Cu + XeF4 = Xe + CuF2

Cu copper + F_4Xe_1 xenon tetrafluoride ⟶ Xe xenon + CuF_2 cupric fluoride

Balance the chemical equation algebraically: Cu + F_4Xe_1 ⟶ Xe + CuF_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cu + c_2 F_4Xe_1 ⟶ c_3 Xe + c_4 CuF_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, F and Xe: Cu: | c_1 = c_4 F: | 4 c_2 = 2 c_4 Xe: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Cu + F_4Xe_1 ⟶ Xe + 2 CuF_2

+ ⟶ +

copper + xenon tetrafluoride ⟶ xenon + cupric fluoride

Construct the equilibrium constant, K, expression for: Cu + F_4Xe_1 ⟶ Xe + CuF_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 Cu + F_4Xe_1 ⟶ Xe + 2 CuF_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 Cu | 2 | -2 F_4Xe_1 | 1 | -1 Xe | 1 | 1 CuF_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cu | 2 | -2 | ([Cu])^(-2) F_4Xe_1 | 1 | -1 | ([F4Xe1])^(-1) Xe | 1 | 1 | [Xe] CuF_2 | 2 | 2 | ([CuF2])^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 = ([Cu])^(-2) ([F4Xe1])^(-1) [Xe] ([CuF2])^2 = ([Xe] ([CuF2])^2)/(([Cu])^2 [F4Xe1])

Construct the rate of reaction expression for: Cu + F_4Xe_1 ⟶ Xe + CuF_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 Cu + F_4Xe_1 ⟶ Xe + 2 CuF_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 Cu | 2 | -2 F_4Xe_1 | 1 | -1 Xe | 1 | 1 CuF_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 Cu | 2 | -2 | -1/2 (Δ[Cu])/(Δt) F_4Xe_1 | 1 | -1 | -(Δ[F4Xe1])/(Δt) Xe | 1 | 1 | (Δ[Xe])/(Δt) CuF_2 | 2 | 2 | 1/2 (Δ[CuF2])/(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[Cu])/(Δt) = -(Δ[F4Xe1])/(Δt) = (Δ[Xe])/(Δt) = 1/2 (Δ[CuF2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| copper | xenon tetrafluoride | xenon | cupric fluoride formula | Cu | F_4Xe_1 | Xe | CuF_2 Hill formula | Cu | F_4Xe | Xe | CuF_2 name | copper | xenon tetrafluoride | xenon | cupric fluoride IUPAC name | copper | tetrafluoroxenon | xenon | difluorocopper

| copper | xenon tetrafluoride | xenon | cupric fluoride molar mass | 63.546 g/mol | 207.287 g/mol | 131.293 g/mol | 101.54 g/mol phase | solid (at STP) | | gas (at STP) | solid (at STP) melting point | 1083 °C | | -111.8 °C | 950 °C boiling point | 2567 °C | | -108 °C | 950 °C density | 8.96 g/cm^3 | | 0.0059 g/cm^3 (at 0 °C) | 4.23 g/cm^3 solubility in water | insoluble | | slightly soluble | dynamic viscosity | | | 2.306×10^-5 Pa s (at 25 °C) | odor | odorless | | odorless |