H2O + F2 = HF + F2O

H_2O water + F_2 fluorine ⟶ HF hydrogen fluoride + F_2O oxygen difluoride

Balance the chemical equation algebraically: H_2O + F_2 ⟶ HF + F_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 F_2 ⟶ c_3 HF + c_4 F_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and F: H: | 2 c_1 = c_3 O: | c_1 = c_4 F: | 2 c_2 = c_3 + 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 = 2 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + 2 F_2 ⟶ 2 HF + F_2O

+ ⟶ +

water + fluorine ⟶ hydrogen fluoride + oxygen difluoride

| water | fluorine | hydrogen fluoride | oxygen difluoride molecular enthalpy | -285.8 kJ/mol | 0 kJ/mol | -273.3 kJ/mol | 109 kJ/mol total enthalpy | -285.8 kJ/mol | 0 kJ/mol | -546.6 kJ/mol | 109 kJ/mol | H_initial = -285.8 kJ/mol | | H_final = -437.6 kJ/mol | ΔH_rxn^0 | -437.6 kJ/mol - -285.8 kJ/mol = -151.8 kJ/mol (exothermic) | | |

| water | fluorine | hydrogen fluoride | oxygen difluoride molecular free energy | -237.1 kJ/mol | 0 kJ/mol | -275.4 kJ/mol | 105.3 kJ/mol total free energy | -237.1 kJ/mol | 0 kJ/mol | -550.8 kJ/mol | 105.3 kJ/mol | G_initial = -237.1 kJ/mol | | G_final = -445.5 kJ/mol | ΔG_rxn^0 | -445.5 kJ/mol - -237.1 kJ/mol = -208.4 kJ/mol (exergonic) | | |

| water | fluorine | hydrogen fluoride | oxygen difluoride molecular entropy | 69.91 J/(mol K) | 202.8 J/(mol K) | 173.8 J/(mol K) | 216.4 J/(mol K) total entropy | 69.91 J/(mol K) | 405.6 J/(mol K) | 347.6 J/(mol K) | 216.4 J/(mol K) | S_initial = 475.5 J/(mol K) | | S_final = 564 J/(mol K) | ΔS_rxn^0 | 564 J/(mol K) - 475.5 J/(mol K) = 88.49 J/(mol K) (endoentropic) | | |

Construct the equilibrium constant, K, expression for: H_2O + F_2 ⟶ HF + F_2O 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: H_2O + 2 F_2 ⟶ 2 HF + F_2O 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 H_2O | 1 | -1 F_2 | 2 | -2 HF | 2 | 2 F_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) F_2 | 2 | -2 | ([F2])^(-2) HF | 2 | 2 | ([HF])^2 F_2O | 1 | 1 | [F2O] 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 = ([H2O])^(-1) ([F2])^(-2) ([HF])^2 [F2O] = (([HF])^2 [F2O])/([H2O] ([F2])^2)

Construct the rate of reaction expression for: H_2O + F_2 ⟶ HF + F_2O 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: H_2O + 2 F_2 ⟶ 2 HF + F_2O 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 H_2O | 1 | -1 F_2 | 2 | -2 HF | 2 | 2 F_2O | 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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) F_2 | 2 | -2 | -1/2 (Δ[F2])/(Δt) HF | 2 | 2 | 1/2 (Δ[HF])/(Δt) F_2O | 1 | 1 | (Δ[F2O])/(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[H2O])/(Δt) = -1/2 (Δ[F2])/(Δt) = 1/2 (Δ[HF])/(Δt) = (Δ[F2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| water | fluorine | hydrogen fluoride | oxygen difluoride formula | H_2O | F_2 | HF | F_2O Hill formula | H_2O | F_2 | FH | F_2O name | water | fluorine | hydrogen fluoride | oxygen difluoride IUPAC name | water | molecular fluorine | hydrogen fluoride | fluoro hypofluorite

| water | fluorine | hydrogen fluoride | oxygen difluoride molar mass | 18.015 g/mol | 37.996806326 g/mol | 20.006 g/mol | 53.996 g/mol phase | liquid (at STP) | gas (at STP) | gas (at STP) | gas (at STP) melting point | 0 °C | -219.6 °C | -83.36 °C | -223.9 °C boiling point | 99.9839 °C | -188.12 °C | 19.5 °C | -145 °C density | 1 g/cm^3 | 0.001696 g/cm^3 (at 0 °C) | 8.18×10^-4 g/cm^3 (at 25 °C) | 0.002207 g/cm^3 (at 25 °C) solubility in water | | reacts | miscible | surface tension | 0.0728 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 2.344×10^-5 Pa s (at 25 °C) | 1.2571×10^-5 Pa s (at 20 °C) | odor | odorless | | |