Search

Cl2 + KOH = H2O + KCl + KOCl

Input interpretation

Cl_2 chlorine + KOH potassium hydroxide ⟶ H_2O water + KCl potassium chloride + KOCl
Cl_2 chlorine + KOH potassium hydroxide ⟶ H_2O water + KCl potassium chloride + KOCl

Balanced equation

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

Structures

+ ⟶ + + KOCl
+ ⟶ + + KOCl

Names

chlorine + potassium hydroxide ⟶ water + potassium chloride + KOCl
chlorine + potassium hydroxide ⟶ water + potassium chloride + KOCl

Equilibrium constant

Construct the equilibrium constant, K, expression for: Cl_2 + KOH ⟶ H_2O + KCl + KOCl 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 ⟶ H_2O + KCl + KOCl 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 H_2O | 1 | 1 KCl | 1 | 1 KOCl | 1 | 1 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) H_2O | 1 | 1 | [H2O] KCl | 1 | 1 | [KCl] KOCl | 1 | 1 | [KOCl] 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) [H2O] [KCl] [KOCl] = ([H2O] [KCl] [KOCl])/([Cl2] ([KOH])^2)
Construct the equilibrium constant, K, expression for: Cl_2 + KOH ⟶ H_2O + KCl + KOCl 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 ⟶ H_2O + KCl + KOCl 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 H_2O | 1 | 1 KCl | 1 | 1 KOCl | 1 | 1 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) H_2O | 1 | 1 | [H2O] KCl | 1 | 1 | [KCl] KOCl | 1 | 1 | [KOCl] 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) [H2O] [KCl] [KOCl] = ([H2O] [KCl] [KOCl])/([Cl2] ([KOH])^2)

Rate of reaction

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

Chemical names and formulas

| chlorine | potassium hydroxide | water | potassium chloride | KOCl formula | Cl_2 | KOH | H_2O | KCl | KOCl Hill formula | Cl_2 | HKO | H_2O | ClK | ClKO name | chlorine | potassium hydroxide | water | potassium chloride | IUPAC name | molecular chlorine | potassium hydroxide | water | potassium chloride |
| chlorine | potassium hydroxide | water | potassium chloride | KOCl formula | Cl_2 | KOH | H_2O | KCl | KOCl Hill formula | Cl_2 | HKO | H_2O | ClK | ClKO name | chlorine | potassium hydroxide | water | potassium chloride | IUPAC name | molecular chlorine | potassium hydroxide | water | potassium chloride |

Substance properties

| chlorine | potassium hydroxide | water | potassium chloride | KOCl molar mass | 70.9 g/mol | 56.105 g/mol | 18.015 g/mol | 74.55 g/mol | 90.55 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 | 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 | water | potassium chloride | KOCl molar mass | 70.9 g/mol | 56.105 g/mol | 18.015 g/mol | 74.55 g/mol | 90.55 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 | 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

Random Queries

crystal system of loveringite
formula of hydronium cation vs sulfate anion
chemical types of carbon monoxide vs hydrogen
Curie point of period 4 elements
molar mass of calcium nitride
molar mass of potassium 3-formylphenyltrifluoroborate
names of sucrose
formula of propanoate anion
mass fractions of sodium metatungstate hydrate
molar mass of D-galactose-1-d