H2SO3 + HNO2 = H2O + H2SO4 + NO

H_2SO_3 sulfurous acid + HNO_2 nitrous acid ⟶ H_2O water + H_2SO_4 sulfuric acid + NO nitric oxide

Balance the chemical equation algebraically: H_2SO_3 + HNO_2 ⟶ H_2O + H_2SO_4 + NO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_3 + c_2 HNO_2 ⟶ c_3 H_2O + c_4 H_2SO_4 + c_5 NO Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and N: H: | 2 c_1 + c_2 = 2 c_3 + 2 c_4 O: | 3 c_1 + 2 c_2 = c_3 + 4 c_4 + c_5 S: | c_1 = c_4 N: | c_2 = c_5 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_3 + 2 HNO_2 ⟶ H_2O + H_2SO_4 + 2 NO

+ ⟶ + +

sulfurous acid + nitrous acid ⟶ water + sulfuric acid + nitric oxide

Construct the equilibrium constant, K, expression for: H_2SO_3 + HNO_2 ⟶ H_2O + H_2SO_4 + NO 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: H_2SO_3 + 2 HNO_2 ⟶ H_2O + H_2SO_4 + 2 NO 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 H_2SO_3 | 1 | -1 HNO_2 | 2 | -2 H_2O | 1 | 1 H_2SO_4 | 1 | 1 NO | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_3 | 1 | -1 | ([H2SO3])^(-1) HNO_2 | 2 | -2 | ([HNO2])^(-2) H_2O | 1 | 1 | [H2O] H_2SO_4 | 1 | 1 | [H2SO4] NO | 2 | 2 | ([NO])^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 = ([H2SO3])^(-1) ([HNO2])^(-2) [H2O] [H2SO4] ([NO])^2 = ([H2O] [H2SO4] ([NO])^2)/([H2SO3] ([HNO2])^2)

Construct the rate of reaction expression for: H_2SO_3 + HNO_2 ⟶ H_2O + H_2SO_4 + NO 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: H_2SO_3 + 2 HNO_2 ⟶ H_2O + H_2SO_4 + 2 NO 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 H_2SO_3 | 1 | -1 HNO_2 | 2 | -2 H_2O | 1 | 1 H_2SO_4 | 1 | 1 NO | 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 H_2SO_3 | 1 | -1 | -(Δ[H2SO3])/(Δt) HNO_2 | 2 | -2 | -1/2 (Δ[HNO2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) H_2SO_4 | 1 | 1 | (Δ[H2SO4])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(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 = -(Δ[H2SO3])/(Δt) = -1/2 (Δ[HNO2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[H2SO4])/(Δt) = 1/2 (Δ[NO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfurous acid | nitrous acid | water | sulfuric acid | nitric oxide formula | H_2SO_3 | HNO_2 | H_2O | H_2SO_4 | NO Hill formula | H_2O_3S | HNO_2 | H_2O | H_2O_4S | NO name | sulfurous acid | nitrous acid | water | sulfuric acid | nitric oxide