F2 + ClF3 = ClF5

F_2 fluorine + ClF_3 chlorine trifluoride ⟶ ClF_5 chlorine pentafluoride

Balance the chemical equation algebraically: F_2 + ClF_3 ⟶ ClF_5 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 F_2 + c_2 ClF_3 ⟶ c_3 ClF_5 Set the number of atoms in the reactants equal to the number of atoms in the products for F and Cl: F: | 2 c_1 + 3 c_2 = 5 c_3 Cl: | 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 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | F_2 + ClF_3 ⟶ ClF_5

+ ⟶

fluorine + chlorine trifluoride ⟶ chlorine pentafluoride

Construct the equilibrium constant, K, expression for: F_2 + ClF_3 ⟶ ClF_5 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 + ClF_3 ⟶ ClF_5 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 ClF_3 | 1 | -1 ClF_5 | 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) ClF_3 | 1 | -1 | ([ClF3])^(-1) ClF_5 | 1 | 1 | [ClF5] 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) ([ClF3])^(-1) [ClF5] = ([ClF5])/([F2] [ClF3])

Construct the rate of reaction expression for: F_2 + ClF_3 ⟶ ClF_5 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 + ClF_3 ⟶ ClF_5 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 ClF_3 | 1 | -1 ClF_5 | 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) ClF_3 | 1 | -1 | -(Δ[ClF3])/(Δt) ClF_5 | 1 | 1 | (Δ[ClF5])/(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[ClF3])/(Δt) = (Δ[ClF5])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| fluorine | chlorine trifluoride | chlorine pentafluoride formula | F_2 | ClF_3 | ClF_5 name | fluorine | chlorine trifluoride | chlorine pentafluoride IUPAC name | molecular fluorine | |

| fluorine | chlorine trifluoride | chlorine pentafluoride molar mass | 37.996806326 g/mol | 92.45 g/mol | 130.44 g/mol phase | gas (at STP) | gas (at STP) | gas (at STP) melting point | -219.6 °C | -80 °C | -90 °C boiling point | -188.12 °C | 11.8 °C | -13.1 °C density | 0.001696 g/cm^3 (at 0 °C) | 0.003779 g/cm^3 (at 25 °C) | 0.005332 g/cm^3 (at 20 °C) solubility in water | reacts | decomposes | dynamic viscosity | 2.344×10^-5 Pa s (at 25 °C) | 9.182×10^-5 Pa s (at 2727 °C) |