H2SO4 + KClO2 = K2SO4 + HClO2

H_2SO_4 sulfuric acid + KClO2 ⟶ K_2SO_4 potassium sulfate + HClO2

Balance the chemical equation algebraically: H_2SO_4 + KClO2 ⟶ K_2SO_4 + HClO2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KClO2 ⟶ c_3 K_2SO_4 + c_4 HClO2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, K and Cl: H: | 2 c_1 = c_4 O: | 4 c_1 + 2 c_2 = 4 c_3 + 2 c_4 S: | c_1 = c_3 K: | c_2 = 2 c_3 Cl: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 2 KClO2 ⟶ K_2SO_4 + 2 HClO2

+ KClO2 ⟶ + HClO2

sulfuric acid + KClO2 ⟶ potassium sulfate + HClO2

Construct the equilibrium constant, K, expression for: H_2SO_4 + KClO2 ⟶ K_2SO_4 + HClO2 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 KClO2 ⟶ K_2SO_4 + 2 HClO2 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 KClO2 | 2 | -2 K_2SO_4 | 1 | 1 HClO2 | 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_4 | 1 | -1 | ([H2SO4])^(-1) KClO2 | 2 | -2 | ([KClO2])^(-2) K_2SO_4 | 1 | 1 | [K2SO4] HClO2 | 2 | 2 | ([HClO2])^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 = ([H2SO4])^(-1) ([KClO2])^(-2) [K2SO4] ([HClO2])^2 = ([K2SO4] ([HClO2])^2)/([H2SO4] ([KClO2])^2)

Construct the rate of reaction expression for: H_2SO_4 + KClO2 ⟶ K_2SO_4 + HClO2 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 KClO2 ⟶ K_2SO_4 + 2 HClO2 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 KClO2 | 2 | -2 K_2SO_4 | 1 | 1 HClO2 | 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_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) KClO2 | 2 | -2 | -1/2 (Δ[KClO2])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) HClO2 | 2 | 2 | 1/2 (Δ[HClO2])/(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[KClO2])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[HClO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | KClO2 | potassium sulfate | HClO2 formula | H_2SO_4 | KClO2 | K_2SO_4 | HClO2 Hill formula | H_2O_4S | ClKO2 | K_2O_4S | HClO2 name | sulfuric acid | | potassium sulfate | IUPAC name | sulfuric acid | | dipotassium sulfate |

| sulfuric acid | KClO2 | potassium sulfate | HClO2 molar mass | 98.07 g/mol | 106.5 g/mol | 174.25 g/mol | 68.46 g/mol phase | liquid (at STP) | | | melting point | 10.371 °C | | | boiling point | 279.6 °C | | | density | 1.8305 g/cm^3 | | | solubility in water | very soluble | | soluble | surface tension | 0.0735 N/m | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | | odor | odorless | | |