CaCl2 + F2 = Cl2 + CaF2

CaCl_2 calcium chloride + F_2 fluorine ⟶ Cl_2 chlorine + CaF_2 calcium fluoride

Balance the chemical equation algebraically: CaCl_2 + F_2 ⟶ Cl_2 + CaF_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CaCl_2 + c_2 F_2 ⟶ c_3 Cl_2 + c_4 CaF_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, Cl and F: Ca: | c_1 = c_4 Cl: | 2 c_1 = 2 c_3 F: | 2 c_2 = 2 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: | | CaCl_2 + F_2 ⟶ Cl_2 + CaF_2

+ ⟶ +

calcium chloride + fluorine ⟶ chlorine + calcium fluoride

| calcium chloride | fluorine | chlorine | calcium fluoride molecular enthalpy | -795.4 kJ/mol | 0 kJ/mol | 0 kJ/mol | -1228 kJ/mol total enthalpy | -795.4 kJ/mol | 0 kJ/mol | 0 kJ/mol | -1228 kJ/mol | H_initial = -795.4 kJ/mol | | H_final = -1228 kJ/mol | ΔH_rxn^0 | -1228 kJ/mol - -795.4 kJ/mol = -432.6 kJ/mol (exothermic) | | |

| calcium chloride | fluorine | chlorine | calcium fluoride molecular free energy | -748.8 kJ/mol | 0 kJ/mol | 0 kJ/mol | -1176 kJ/mol total free energy | -748.8 kJ/mol | 0 kJ/mol | 0 kJ/mol | -1176 kJ/mol | G_initial = -748.8 kJ/mol | | G_final = -1176 kJ/mol | ΔG_rxn^0 | -1176 kJ/mol - -748.8 kJ/mol = -426.8 kJ/mol (exergonic) | | |

Construct the equilibrium constant, K, expression for: CaCl_2 + F_2 ⟶ Cl_2 + CaF_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: CaCl_2 + F_2 ⟶ Cl_2 + CaF_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 CaCl_2 | 1 | -1 F_2 | 1 | -1 Cl_2 | 1 | 1 CaF_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CaCl_2 | 1 | -1 | ([CaCl2])^(-1) F_2 | 1 | -1 | ([F2])^(-1) Cl_2 | 1 | 1 | [Cl2] CaF_2 | 1 | 1 | [CaF2] 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 = ([CaCl2])^(-1) ([F2])^(-1) [Cl2] [CaF2] = ([Cl2] [CaF2])/([CaCl2] [F2])

Construct the rate of reaction expression for: CaCl_2 + F_2 ⟶ Cl_2 + CaF_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: CaCl_2 + F_2 ⟶ Cl_2 + CaF_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 CaCl_2 | 1 | -1 F_2 | 1 | -1 Cl_2 | 1 | 1 CaF_2 | 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 CaCl_2 | 1 | -1 | -(Δ[CaCl2])/(Δt) F_2 | 1 | -1 | -(Δ[F2])/(Δt) Cl_2 | 1 | 1 | (Δ[Cl2])/(Δt) CaF_2 | 1 | 1 | (Δ[CaF2])/(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[CaCl2])/(Δt) = -(Δ[F2])/(Δt) = (Δ[Cl2])/(Δt) = (Δ[CaF2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| calcium chloride | fluorine | chlorine | calcium fluoride formula | CaCl_2 | F_2 | Cl_2 | CaF_2 name | calcium chloride | fluorine | chlorine | calcium fluoride IUPAC name | calcium dichloride | molecular fluorine | molecular chlorine | calcium difluoride

| calcium chloride | fluorine | chlorine | calcium fluoride molar mass | 111 g/mol | 37.996806326 g/mol | 70.9 g/mol | 78.075 g/mol phase | solid (at STP) | gas (at STP) | gas (at STP) | solid (at STP) melting point | 772 °C | -219.6 °C | -101 °C | 1418 °C boiling point | | -188.12 °C | -34 °C | 2500 °C density | 2.15 g/cm^3 | 0.001696 g/cm^3 (at 0 °C) | 0.003214 g/cm^3 (at 0 °C) | 3.18 g/cm^3 solubility in water | soluble | reacts | | dynamic viscosity | | 2.344×10^-5 Pa s (at 25 °C) | |