KOH + SO2 = KHSO3

KOH potassium hydroxide + SO_2 sulfur dioxide ⟶ KHSO3

Balance the chemical equation algebraically: KOH + SO_2 ⟶ KHSO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 SO_2 ⟶ c_3 KHSO3 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 = c_3 K: | c_1 = c_3 O: | c_1 + 2 c_2 = 3 c_3 S: | 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 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | KOH + SO_2 ⟶ KHSO3

+ ⟶ KHSO3

potassium hydroxide + sulfur dioxide ⟶ KHSO3

Construct the equilibrium constant, K, expression for: KOH + SO_2 ⟶ KHSO3 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: KOH + SO_2 ⟶ KHSO3 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 KOH | 1 | -1 SO_2 | 1 | -1 KHSO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 1 | -1 | ([KOH])^(-1) SO_2 | 1 | -1 | ([SO2])^(-1) KHSO3 | 1 | 1 | [KHSO3] 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 = ([KOH])^(-1) ([SO2])^(-1) [KHSO3] = ([KHSO3])/([KOH] [SO2])

Construct the rate of reaction expression for: KOH + SO_2 ⟶ KHSO3 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: KOH + SO_2 ⟶ KHSO3 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 KOH | 1 | -1 SO_2 | 1 | -1 KHSO3 | 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 KOH | 1 | -1 | -(Δ[KOH])/(Δt) SO_2 | 1 | -1 | -(Δ[SO2])/(Δt) KHSO3 | 1 | 1 | (Δ[KHSO3])/(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[KOH])/(Δt) = -(Δ[SO2])/(Δt) = (Δ[KHSO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium hydroxide | sulfur dioxide | KHSO3 formula | KOH | SO_2 | KHSO3 Hill formula | HKO | O_2S | HKO3S name | potassium hydroxide | sulfur dioxide |

| potassium hydroxide | sulfur dioxide | KHSO3 molar mass | 56.105 g/mol | 64.06 g/mol | 120.2 g/mol phase | solid (at STP) | gas (at STP) | melting point | 406 °C | -73 °C | boiling point | 1327 °C | -10 °C | density | 2.044 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | solubility in water | soluble | | surface tension | | 0.02859 N/m | dynamic viscosity | 0.001 Pa s (at 550 °C) | 1.282×10^-5 Pa s (at 25 °C) |