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Cl2 + KOH + K2S = H2O + K2SO4 + KCl

Input interpretation

Cl_2 chlorine + KOH potassium hydroxide + K2S ⟶ H_2O water + K_2SO_4 potassium sulfate + KCl potassium chloride
Cl_2 chlorine + KOH potassium hydroxide + K2S ⟶ H_2O water + K_2SO_4 potassium sulfate + KCl potassium chloride

Balanced equation

Balance the chemical equation algebraically: Cl_2 + KOH + K2S ⟶ 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 K2S ⟶ 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 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 8 c_3 = 1 c_4 = 4 c_5 = 1 c_6 = 8 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 Cl_2 + 8 KOH + K2S ⟶ 4 H_2O + K_2SO_4 + 8 KCl
Balance the chemical equation algebraically: Cl_2 + KOH + K2S ⟶ 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 K2S ⟶ 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 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 8 c_3 = 1 c_4 = 4 c_5 = 1 c_6 = 8 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 Cl_2 + 8 KOH + K2S ⟶ 4 H_2O + K_2SO_4 + 8 KCl

Structures

+ + K2S ⟶ + +
+ + K2S ⟶ + +

Names

chlorine + potassium hydroxide + K2S ⟶ water + potassium sulfate + potassium chloride
chlorine + potassium hydroxide + K2S ⟶ water + potassium sulfate + potassium chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: Cl_2 + KOH + K2S ⟶ 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: 4 Cl_2 + 8 KOH + K2S ⟶ 4 H_2O + K_2SO_4 + 8 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 | 4 | -4 KOH | 8 | -8 K2S | 1 | -1 H_2O | 4 | 4 K_2SO_4 | 1 | 1 KCl | 8 | 8 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 4 | -4 | ([Cl2])^(-4) KOH | 8 | -8 | ([KOH])^(-8) K2S | 1 | -1 | ([K2S])^(-1) H_2O | 4 | 4 | ([H2O])^4 K_2SO_4 | 1 | 1 | [K2SO4] KCl | 8 | 8 | ([KCl])^8 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])^(-4) ([KOH])^(-8) ([K2S])^(-1) ([H2O])^4 [K2SO4] ([KCl])^8 = (([H2O])^4 [K2SO4] ([KCl])^8)/(([Cl2])^4 ([KOH])^8 [K2S])
Construct the equilibrium constant, K, expression for: Cl_2 + KOH + K2S ⟶ 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: 4 Cl_2 + 8 KOH + K2S ⟶ 4 H_2O + K_2SO_4 + 8 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 | 4 | -4 KOH | 8 | -8 K2S | 1 | -1 H_2O | 4 | 4 K_2SO_4 | 1 | 1 KCl | 8 | 8 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 4 | -4 | ([Cl2])^(-4) KOH | 8 | -8 | ([KOH])^(-8) K2S | 1 | -1 | ([K2S])^(-1) H_2O | 4 | 4 | ([H2O])^4 K_2SO_4 | 1 | 1 | [K2SO4] KCl | 8 | 8 | ([KCl])^8 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])^(-4) ([KOH])^(-8) ([K2S])^(-1) ([H2O])^4 [K2SO4] ([KCl])^8 = (([H2O])^4 [K2SO4] ([KCl])^8)/(([Cl2])^4 ([KOH])^8 [K2S])

Rate of reaction

Construct the rate of reaction expression for: Cl_2 + KOH + K2S ⟶ 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: 4 Cl_2 + 8 KOH + K2S ⟶ 4 H_2O + K_2SO_4 + 8 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 | 4 | -4 KOH | 8 | -8 K2S | 1 | -1 H_2O | 4 | 4 K_2SO_4 | 1 | 1 KCl | 8 | 8 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 | 4 | -4 | -1/4 (Δ[Cl2])/(Δt) KOH | 8 | -8 | -1/8 (Δ[KOH])/(Δt) K2S | 1 | -1 | -(Δ[K2S])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) KCl | 8 | 8 | 1/8 (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 = -1/4 (Δ[Cl2])/(Δt) = -1/8 (Δ[KOH])/(Δt) = -(Δ[K2S])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/8 (Δ[KCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Cl_2 + KOH + K2S ⟶ 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: 4 Cl_2 + 8 KOH + K2S ⟶ 4 H_2O + K_2SO_4 + 8 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 | 4 | -4 KOH | 8 | -8 K2S | 1 | -1 H_2O | 4 | 4 K_2SO_4 | 1 | 1 KCl | 8 | 8 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 | 4 | -4 | -1/4 (Δ[Cl2])/(Δt) KOH | 8 | -8 | -1/8 (Δ[KOH])/(Δt) K2S | 1 | -1 | -(Δ[K2S])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) KCl | 8 | 8 | 1/8 (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 = -1/4 (Δ[Cl2])/(Δt) = -1/8 (Δ[KOH])/(Δt) = -(Δ[K2S])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/8 (Δ[KCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| chlorine | potassium hydroxide | K2S | water | potassium sulfate | potassium chloride formula | Cl_2 | KOH | K2S | H_2O | K_2SO_4 | KCl Hill formula | Cl_2 | HKO | K2S | H_2O | K_2O_4S | ClK name | chlorine | potassium hydroxide | | water | potassium sulfate | potassium chloride IUPAC name | molecular chlorine | potassium hydroxide | | water | dipotassium sulfate | potassium chloride
| chlorine | potassium hydroxide | K2S | water | potassium sulfate | potassium chloride formula | Cl_2 | KOH | K2S | H_2O | K_2SO_4 | KCl Hill formula | Cl_2 | HKO | K2S | H_2O | K_2O_4S | ClK name | chlorine | potassium hydroxide | | water | potassium sulfate | potassium chloride IUPAC name | molecular chlorine | potassium hydroxide | | water | dipotassium sulfate | potassium chloride

Substance properties

| chlorine | potassium hydroxide | K2S | water | potassium sulfate | potassium chloride molar mass | 70.9 g/mol | 56.105 g/mol | 110.26 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 | K2S | water | potassium sulfate | potassium chloride molar mass | 70.9 g/mol | 56.105 g/mol | 110.26 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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