Search

KOH + Br2 = H2O + KBr + KBrO

Input interpretation

KOH potassium hydroxide + Br_2 bromine ⟶ H_2O water + KBr potassium bromide + KBrO
KOH potassium hydroxide + Br_2 bromine ⟶ H_2O water + KBr potassium bromide + KBrO

Balanced equation

Balance the chemical equation algebraically: KOH + Br_2 ⟶ H_2O + KBr + KBrO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 Br_2 ⟶ c_3 H_2O + c_4 KBr + c_5 KBrO Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O and Br: H: | c_1 = 2 c_3 K: | c_1 = c_4 + c_5 O: | c_1 = c_3 + c_5 Br: | 2 c_2 = c_4 + 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + Br_2 ⟶ H_2O + KBr + KBrO
Balance the chemical equation algebraically: KOH + Br_2 ⟶ H_2O + KBr + KBrO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 Br_2 ⟶ c_3 H_2O + c_4 KBr + c_5 KBrO Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O and Br: H: | c_1 = 2 c_3 K: | c_1 = c_4 + c_5 O: | c_1 = c_3 + c_5 Br: | 2 c_2 = c_4 + 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + Br_2 ⟶ H_2O + KBr + KBrO

Structures

+ ⟶ + + KBrO
+ ⟶ + + KBrO

Names

potassium hydroxide + bromine ⟶ water + potassium bromide + KBrO
potassium hydroxide + bromine ⟶ water + potassium bromide + KBrO

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + Br_2 ⟶ H_2O + KBr + KBrO 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: 2 KOH + Br_2 ⟶ H_2O + KBr + KBrO 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 | 2 | -2 Br_2 | 1 | -1 H_2O | 1 | 1 KBr | 1 | 1 KBrO | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 2 | -2 | ([KOH])^(-2) Br_2 | 1 | -1 | ([Br2])^(-1) H_2O | 1 | 1 | [H2O] KBr | 1 | 1 | [KBr] KBrO | 1 | 1 | [KBrO] 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])^(-2) ([Br2])^(-1) [H2O] [KBr] [KBrO] = ([H2O] [KBr] [KBrO])/(([KOH])^2 [Br2])
Construct the equilibrium constant, K, expression for: KOH + Br_2 ⟶ H_2O + KBr + KBrO 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: 2 KOH + Br_2 ⟶ H_2O + KBr + KBrO 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 | 2 | -2 Br_2 | 1 | -1 H_2O | 1 | 1 KBr | 1 | 1 KBrO | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 2 | -2 | ([KOH])^(-2) Br_2 | 1 | -1 | ([Br2])^(-1) H_2O | 1 | 1 | [H2O] KBr | 1 | 1 | [KBr] KBrO | 1 | 1 | [KBrO] 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])^(-2) ([Br2])^(-1) [H2O] [KBr] [KBrO] = ([H2O] [KBr] [KBrO])/(([KOH])^2 [Br2])

Rate of reaction

Construct the rate of reaction expression for: KOH + Br_2 ⟶ H_2O + KBr + KBrO 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: 2 KOH + Br_2 ⟶ H_2O + KBr + KBrO 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 | 2 | -2 Br_2 | 1 | -1 H_2O | 1 | 1 KBr | 1 | 1 KBrO | 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 | 2 | -2 | -1/2 (Δ[KOH])/(Δt) Br_2 | 1 | -1 | -(Δ[Br2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) KBr | 1 | 1 | (Δ[KBr])/(Δt) KBrO | 1 | 1 | (Δ[KBrO])/(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 = -1/2 (Δ[KOH])/(Δt) = -(Δ[Br2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[KBr])/(Δt) = (Δ[KBrO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + Br_2 ⟶ H_2O + KBr + KBrO 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: 2 KOH + Br_2 ⟶ H_2O + KBr + KBrO 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 | 2 | -2 Br_2 | 1 | -1 H_2O | 1 | 1 KBr | 1 | 1 KBrO | 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 | 2 | -2 | -1/2 (Δ[KOH])/(Δt) Br_2 | 1 | -1 | -(Δ[Br2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) KBr | 1 | 1 | (Δ[KBr])/(Δt) KBrO | 1 | 1 | (Δ[KBrO])/(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 = -1/2 (Δ[KOH])/(Δt) = -(Δ[Br2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[KBr])/(Δt) = (Δ[KBrO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | bromine | water | potassium bromide | KBrO formula | KOH | Br_2 | H_2O | KBr | KBrO Hill formula | HKO | Br_2 | H_2O | BrK | BrKO name | potassium hydroxide | bromine | water | potassium bromide | IUPAC name | potassium hydroxide | molecular bromine | water | potassium bromide |
| potassium hydroxide | bromine | water | potassium bromide | KBrO formula | KOH | Br_2 | H_2O | KBr | KBrO Hill formula | HKO | Br_2 | H_2O | BrK | BrKO name | potassium hydroxide | bromine | water | potassium bromide | IUPAC name | potassium hydroxide | molecular bromine | water | potassium bromide |

Substance properties

| potassium hydroxide | bromine | water | potassium bromide | KBrO molar mass | 56.105 g/mol | 159.81 g/mol | 18.015 g/mol | 119 g/mol | 135 g/mol phase | solid (at STP) | liquid (at STP) | liquid (at STP) | solid (at STP) | melting point | 406 °C | -7.2 °C | 0 °C | 734 °C | boiling point | 1327 °C | 58.8 °C | 99.9839 °C | 1435 °C | density | 2.044 g/cm^3 | 3.119 g/cm^3 | 1 g/cm^3 | 2.75 g/cm^3 | solubility in water | soluble | insoluble | | soluble | surface tension | | 0.0409 N/m | 0.0728 N/m | | dynamic viscosity | 0.001 Pa s (at 550 °C) | 9.44×10^-4 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | |
| potassium hydroxide | bromine | water | potassium bromide | KBrO molar mass | 56.105 g/mol | 159.81 g/mol | 18.015 g/mol | 119 g/mol | 135 g/mol phase | solid (at STP) | liquid (at STP) | liquid (at STP) | solid (at STP) | melting point | 406 °C | -7.2 °C | 0 °C | 734 °C | boiling point | 1327 °C | 58.8 °C | 99.9839 °C | 1435 °C | density | 2.044 g/cm^3 | 3.119 g/cm^3 | 1 g/cm^3 | 2.75 g/cm^3 | solubility in water | soluble | insoluble | | soluble | surface tension | | 0.0409 N/m | 0.0728 N/m | | dynamic viscosity | 0.001 Pa s (at 550 °C) | 9.44×10^-4 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | |

Units

Random Queries

melting point of 5-chloro-7-iodo-8-quinolinol
formula of magnesium nitride vs tantalum(V) bromide
alternate names of boric acid vs zinc
IUPAC name of carbon disulfide
formula of potassium dihydrogen phosphate vs 4-methylbenzylmagnesium chloride
Ag(NO3)3 = O2 + NO2 + Ag
formula of rubidium cation vs francium cation
IUPAC sodium amide
alternate names of iron(III) cation vs gold(I) cation
molar mass of sodium cation