H2SO4 = O2 + H2 + S

H_2SO_4 sulfuric acid ⟶ O_2 oxygen + H_2 hydrogen + S mixed sulfur

Balance the chemical equation algebraically: H_2SO_4 ⟶ O_2 + H_2 + S Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 ⟶ c_2 O_2 + c_3 H_2 + c_4 S Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and S: H: | 2 c_1 = 2 c_3 O: | 4 c_1 = 2 c_2 S: | c_1 = 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 ⟶ 2 O_2 + H_2 + S

⟶ + +

sulfuric acid ⟶ oxygen + hydrogen + mixed sulfur

Construct the equilibrium constant, K, expression for: H_2SO_4 ⟶ O_2 + H_2 + 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 O_2 + H_2 + 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 O_2 | 2 | 2 H_2 | 1 | 1 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) O_2 | 2 | 2 | ([O2])^2 H_2 | 1 | 1 | [H2] 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) ([O2])^2 [H2] [S] = (([O2])^2 [H2] [S])/([H2SO4])

Construct the rate of reaction expression for: H_2SO_4 ⟶ O_2 + H_2 + 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 O_2 + H_2 + 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 O_2 | 2 | 2 H_2 | 1 | 1 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) O_2 | 2 | 2 | 1/2 (Δ[O2])/(Δt) H_2 | 1 | 1 | (Δ[H2])/(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[O2])/(Δt) = (Δ[H2])/(Δt) = (Δ[S])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | oxygen | hydrogen | mixed sulfur formula | H_2SO_4 | O_2 | H_2 | S Hill formula | H_2O_4S | O_2 | H_2 | S name | sulfuric acid | oxygen | hydrogen | mixed sulfur IUPAC name | sulfuric acid | molecular oxygen | molecular hydrogen | sulfur

| sulfuric acid | oxygen | hydrogen | mixed sulfur molar mass | 98.07 g/mol | 31.998 g/mol | 2.016 g/mol | 32.06 g/mol phase | liquid (at STP) | gas (at STP) | gas (at STP) | solid (at STP) melting point | 10.371 °C | -218 °C | -259.2 °C | 112.8 °C boiling point | 279.6 °C | -183 °C | -252.8 °C | 444.7 °C density | 1.8305 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 8.99×10^-5 g/cm^3 (at 0 °C) | 2.07 g/cm^3 solubility in water | very soluble | | | surface tension | 0.0735 N/m | 0.01347 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | 8.9×10^-6 Pa s (at 25 °C) | odor | odorless | odorless | odorless |