O2 + P4O6 = P2O5

O_2 oxygen + O_6P_4 tetraphosphorus(III) hexoxide ⟶ P2O5

Balance the chemical equation algebraically: O_2 + O_6P_4 ⟶ P2O5 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 O_6P_4 ⟶ c_3 P2O5 Set the number of atoms in the reactants equal to the number of atoms in the products for O and P: O: | 2 c_1 + 6 c_2 = 5 c_3 P: | 4 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 O_2 + O_6P_4 ⟶ 2 P2O5

+ ⟶ P2O5

oxygen + tetraphosphorus(III) hexoxide ⟶ P2O5

Construct the equilibrium constant, K, expression for: O_2 + O_6P_4 ⟶ P2O5 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 O_2 + O_6P_4 ⟶ 2 P2O5 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 O_2 | 2 | -2 O_6P_4 | 1 | -1 P2O5 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 2 | -2 | ([O2])^(-2) O_6P_4 | 1 | -1 | ([O6P4])^(-1) P2O5 | 2 | 2 | ([P2O5])^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 = ([O2])^(-2) ([O6P4])^(-1) ([P2O5])^2 = ([P2O5])^2/(([O2])^2 [O6P4])

Construct the rate of reaction expression for: O_2 + O_6P_4 ⟶ P2O5 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 O_2 + O_6P_4 ⟶ 2 P2O5 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 O_2 | 2 | -2 O_6P_4 | 1 | -1 P2O5 | 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 O_2 | 2 | -2 | -1/2 (Δ[O2])/(Δt) O_6P_4 | 1 | -1 | -(Δ[O6P4])/(Δt) P2O5 | 2 | 2 | 1/2 (Δ[P2O5])/(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[O2])/(Δt) = -(Δ[O6P4])/(Δt) = 1/2 (Δ[P2O5])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| oxygen | tetraphosphorus(III) hexoxide | P2O5 formula | O_2 | O_6P_4 | P2O5 Hill formula | O_2 | O_6P_4 | O5P2 name | oxygen | tetraphosphorus(III) hexoxide | IUPAC name | molecular oxygen | |

| oxygen | tetraphosphorus(III) hexoxide | P2O5 molar mass | 31.998 g/mol | 219.89 g/mol | 141.94 g/mol phase | gas (at STP) | | melting point | -218 °C | | boiling point | -183 °C | | density | 0.001429 g/cm^3 (at 0 °C) | | surface tension | 0.01347 N/m | | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | | odor | odorless | |