KHSO4 = H2O + SO3 + K2O

KHSO_4 potassium bisulfate ⟶ H_2O water + SO_3 sulfur trioxide + K_2O potassium oxide

Balance the chemical equation algebraically: KHSO_4 ⟶ H_2O + SO_3 + K_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KHSO_4 ⟶ c_2 H_2O + c_3 SO_3 + c_4 K_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O and S: H: | c_1 = 2 c_2 K: | c_1 = 2 c_4 O: | 4 c_1 = c_2 + 3 c_3 + c_4 S: | c_1 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KHSO_4 ⟶ H_2O + 2 SO_3 + K_2O

⟶ + +

potassium bisulfate ⟶ water + sulfur trioxide + potassium oxide

Construct the equilibrium constant, K, expression for: KHSO_4 ⟶ H_2O + SO_3 + K_2O 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: 2 KHSO_4 ⟶ H_2O + 2 SO_3 + K_2O 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 KHSO_4 | 2 | -2 H_2O | 1 | 1 SO_3 | 2 | 2 K_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KHSO_4 | 2 | -2 | ([KHSO4])^(-2) H_2O | 1 | 1 | [H2O] SO_3 | 2 | 2 | ([SO3])^2 K_2O | 1 | 1 | [K2O] 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 = ([KHSO4])^(-2) [H2O] ([SO3])^2 [K2O] = ([H2O] ([SO3])^2 [K2O])/([KHSO4])^2

Construct the rate of reaction expression for: KHSO_4 ⟶ H_2O + SO_3 + K_2O 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: 2 KHSO_4 ⟶ H_2O + 2 SO_3 + K_2O 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 KHSO_4 | 2 | -2 H_2O | 1 | 1 SO_3 | 2 | 2 K_2O | 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 KHSO_4 | 2 | -2 | -1/2 (Δ[KHSO4])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) SO_3 | 2 | 2 | 1/2 (Δ[SO3])/(Δt) K_2O | 1 | 1 | (Δ[K2O])/(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 = -1/2 (Δ[KHSO4])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[SO3])/(Δt) = (Δ[K2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium bisulfate | water | sulfur trioxide | potassium oxide formula | KHSO_4 | H_2O | SO_3 | K_2O Hill formula | HKO_4S | H_2O | O_3S | K_2O name | potassium bisulfate | water | sulfur trioxide | potassium oxide IUPAC name | potassium hydrogen sulfate | water | sulfur trioxide | dipotassium oxygen(2-)

| potassium bisulfate | water | sulfur trioxide | potassium oxide molar mass | 136.16 g/mol | 18.015 g/mol | 80.06 g/mol | 94.196 g/mol phase | solid (at STP) | liquid (at STP) | liquid (at STP) | melting point | 214 °C | 0 °C | 16.8 °C | boiling point | | 99.9839 °C | 44.7 °C | density | 2.32 g/cm^3 | 1 g/cm^3 | 1.97 g/cm^3 | solubility in water | | | reacts | surface tension | | 0.0728 N/m | | dynamic viscosity | | 8.9×10^-4 Pa s (at 25 °C) | 0.00159 Pa s (at 30 °C) | odor | | odorless | |