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Cl2 + KOH + K2SO3 = H2O + K2SO4 + KCl

Input interpretation

Cl_2 chlorine + KOH potassium hydroxide + K_2SO_3 potassium sulfite ⟶ H_2O water + K_2SO_4 potassium sulfate + KCl potassium chloride
Cl_2 chlorine + KOH potassium hydroxide + K_2SO_3 potassium sulfite ⟶ H_2O water + K_2SO_4 potassium sulfate + KCl potassium chloride

Balanced equation

Balance the chemical equation algebraically: Cl_2 + KOH + K_2SO_3 ⟶ H_2O + K_2SO_4 + KCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 KOH + c_3 K_2SO_3 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 KCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, K, O and S: Cl: | 2 c_1 = c_6 H: | c_2 = 2 c_4 K: | c_2 + 2 c_3 = 2 c_5 + c_6 O: | c_2 + 3 c_3 = c_4 + 4 c_5 S: | c_3 = c_5 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 c_5 = 1 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Cl_2 + 2 KOH + K_2SO_3 ⟶ H_2O + K_2SO_4 + 2 KCl
Balance the chemical equation algebraically: Cl_2 + KOH + K_2SO_3 ⟶ H_2O + K_2SO_4 + KCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 KOH + c_3 K_2SO_3 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 KCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, K, O and S: Cl: | 2 c_1 = c_6 H: | c_2 = 2 c_4 K: | c_2 + 2 c_3 = 2 c_5 + c_6 O: | c_2 + 3 c_3 = c_4 + 4 c_5 S: | c_3 = c_5 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 c_5 = 1 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Cl_2 + 2 KOH + K_2SO_3 ⟶ H_2O + K_2SO_4 + 2 KCl

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

chlorine + potassium hydroxide + potassium sulfite ⟶ water + potassium sulfate + potassium chloride
chlorine + potassium hydroxide + potassium sulfite ⟶ water + potassium sulfate + potassium chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: Cl_2 + KOH + K_2SO_3 ⟶ H_2O + K_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: Cl_2 + 2 KOH + K_2SO_3 ⟶ H_2O + K_2SO_4 + 2 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 Cl_2 | 1 | -1 KOH | 2 | -2 K_2SO_3 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 KCl | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 1 | -1 | ([Cl2])^(-1) KOH | 2 | -2 | ([KOH])^(-2) K_2SO_3 | 1 | -1 | ([K2SO3])^(-1) H_2O | 1 | 1 | [H2O] K_2SO_4 | 1 | 1 | [K2SO4] KCl | 2 | 2 | ([KCl])^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 = ([Cl2])^(-1) ([KOH])^(-2) ([K2SO3])^(-1) [H2O] [K2SO4] ([KCl])^2 = ([H2O] [K2SO4] ([KCl])^2)/([Cl2] ([KOH])^2 [K2SO3])
Construct the equilibrium constant, K, expression for: Cl_2 + KOH + K_2SO_3 ⟶ H_2O + K_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: Cl_2 + 2 KOH + K_2SO_3 ⟶ H_2O + K_2SO_4 + 2 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 Cl_2 | 1 | -1 KOH | 2 | -2 K_2SO_3 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 KCl | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 1 | -1 | ([Cl2])^(-1) KOH | 2 | -2 | ([KOH])^(-2) K_2SO_3 | 1 | -1 | ([K2SO3])^(-1) H_2O | 1 | 1 | [H2O] K_2SO_4 | 1 | 1 | [K2SO4] KCl | 2 | 2 | ([KCl])^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 = ([Cl2])^(-1) ([KOH])^(-2) ([K2SO3])^(-1) [H2O] [K2SO4] ([KCl])^2 = ([H2O] [K2SO4] ([KCl])^2)/([Cl2] ([KOH])^2 [K2SO3])

Rate of reaction

Construct the rate of reaction expression for: Cl_2 + KOH + K_2SO_3 ⟶ H_2O + K_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: Cl_2 + 2 KOH + K_2SO_3 ⟶ H_2O + K_2SO_4 + 2 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 Cl_2 | 1 | -1 KOH | 2 | -2 K_2SO_3 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 KCl | 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 Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) K_2SO_3 | 1 | -1 | -(Δ[K2SO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) KCl | 2 | 2 | 1/2 (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[Cl2])/(Δt) = -1/2 (Δ[KOH])/(Δt) = -(Δ[K2SO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[KCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Cl_2 + KOH + K_2SO_3 ⟶ H_2O + K_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: Cl_2 + 2 KOH + K_2SO_3 ⟶ H_2O + K_2SO_4 + 2 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 Cl_2 | 1 | -1 KOH | 2 | -2 K_2SO_3 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 KCl | 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 Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) K_2SO_3 | 1 | -1 | -(Δ[K2SO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) KCl | 2 | 2 | 1/2 (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[Cl2])/(Δt) = -1/2 (Δ[KOH])/(Δt) = -(Δ[K2SO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[KCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| chlorine | potassium hydroxide | potassium sulfite | water | potassium sulfate | potassium chloride formula | Cl_2 | KOH | K_2SO_3 | H_2O | K_2SO_4 | KCl Hill formula | Cl_2 | HKO | K_2O_3S | H_2O | K_2O_4S | ClK name | chlorine | potassium hydroxide | potassium sulfite | water | potassium sulfate | potassium chloride IUPAC name | molecular chlorine | potassium hydroxide | dipotassium sulfite | water | dipotassium sulfate | potassium chloride
| chlorine | potassium hydroxide | potassium sulfite | water | potassium sulfate | potassium chloride formula | Cl_2 | KOH | K_2SO_3 | H_2O | K_2SO_4 | KCl Hill formula | Cl_2 | HKO | K_2O_3S | H_2O | K_2O_4S | ClK name | chlorine | potassium hydroxide | potassium sulfite | water | potassium sulfate | potassium chloride IUPAC name | molecular chlorine | potassium hydroxide | dipotassium sulfite | water | dipotassium sulfate | potassium chloride

Substance properties

| chlorine | potassium hydroxide | potassium sulfite | water | potassium sulfate | potassium chloride molar mass | 70.9 g/mol | 56.105 g/mol | 158.25 g/mol | 18.015 g/mol | 174.25 g/mol | 74.55 g/mol phase | gas (at STP) | solid (at STP) | | liquid (at STP) | | solid (at STP) melting point | -101 °C | 406 °C | | 0 °C | | 770 °C boiling point | -34 °C | 1327 °C | | 99.9839 °C | | 1420 °C density | 0.003214 g/cm^3 (at 0 °C) | 2.044 g/cm^3 | | 1 g/cm^3 | | 1.98 g/cm^3 solubility in water | | soluble | | | soluble | soluble surface tension | | | | 0.0728 N/m | | dynamic viscosity | | 0.001 Pa s (at 550 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | | odorless | | odorless
| chlorine | potassium hydroxide | potassium sulfite | water | potassium sulfate | potassium chloride molar mass | 70.9 g/mol | 56.105 g/mol | 158.25 g/mol | 18.015 g/mol | 174.25 g/mol | 74.55 g/mol phase | gas (at STP) | solid (at STP) | | liquid (at STP) | | solid (at STP) melting point | -101 °C | 406 °C | | 0 °C | | 770 °C boiling point | -34 °C | 1327 °C | | 99.9839 °C | | 1420 °C density | 0.003214 g/cm^3 (at 0 °C) | 2.044 g/cm^3 | | 1 g/cm^3 | | 1.98 g/cm^3 solubility in water | | soluble | | | soluble | soluble surface tension | | | | 0.0728 N/m | | dynamic viscosity | | 0.001 Pa s (at 550 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | | odorless | | odorless

Units

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