Search

NaOH + KClO3 + Cr(OH)3 = H2O + KCl + Na2CrO4

Input interpretation

NaOH sodium hydroxide + KClO_3 potassium chlorate + Cr(OH)3 ⟶ H_2O water + KCl potassium chloride + Na_2CrO_4 sodium chromate
NaOH sodium hydroxide + KClO_3 potassium chlorate + Cr(OH)3 ⟶ H_2O water + KCl potassium chloride + Na_2CrO_4 sodium chromate

Balanced equation

Balance the chemical equation algebraically: NaOH + KClO_3 + Cr(OH)3 ⟶ H_2O + KCl + Na_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 KClO_3 + c_3 Cr(OH)3 ⟶ c_4 H_2O + c_5 KCl + c_6 Na_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Cl, K and Cr: H: | c_1 + 3 c_3 = 2 c_4 Na: | c_1 = 2 c_6 O: | c_1 + 3 c_2 + 3 c_3 = c_4 + 4 c_6 Cl: | c_2 = c_5 K: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 1 c_3 = 2 c_4 = 5 c_5 = 1 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 NaOH + KClO_3 + 2 Cr(OH)3 ⟶ 5 H_2O + KCl + 2 Na_2CrO_4
Balance the chemical equation algebraically: NaOH + KClO_3 + Cr(OH)3 ⟶ H_2O + KCl + Na_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 KClO_3 + c_3 Cr(OH)3 ⟶ c_4 H_2O + c_5 KCl + c_6 Na_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Cl, K and Cr: H: | c_1 + 3 c_3 = 2 c_4 Na: | c_1 = 2 c_6 O: | c_1 + 3 c_2 + 3 c_3 = c_4 + 4 c_6 Cl: | c_2 = c_5 K: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 1 c_3 = 2 c_4 = 5 c_5 = 1 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 NaOH + KClO_3 + 2 Cr(OH)3 ⟶ 5 H_2O + KCl + 2 Na_2CrO_4

Structures

+ + Cr(OH)3 ⟶ + +
+ + Cr(OH)3 ⟶ + +

Names

sodium hydroxide + potassium chlorate + Cr(OH)3 ⟶ water + potassium chloride + sodium chromate
sodium hydroxide + potassium chlorate + Cr(OH)3 ⟶ water + potassium chloride + sodium chromate

Equilibrium constant

Construct the equilibrium constant, K, expression for: NaOH + KClO_3 + Cr(OH)3 ⟶ H_2O + KCl + Na_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: 4 NaOH + KClO_3 + 2 Cr(OH)3 ⟶ 5 H_2O + KCl + 2 Na_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 NaOH | 4 | -4 KClO_3 | 1 | -1 Cr(OH)3 | 2 | -2 H_2O | 5 | 5 KCl | 1 | 1 Na_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 NaOH | 4 | -4 | ([NaOH])^(-4) KClO_3 | 1 | -1 | ([KClO3])^(-1) Cr(OH)3 | 2 | -2 | ([Cr(OH)3])^(-2) H_2O | 5 | 5 | ([H2O])^5 KCl | 1 | 1 | [KCl] Na_2CrO_4 | 2 | 2 | ([Na2CrO4])^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 = ([NaOH])^(-4) ([KClO3])^(-1) ([Cr(OH)3])^(-2) ([H2O])^5 [KCl] ([Na2CrO4])^2 = (([H2O])^5 [KCl] ([Na2CrO4])^2)/(([NaOH])^4 [KClO3] ([Cr(OH)3])^2)
Construct the equilibrium constant, K, expression for: NaOH + KClO_3 + Cr(OH)3 ⟶ H_2O + KCl + Na_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: 4 NaOH + KClO_3 + 2 Cr(OH)3 ⟶ 5 H_2O + KCl + 2 Na_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 NaOH | 4 | -4 KClO_3 | 1 | -1 Cr(OH)3 | 2 | -2 H_2O | 5 | 5 KCl | 1 | 1 Na_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 NaOH | 4 | -4 | ([NaOH])^(-4) KClO_3 | 1 | -1 | ([KClO3])^(-1) Cr(OH)3 | 2 | -2 | ([Cr(OH)3])^(-2) H_2O | 5 | 5 | ([H2O])^5 KCl | 1 | 1 | [KCl] Na_2CrO_4 | 2 | 2 | ([Na2CrO4])^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 = ([NaOH])^(-4) ([KClO3])^(-1) ([Cr(OH)3])^(-2) ([H2O])^5 [KCl] ([Na2CrO4])^2 = (([H2O])^5 [KCl] ([Na2CrO4])^2)/(([NaOH])^4 [KClO3] ([Cr(OH)3])^2)

Rate of reaction

Construct the rate of reaction expression for: NaOH + KClO_3 + Cr(OH)3 ⟶ H_2O + KCl + Na_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: 4 NaOH + KClO_3 + 2 Cr(OH)3 ⟶ 5 H_2O + KCl + 2 Na_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 NaOH | 4 | -4 KClO_3 | 1 | -1 Cr(OH)3 | 2 | -2 H_2O | 5 | 5 KCl | 1 | 1 Na_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 NaOH | 4 | -4 | -1/4 (Δ[NaOH])/(Δt) KClO_3 | 1 | -1 | -(Δ[KClO3])/(Δt) Cr(OH)3 | 2 | -2 | -1/2 (Δ[Cr(OH)3])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(Δt) Na_2CrO_4 | 2 | 2 | 1/2 (Δ[Na2CrO4])/(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[NaOH])/(Δt) = -(Δ[KClO3])/(Δt) = -1/2 (Δ[Cr(OH)3])/(Δt) = 1/5 (Δ[H2O])/(Δt) = (Δ[KCl])/(Δt) = 1/2 (Δ[Na2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NaOH + KClO_3 + Cr(OH)3 ⟶ H_2O + KCl + Na_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: 4 NaOH + KClO_3 + 2 Cr(OH)3 ⟶ 5 H_2O + KCl + 2 Na_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 NaOH | 4 | -4 KClO_3 | 1 | -1 Cr(OH)3 | 2 | -2 H_2O | 5 | 5 KCl | 1 | 1 Na_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 NaOH | 4 | -4 | -1/4 (Δ[NaOH])/(Δt) KClO_3 | 1 | -1 | -(Δ[KClO3])/(Δt) Cr(OH)3 | 2 | -2 | -1/2 (Δ[Cr(OH)3])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(Δt) Na_2CrO_4 | 2 | 2 | 1/2 (Δ[Na2CrO4])/(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[NaOH])/(Δt) = -(Δ[KClO3])/(Δt) = -1/2 (Δ[Cr(OH)3])/(Δt) = 1/5 (Δ[H2O])/(Δt) = (Δ[KCl])/(Δt) = 1/2 (Δ[Na2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium hydroxide | potassium chlorate | Cr(OH)3 | water | potassium chloride | sodium chromate formula | NaOH | KClO_3 | Cr(OH)3 | H_2O | KCl | Na_2CrO_4 Hill formula | HNaO | ClKO_3 | H3CrO3 | H_2O | ClK | CrNa_2O_4 name | sodium hydroxide | potassium chlorate | | water | potassium chloride | sodium chromate IUPAC name | sodium hydroxide | potassium chlorate | | water | potassium chloride | disodium dioxido(dioxo)chromium
| sodium hydroxide | potassium chlorate | Cr(OH)3 | water | potassium chloride | sodium chromate formula | NaOH | KClO_3 | Cr(OH)3 | H_2O | KCl | Na_2CrO_4 Hill formula | HNaO | ClKO_3 | H3CrO3 | H_2O | ClK | CrNa_2O_4 name | sodium hydroxide | potassium chlorate | | water | potassium chloride | sodium chromate IUPAC name | sodium hydroxide | potassium chlorate | | water | potassium chloride | disodium dioxido(dioxo)chromium

Substance properties

| sodium hydroxide | potassium chlorate | Cr(OH)3 | water | potassium chloride | sodium chromate molar mass | 39.997 g/mol | 122.5 g/mol | 103.02 g/mol | 18.015 g/mol | 74.55 g/mol | 161.97 g/mol phase | solid (at STP) | solid (at STP) | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 323 °C | 356 °C | | 0 °C | 770 °C | 780 °C boiling point | 1390 °C | | | 99.9839 °C | 1420 °C | density | 2.13 g/cm^3 | 2.34 g/cm^3 | | 1 g/cm^3 | 1.98 g/cm^3 | 2.698 g/cm^3 solubility in water | soluble | soluble | | | soluble | surface tension | 0.07435 N/m | | | 0.0728 N/m | | dynamic viscosity | 0.004 Pa s (at 350 °C) | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | | odorless | odorless |
| sodium hydroxide | potassium chlorate | Cr(OH)3 | water | potassium chloride | sodium chromate molar mass | 39.997 g/mol | 122.5 g/mol | 103.02 g/mol | 18.015 g/mol | 74.55 g/mol | 161.97 g/mol phase | solid (at STP) | solid (at STP) | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 323 °C | 356 °C | | 0 °C | 770 °C | 780 °C boiling point | 1390 °C | | | 99.9839 °C | 1420 °C | density | 2.13 g/cm^3 | 2.34 g/cm^3 | | 1 g/cm^3 | 1.98 g/cm^3 | 2.698 g/cm^3 solubility in water | soluble | soluble | | | soluble | surface tension | 0.07435 N/m | | | 0.0728 N/m | | dynamic viscosity | 0.004 Pa s (at 350 °C) | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | | odorless | odorless |

Units

Random Queries

structure diagram of iodide anion vs fluoride anion
rhodium(III) chloride hydrate vs vanadium boride
molar mass of nickel(II) nitrate
edge types of cadmium phosphate vs methyl eosin
SMILES identifier of fluorosulfonic acid
alternate names of iodine(III) cation
IUPAC name of (S)-2-chloropropionic acid vs methyltin trichloride
melting point of manganese antimonide (1:1) vs stibine
image closing image natroapophyllite
atomic mass of nitrogen vs oxygen