O2 + FeS2 = SO2 + FeO

O_2 oxygen + FeS_2 pyrite ⟶ SO_2 sulfur dioxide + FeO iron(II) oxide

Balance the chemical equation algebraically: O_2 + FeS_2 ⟶ SO_2 + FeO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 FeS_2 ⟶ c_3 SO_2 + c_4 FeO 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 = 2 c_3 + c_4 Fe: | c_2 = c_4 S: | 2 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 = 5/2 c_2 = 1 c_3 = 2 c_4 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 5 c_2 = 2 c_3 = 4 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 5 O_2 + 2 FeS_2 ⟶ 4 SO_2 + 2 FeO

+ ⟶ +

oxygen + pyrite ⟶ sulfur dioxide + iron(II) oxide

Construct the equilibrium constant, K, expression for: O_2 + FeS_2 ⟶ SO_2 + FeO 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: 5 O_2 + 2 FeS_2 ⟶ 4 SO_2 + 2 FeO 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 | 5 | -5 FeS_2 | 2 | -2 SO_2 | 4 | 4 FeO | 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 | 5 | -5 | ([O2])^(-5) FeS_2 | 2 | -2 | ([FeS2])^(-2) SO_2 | 4 | 4 | ([SO2])^4 FeO | 2 | 2 | ([FeO])^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])^(-5) ([FeS2])^(-2) ([SO2])^4 ([FeO])^2 = (([SO2])^4 ([FeO])^2)/(([O2])^5 ([FeS2])^2)

Construct the rate of reaction expression for: O_2 + FeS_2 ⟶ SO_2 + FeO 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: 5 O_2 + 2 FeS_2 ⟶ 4 SO_2 + 2 FeO 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 | 5 | -5 FeS_2 | 2 | -2 SO_2 | 4 | 4 FeO | 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 | 5 | -5 | -1/5 (Δ[O2])/(Δt) FeS_2 | 2 | -2 | -1/2 (Δ[FeS2])/(Δt) SO_2 | 4 | 4 | 1/4 (Δ[SO2])/(Δt) FeO | 2 | 2 | 1/2 (Δ[FeO])/(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 = -1/5 (Δ[O2])/(Δt) = -1/2 (Δ[FeS2])/(Δt) = 1/4 (Δ[SO2])/(Δt) = 1/2 (Δ[FeO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| oxygen | pyrite | sulfur dioxide | iron(II) oxide formula | O_2 | FeS_2 | SO_2 | FeO Hill formula | O_2 | FeS_2 | O_2S | FeO name | oxygen | pyrite | sulfur dioxide | iron(II) oxide IUPAC name | molecular oxygen | bis(sulfanylidene)iron | sulfur dioxide | oxoiron

| oxygen | pyrite | sulfur dioxide | iron(II) oxide molar mass | 31.998 g/mol | 120 g/mol | 64.06 g/mol | 71.844 g/mol phase | gas (at STP) | | gas (at STP) | solid (at STP) melting point | -218 °C | | -73 °C | 1360 °C boiling point | -183 °C | | -10 °C | density | 0.001429 g/cm^3 (at 0 °C) | 4.89 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | 5.7 g/cm^3 solubility in water | | | | insoluble surface tension | 0.01347 N/m | | 0.02859 N/m | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | | 1.282×10^-5 Pa s (at 25 °C) | odor | odorless | odorless | |