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KClO3 + H2SO3 = H2SO4 + KCl

Input interpretation

KClO_3 potassium chlorate + H_2SO_3 sulfurous acid ⟶ H_2SO_4 sulfuric acid + KCl potassium chloride
KClO_3 potassium chlorate + H_2SO_3 sulfurous acid ⟶ H_2SO_4 sulfuric acid + KCl potassium chloride

Balanced equation

Balance the chemical equation algebraically: KClO_3 + H_2SO_3 ⟶ H_2SO_4 + KCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KClO_3 + c_2 H_2SO_3 ⟶ c_3 H_2SO_4 + c_4 KCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, K, O, H and S: Cl: | c_1 = c_4 K: | c_1 = c_4 O: | 3 c_1 + 3 c_2 = 4 c_3 H: | 2 c_2 = 2 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 = 3 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | KClO_3 + 3 H_2SO_3 ⟶ 3 H_2SO_4 + KCl
Balance the chemical equation algebraically: KClO_3 + H_2SO_3 ⟶ H_2SO_4 + KCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KClO_3 + c_2 H_2SO_3 ⟶ c_3 H_2SO_4 + c_4 KCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, K, O, H and S: Cl: | c_1 = c_4 K: | c_1 = c_4 O: | 3 c_1 + 3 c_2 = 4 c_3 H: | 2 c_2 = 2 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 = 3 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | KClO_3 + 3 H_2SO_3 ⟶ 3 H_2SO_4 + KCl

Structures

+ ⟶ +
+ ⟶ +

Names

potassium chlorate + sulfurous acid ⟶ sulfuric acid + potassium chloride
potassium chlorate + sulfurous acid ⟶ sulfuric acid + potassium chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: KClO_3 + H_2SO_3 ⟶ H_2SO_4 + KCl 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: KClO_3 + 3 H_2SO_3 ⟶ 3 H_2SO_4 + KCl 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 KClO_3 | 1 | -1 H_2SO_3 | 3 | -3 H_2SO_4 | 3 | 3 KCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KClO_3 | 1 | -1 | ([KClO3])^(-1) H_2SO_3 | 3 | -3 | ([H2SO3])^(-3) H_2SO_4 | 3 | 3 | ([H2SO4])^3 KCl | 1 | 1 | [KCl] 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 = ([KClO3])^(-1) ([H2SO3])^(-3) ([H2SO4])^3 [KCl] = (([H2SO4])^3 [KCl])/([KClO3] ([H2SO3])^3)
Construct the equilibrium constant, K, expression for: KClO_3 + H_2SO_3 ⟶ H_2SO_4 + KCl 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: KClO_3 + 3 H_2SO_3 ⟶ 3 H_2SO_4 + KCl 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 KClO_3 | 1 | -1 H_2SO_3 | 3 | -3 H_2SO_4 | 3 | 3 KCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KClO_3 | 1 | -1 | ([KClO3])^(-1) H_2SO_3 | 3 | -3 | ([H2SO3])^(-3) H_2SO_4 | 3 | 3 | ([H2SO4])^3 KCl | 1 | 1 | [KCl] 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 = ([KClO3])^(-1) ([H2SO3])^(-3) ([H2SO4])^3 [KCl] = (([H2SO4])^3 [KCl])/([KClO3] ([H2SO3])^3)

Rate of reaction

Construct the rate of reaction expression for: KClO_3 + H_2SO_3 ⟶ H_2SO_4 + KCl 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: KClO_3 + 3 H_2SO_3 ⟶ 3 H_2SO_4 + KCl 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 KClO_3 | 1 | -1 H_2SO_3 | 3 | -3 H_2SO_4 | 3 | 3 KCl | 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 KClO_3 | 1 | -1 | -(Δ[KClO3])/(Δt) H_2SO_3 | 3 | -3 | -1/3 (Δ[H2SO3])/(Δt) H_2SO_4 | 3 | 3 | 1/3 (Δ[H2SO4])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(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[KClO3])/(Δt) = -1/3 (Δ[H2SO3])/(Δt) = 1/3 (Δ[H2SO4])/(Δt) = (Δ[KCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KClO_3 + H_2SO_3 ⟶ H_2SO_4 + KCl 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: KClO_3 + 3 H_2SO_3 ⟶ 3 H_2SO_4 + KCl 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 KClO_3 | 1 | -1 H_2SO_3 | 3 | -3 H_2SO_4 | 3 | 3 KCl | 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 KClO_3 | 1 | -1 | -(Δ[KClO3])/(Δt) H_2SO_3 | 3 | -3 | -1/3 (Δ[H2SO3])/(Δt) H_2SO_4 | 3 | 3 | 1/3 (Δ[H2SO4])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(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[KClO3])/(Δt) = -1/3 (Δ[H2SO3])/(Δt) = 1/3 (Δ[H2SO4])/(Δt) = (Δ[KCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium chlorate | sulfurous acid | sulfuric acid | potassium chloride formula | KClO_3 | H_2SO_3 | H_2SO_4 | KCl Hill formula | ClKO_3 | H_2O_3S | H_2O_4S | ClK name | potassium chlorate | sulfurous acid | sulfuric acid | potassium chloride
| potassium chlorate | sulfurous acid | sulfuric acid | potassium chloride formula | KClO_3 | H_2SO_3 | H_2SO_4 | KCl Hill formula | ClKO_3 | H_2O_3S | H_2O_4S | ClK name | potassium chlorate | sulfurous acid | sulfuric acid | potassium chloride

Substance properties

| potassium chlorate | sulfurous acid | sulfuric acid | potassium chloride molar mass | 122.5 g/mol | 82.07 g/mol | 98.07 g/mol | 74.55 g/mol phase | solid (at STP) | | liquid (at STP) | solid (at STP) melting point | 356 °C | | 10.371 °C | 770 °C boiling point | | | 279.6 °C | 1420 °C density | 2.34 g/cm^3 | 1.03 g/cm^3 | 1.8305 g/cm^3 | 1.98 g/cm^3 solubility in water | soluble | very soluble | very soluble | soluble surface tension | | | 0.0735 N/m | dynamic viscosity | | | 0.021 Pa s (at 25 °C) | odor | | | odorless | odorless
| potassium chlorate | sulfurous acid | sulfuric acid | potassium chloride molar mass | 122.5 g/mol | 82.07 g/mol | 98.07 g/mol | 74.55 g/mol phase | solid (at STP) | | liquid (at STP) | solid (at STP) melting point | 356 °C | | 10.371 °C | 770 °C boiling point | | | 279.6 °C | 1420 °C density | 2.34 g/cm^3 | 1.03 g/cm^3 | 1.8305 g/cm^3 | 1.98 g/cm^3 solubility in water | soluble | very soluble | very soluble | soluble surface tension | | | 0.0735 N/m | dynamic viscosity | | | 0.021 Pa s (at 25 °C) | odor | | | odorless | odorless

Units

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