Search

KOH + KClO + KCrO2 = H2O + KCl + K2CrO4

Input interpretation

KOH potassium hydroxide + KClO + KCrO2 ⟶ H_2O water + KCl potassium chloride + K_2CrO_4 potassium chromate
KOH potassium hydroxide + KClO + KCrO2 ⟶ H_2O water + KCl potassium chloride + K_2CrO_4 potassium chromate

Balanced equation

Balance the chemical equation algebraically: KOH + KClO + KCrO2 ⟶ H_2O + KCl + K_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 KClO + c_3 KCrO2 ⟶ c_4 H_2O + c_5 KCl + c_6 K_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Cl and Cr: H: | c_1 = 2 c_4 K: | c_1 + c_2 + c_3 = c_5 + 2 c_6 O: | c_1 + c_2 + 2 c_3 = c_4 + 4 c_6 Cl: | c_2 = c_5 Cr: | c_3 = c_6 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 2 c_4 = 1 c_5 = 3 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + 3 KClO + 2 KCrO2 ⟶ H_2O + 3 KCl + 2 K_2CrO_4
Balance the chemical equation algebraically: KOH + KClO + KCrO2 ⟶ H_2O + KCl + K_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 KClO + c_3 KCrO2 ⟶ c_4 H_2O + c_5 KCl + c_6 K_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Cl and Cr: H: | c_1 = 2 c_4 K: | c_1 + c_2 + c_3 = c_5 + 2 c_6 O: | c_1 + c_2 + 2 c_3 = c_4 + 4 c_6 Cl: | c_2 = c_5 Cr: | c_3 = c_6 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 2 c_4 = 1 c_5 = 3 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + 3 KClO + 2 KCrO2 ⟶ H_2O + 3 KCl + 2 K_2CrO_4

Structures

+ KClO + KCrO2 ⟶ + +
+ KClO + KCrO2 ⟶ + +

Names

potassium hydroxide + KClO + KCrO2 ⟶ water + potassium chloride + potassium chromate
potassium hydroxide + KClO + KCrO2 ⟶ water + potassium chloride + potassium chromate

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + KClO + KCrO2 ⟶ H_2O + KCl + K_2CrO_4 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 + 3 KClO + 2 KCrO2 ⟶ H_2O + 3 KCl + 2 K_2CrO_4 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 KClO | 3 | -3 KCrO2 | 2 | -2 H_2O | 1 | 1 KCl | 3 | 3 K_2CrO_4 | 2 | 2 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) KClO | 3 | -3 | ([KClO])^(-3) KCrO2 | 2 | -2 | ([KCrO2])^(-2) H_2O | 1 | 1 | [H2O] KCl | 3 | 3 | ([KCl])^3 K_2CrO_4 | 2 | 2 | ([K2CrO4])^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 = ([KOH])^(-2) ([KClO])^(-3) ([KCrO2])^(-2) [H2O] ([KCl])^3 ([K2CrO4])^2 = ([H2O] ([KCl])^3 ([K2CrO4])^2)/(([KOH])^2 ([KClO])^3 ([KCrO2])^2)
Construct the equilibrium constant, K, expression for: KOH + KClO + KCrO2 ⟶ H_2O + KCl + K_2CrO_4 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 + 3 KClO + 2 KCrO2 ⟶ H_2O + 3 KCl + 2 K_2CrO_4 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 KClO | 3 | -3 KCrO2 | 2 | -2 H_2O | 1 | 1 KCl | 3 | 3 K_2CrO_4 | 2 | 2 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) KClO | 3 | -3 | ([KClO])^(-3) KCrO2 | 2 | -2 | ([KCrO2])^(-2) H_2O | 1 | 1 | [H2O] KCl | 3 | 3 | ([KCl])^3 K_2CrO_4 | 2 | 2 | ([K2CrO4])^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 = ([KOH])^(-2) ([KClO])^(-3) ([KCrO2])^(-2) [H2O] ([KCl])^3 ([K2CrO4])^2 = ([H2O] ([KCl])^3 ([K2CrO4])^2)/(([KOH])^2 ([KClO])^3 ([KCrO2])^2)

Rate of reaction

Construct the rate of reaction expression for: KOH + KClO + KCrO2 ⟶ H_2O + KCl + K_2CrO_4 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 + 3 KClO + 2 KCrO2 ⟶ H_2O + 3 KCl + 2 K_2CrO_4 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 KClO | 3 | -3 KCrO2 | 2 | -2 H_2O | 1 | 1 KCl | 3 | 3 K_2CrO_4 | 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 KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) KClO | 3 | -3 | -1/3 (Δ[KClO])/(Δt) KCrO2 | 2 | -2 | -1/2 (Δ[KCrO2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) KCl | 3 | 3 | 1/3 (Δ[KCl])/(Δt) K_2CrO_4 | 2 | 2 | 1/2 (Δ[K2CrO4])/(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) = -1/3 (Δ[KClO])/(Δt) = -1/2 (Δ[KCrO2])/(Δt) = (Δ[H2O])/(Δt) = 1/3 (Δ[KCl])/(Δt) = 1/2 (Δ[K2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + KClO + KCrO2 ⟶ H_2O + KCl + K_2CrO_4 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 + 3 KClO + 2 KCrO2 ⟶ H_2O + 3 KCl + 2 K_2CrO_4 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 KClO | 3 | -3 KCrO2 | 2 | -2 H_2O | 1 | 1 KCl | 3 | 3 K_2CrO_4 | 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 KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) KClO | 3 | -3 | -1/3 (Δ[KClO])/(Δt) KCrO2 | 2 | -2 | -1/2 (Δ[KCrO2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) KCl | 3 | 3 | 1/3 (Δ[KCl])/(Δt) K_2CrO_4 | 2 | 2 | 1/2 (Δ[K2CrO4])/(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) = -1/3 (Δ[KClO])/(Δt) = -1/2 (Δ[KCrO2])/(Δt) = (Δ[H2O])/(Δt) = 1/3 (Δ[KCl])/(Δt) = 1/2 (Δ[K2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | KClO | KCrO2 | water | potassium chloride | potassium chromate formula | KOH | KClO | KCrO2 | H_2O | KCl | K_2CrO_4 Hill formula | HKO | ClKO | CrKO2 | H_2O | ClK | CrK_2O_4 name | potassium hydroxide | | | water | potassium chloride | potassium chromate IUPAC name | potassium hydroxide | | | water | potassium chloride | dipotassium dioxido-dioxochromium
| potassium hydroxide | KClO | KCrO2 | water | potassium chloride | potassium chromate formula | KOH | KClO | KCrO2 | H_2O | KCl | K_2CrO_4 Hill formula | HKO | ClKO | CrKO2 | H_2O | ClK | CrK_2O_4 name | potassium hydroxide | | | water | potassium chloride | potassium chromate IUPAC name | potassium hydroxide | | | water | potassium chloride | dipotassium dioxido-dioxochromium

Substance properties

| potassium hydroxide | KClO | KCrO2 | water | potassium chloride | potassium chromate molar mass | 56.105 g/mol | 90.55 g/mol | 123.09 g/mol | 18.015 g/mol | 74.55 g/mol | 194.19 g/mol phase | solid (at STP) | | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 406 °C | | | 0 °C | 770 °C | 971 °C boiling point | 1327 °C | | | 99.9839 °C | 1420 °C | density | 2.044 g/cm^3 | | | 1 g/cm^3 | 1.98 g/cm^3 | 2.73 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 | odorless
| potassium hydroxide | KClO | KCrO2 | water | potassium chloride | potassium chromate molar mass | 56.105 g/mol | 90.55 g/mol | 123.09 g/mol | 18.015 g/mol | 74.55 g/mol | 194.19 g/mol phase | solid (at STP) | | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 406 °C | | | 0 °C | 770 °C | 971 °C boiling point | 1327 °C | | | 99.9839 °C | 1420 °C | density | 2.044 g/cm^3 | | | 1 g/cm^3 | 1.98 g/cm^3 | 2.73 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 | odorless

Units

Random Queries

common sources of ion of copper(II) cation vs acetate anion
CAS number of thallium(III) nitrate vs lutetium(III) carbonate hydrate
atomic radius of bromine vs iodine
chemical uses of L-thiocitrulline
name of copper(II) phosphate
names of L tyrosine
manganese dioxide vs ammonium cobalt(II) sulfate hexahydrate
bond counts of water vs acetic acid
mass fractions of tin(IV) fluoride
approval status of teriparatide