H2SO4 + NO = HNO3 + S

H_2SO_4 sulfuric acid + NO nitric oxide ⟶ HNO_3 nitric acid + S mixed sulfur

Balance the chemical equation algebraically: H_2SO_4 + NO ⟶ HNO_3 + S Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 NO ⟶ c_3 HNO_3 + c_4 S 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_3 O: | 4 c_1 + c_2 = 3 c_3 S: | c_1 = c_4 N: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 2 NO ⟶ 2 HNO_3 + S

+ ⟶ +

sulfuric acid + nitric oxide ⟶ nitric acid + mixed sulfur

Construct the equilibrium constant, K, expression for: H_2SO_4 + NO ⟶ HNO_3 + S 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_4 + 2 NO ⟶ 2 HNO_3 + S 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_4 | 1 | -1 NO | 2 | -2 HNO_3 | 2 | 2 S | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) NO | 2 | -2 | ([NO])^(-2) HNO_3 | 2 | 2 | ([HNO3])^2 S | 1 | 1 | [S] 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 = ([H2SO4])^(-1) ([NO])^(-2) ([HNO3])^2 [S] = (([HNO3])^2 [S])/([H2SO4] ([NO])^2)

Construct the rate of reaction expression for: H_2SO_4 + NO ⟶ HNO_3 + S 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_4 + 2 NO ⟶ 2 HNO_3 + S 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_4 | 1 | -1 NO | 2 | -2 HNO_3 | 2 | 2 S | 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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) NO | 2 | -2 | -1/2 (Δ[NO])/(Δt) HNO_3 | 2 | 2 | 1/2 (Δ[HNO3])/(Δt) S | 1 | 1 | (Δ[S])/(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[H2SO4])/(Δt) = -1/2 (Δ[NO])/(Δt) = 1/2 (Δ[HNO3])/(Δt) = (Δ[S])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | nitric oxide | nitric acid | mixed sulfur formula | H_2SO_4 | NO | HNO_3 | S Hill formula | H_2O_4S | NO | HNO_3 | S name | sulfuric acid | nitric oxide | nitric acid | mixed sulfur IUPAC name | sulfuric acid | nitric oxide | nitric acid | sulfur

| sulfuric acid | nitric oxide | nitric acid | mixed sulfur molar mass | 98.07 g/mol | 30.006 g/mol | 63.012 g/mol | 32.06 g/mol phase | liquid (at STP) | gas (at STP) | liquid (at STP) | solid (at STP) melting point | 10.371 °C | -163.6 °C | -41.6 °C | 112.8 °C boiling point | 279.6 °C | -151.7 °C | 83 °C | 444.7 °C density | 1.8305 g/cm^3 | 0.001226 g/cm^3 (at 25 °C) | 1.5129 g/cm^3 | 2.07 g/cm^3 solubility in water | very soluble | | miscible | surface tension | 0.0735 N/m | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | 1.911×10^-5 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 25 °C) | odor | odorless | | |