HNO3 + FeS2 = H2O + H2SO4 + NO + FeNO3

HNO_3 nitric acid + FeS_2 pyrite ⟶ H_2O water + H_2SO_4 sulfuric acid + NO nitric oxide + FeNO3

Balance the chemical equation algebraically: HNO_3 + FeS_2 ⟶ H_2O + H_2SO_4 + NO + FeNO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 FeS_2 ⟶ c_3 H_2O + c_4 H_2SO_4 + c_5 NO + c_6 FeNO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, Fe and S: H: | c_1 = 2 c_3 + 2 c_4 N: | c_1 = c_5 + c_6 O: | 3 c_1 = c_3 + 4 c_4 + c_5 + 3 c_6 Fe: | c_2 = c_6 S: | 2 c_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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 3/2 c_3 = 1 c_4 = 3 c_5 = 13/2 c_6 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 16 c_2 = 3 c_3 = 2 c_4 = 6 c_5 = 13 c_6 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 16 HNO_3 + 3 FeS_2 ⟶ 2 H_2O + 6 H_2SO_4 + 13 NO + 3 FeNO3

+ ⟶ + + + FeNO3

nitric acid + pyrite ⟶ water + sulfuric acid + nitric oxide + FeNO3

Construct the equilibrium constant, K, expression for: HNO_3 + FeS_2 ⟶ H_2O + H_2SO_4 + NO + FeNO3 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: 16 HNO_3 + 3 FeS_2 ⟶ 2 H_2O + 6 H_2SO_4 + 13 NO + 3 FeNO3 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 HNO_3 | 16 | -16 FeS_2 | 3 | -3 H_2O | 2 | 2 H_2SO_4 | 6 | 6 NO | 13 | 13 FeNO3 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 16 | -16 | ([HNO3])^(-16) FeS_2 | 3 | -3 | ([FeS2])^(-3) H_2O | 2 | 2 | ([H2O])^2 H_2SO_4 | 6 | 6 | ([H2SO4])^6 NO | 13 | 13 | ([NO])^13 FeNO3 | 3 | 3 | ([FeNO3])^3 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 = ([HNO3])^(-16) ([FeS2])^(-3) ([H2O])^2 ([H2SO4])^6 ([NO])^13 ([FeNO3])^3 = (([H2O])^2 ([H2SO4])^6 ([NO])^13 ([FeNO3])^3)/(([HNO3])^16 ([FeS2])^3)

Construct the rate of reaction expression for: HNO_3 + FeS_2 ⟶ H_2O + H_2SO_4 + NO + FeNO3 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: 16 HNO_3 + 3 FeS_2 ⟶ 2 H_2O + 6 H_2SO_4 + 13 NO + 3 FeNO3 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 HNO_3 | 16 | -16 FeS_2 | 3 | -3 H_2O | 2 | 2 H_2SO_4 | 6 | 6 NO | 13 | 13 FeNO3 | 3 | 3 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 HNO_3 | 16 | -16 | -1/16 (Δ[HNO3])/(Δt) FeS_2 | 3 | -3 | -1/3 (Δ[FeS2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) H_2SO_4 | 6 | 6 | 1/6 (Δ[H2SO4])/(Δt) NO | 13 | 13 | 1/13 (Δ[NO])/(Δt) FeNO3 | 3 | 3 | 1/3 (Δ[FeNO3])/(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 = -1/16 (Δ[HNO3])/(Δt) = -1/3 (Δ[FeS2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/6 (Δ[H2SO4])/(Δt) = 1/13 (Δ[NO])/(Δt) = 1/3 (Δ[FeNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| nitric acid | pyrite | water | sulfuric acid | nitric oxide | FeNO3 formula | HNO_3 | FeS_2 | H_2O | H_2SO_4 | NO | FeNO3 Hill formula | HNO_3 | FeS_2 | H_2O | H_2O_4S | NO | FeNO3 name | nitric acid | pyrite | water | sulfuric acid | nitric oxide | IUPAC name | nitric acid | bis(sulfanylidene)iron | water | sulfuric acid | nitric oxide |