1200 °C boiling point | | -188.12 °C | density | 3.88 g/cm^3 | 0.001696 g/cm^3 (at 0 °C) | 4.43 g/cm^3 solubility in water | | reacts | dynamic viscosity | | 2.344×10^-5 Pa s (at 25 °C) |