O2 + FeS = FeSO4

O_2 oxygen + FeS ferrous sulfide ⟶ FeSO_4 duretter

Balance the chemical equation algebraically: O_2 + FeS ⟶ FeSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 FeS ⟶ c_3 FeSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for O, Fe and S: O: | 2 c_1 = 4 c_3 Fe: | c_2 = c_3 S: | 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 O_2 + FeS ⟶ FeSO_4

+ ⟶

oxygen + ferrous sulfide ⟶ duretter

Construct the equilibrium constant, K, expression for: O_2 + FeS ⟶ FeSO_4 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 + FeS ⟶ FeSO_4 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 FeS | 1 | -1 FeSO_4 | 1 | 1 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) FeS | 1 | -1 | ([FeS])^(-1) FeSO_4 | 1 | 1 | [FeSO4] 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) ([FeS])^(-1) [FeSO4] = ([FeSO4])/(([O2])^2 [FeS])

Construct the rate of reaction expression for: O_2 + FeS ⟶ FeSO_4 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 + FeS ⟶ FeSO_4 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 FeS | 1 | -1 FeSO_4 | 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 O_2 | 2 | -2 | -1/2 (Δ[O2])/(Δt) FeS | 1 | -1 | -(Δ[FeS])/(Δt) FeSO_4 | 1 | 1 | (Δ[FeSO4])/(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[FeS])/(Δt) = (Δ[FeSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| oxygen | ferrous sulfide | duretter formula | O_2 | FeS | FeSO_4 Hill formula | O_2 | FeS | FeO_4S name | oxygen | ferrous sulfide | duretter IUPAC name | molecular oxygen | | iron(+2) cation sulfate

| oxygen | ferrous sulfide | duretter molar mass | 31.998 g/mol | 87.9 g/mol | 151.9 g/mol phase | gas (at STP) | solid (at STP) | melting point | -218 °C | 1195 °C | boiling point | -183 °C | | density | 0.001429 g/cm^3 (at 0 °C) | 4.84 g/cm^3 | 2.841 g/cm^3 solubility in water | | insoluble | surface tension | 0.01347 N/m | | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | 0.00343 Pa s (at 1250 °C) | odor | odorless | |