Search

H2O + HCl + KIO3 + Sb2O3 = KCl + ICl + HSb(OH)6

Input interpretation

H_2O water + HCl hydrogen chloride + KIO_3 potassium iodate + Sb_2O_3 antimony trioxide ⟶ KCl potassium chloride + ICl iodine monochloride + HSb(OH)6
H_2O water + HCl hydrogen chloride + KIO_3 potassium iodate + Sb_2O_3 antimony trioxide ⟶ KCl potassium chloride + ICl iodine monochloride + HSb(OH)6

Balanced equation

Balance the chemical equation algebraically: H_2O + HCl + KIO_3 + Sb_2O_3 ⟶ KCl + ICl + HSb(OH)6 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 HCl + c_3 KIO_3 + c_4 Sb_2O_3 ⟶ c_5 KCl + c_6 ICl + c_7 HSb(OH)6 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, I, K and Sb: H: | 2 c_1 + c_2 = 7 c_7 O: | c_1 + 3 c_3 + 3 c_4 = 6 c_7 Cl: | c_2 = c_5 + c_6 I: | c_3 = c_6 K: | c_3 = c_5 Sb: | 2 c_4 = c_7 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 = 6 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 1 c_6 = 1 c_7 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 H_2O + 2 HCl + KIO_3 + Sb_2O_3 ⟶ KCl + ICl + 2 HSb(OH)6
Balance the chemical equation algebraically: H_2O + HCl + KIO_3 + Sb_2O_3 ⟶ KCl + ICl + HSb(OH)6 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 HCl + c_3 KIO_3 + c_4 Sb_2O_3 ⟶ c_5 KCl + c_6 ICl + c_7 HSb(OH)6 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, I, K and Sb: H: | 2 c_1 + c_2 = 7 c_7 O: | c_1 + 3 c_3 + 3 c_4 = 6 c_7 Cl: | c_2 = c_5 + c_6 I: | c_3 = c_6 K: | c_3 = c_5 Sb: | 2 c_4 = c_7 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 = 6 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 1 c_6 = 1 c_7 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 H_2O + 2 HCl + KIO_3 + Sb_2O_3 ⟶ KCl + ICl + 2 HSb(OH)6

Structures

+ + + ⟶ + + HSb(OH)6
+ + + ⟶ + + HSb(OH)6

Names

water + hydrogen chloride + potassium iodate + antimony trioxide ⟶ potassium chloride + iodine monochloride + HSb(OH)6
water + hydrogen chloride + potassium iodate + antimony trioxide ⟶ potassium chloride + iodine monochloride + HSb(OH)6

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + HCl + KIO_3 + Sb_2O_3 ⟶ KCl + ICl + HSb(OH)6 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: 6 H_2O + 2 HCl + KIO_3 + Sb_2O_3 ⟶ KCl + ICl + 2 HSb(OH)6 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 H_2O | 6 | -6 HCl | 2 | -2 KIO_3 | 1 | -1 Sb_2O_3 | 1 | -1 KCl | 1 | 1 ICl | 1 | 1 HSb(OH)6 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 6 | -6 | ([H2O])^(-6) HCl | 2 | -2 | ([HCl])^(-2) KIO_3 | 1 | -1 | ([KIO3])^(-1) Sb_2O_3 | 1 | -1 | ([Sb2O3])^(-1) KCl | 1 | 1 | [KCl] ICl | 1 | 1 | [ICl] HSb(OH)6 | 2 | 2 | ([HSb(OH)6])^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 = ([H2O])^(-6) ([HCl])^(-2) ([KIO3])^(-1) ([Sb2O3])^(-1) [KCl] [ICl] ([HSb(OH)6])^2 = ([KCl] [ICl] ([HSb(OH)6])^2)/(([H2O])^6 ([HCl])^2 [KIO3] [Sb2O3])
Construct the equilibrium constant, K, expression for: H_2O + HCl + KIO_3 + Sb_2O_3 ⟶ KCl + ICl + HSb(OH)6 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: 6 H_2O + 2 HCl + KIO_3 + Sb_2O_3 ⟶ KCl + ICl + 2 HSb(OH)6 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 H_2O | 6 | -6 HCl | 2 | -2 KIO_3 | 1 | -1 Sb_2O_3 | 1 | -1 KCl | 1 | 1 ICl | 1 | 1 HSb(OH)6 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 6 | -6 | ([H2O])^(-6) HCl | 2 | -2 | ([HCl])^(-2) KIO_3 | 1 | -1 | ([KIO3])^(-1) Sb_2O_3 | 1 | -1 | ([Sb2O3])^(-1) KCl | 1 | 1 | [KCl] ICl | 1 | 1 | [ICl] HSb(OH)6 | 2 | 2 | ([HSb(OH)6])^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 = ([H2O])^(-6) ([HCl])^(-2) ([KIO3])^(-1) ([Sb2O3])^(-1) [KCl] [ICl] ([HSb(OH)6])^2 = ([KCl] [ICl] ([HSb(OH)6])^2)/(([H2O])^6 ([HCl])^2 [KIO3] [Sb2O3])

Rate of reaction

Construct the rate of reaction expression for: H_2O + HCl + KIO_3 + Sb_2O_3 ⟶ KCl + ICl + HSb(OH)6 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: 6 H_2O + 2 HCl + KIO_3 + Sb_2O_3 ⟶ KCl + ICl + 2 HSb(OH)6 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 H_2O | 6 | -6 HCl | 2 | -2 KIO_3 | 1 | -1 Sb_2O_3 | 1 | -1 KCl | 1 | 1 ICl | 1 | 1 HSb(OH)6 | 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 H_2O | 6 | -6 | -1/6 (Δ[H2O])/(Δt) HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) KIO_3 | 1 | -1 | -(Δ[KIO3])/(Δt) Sb_2O_3 | 1 | -1 | -(Δ[Sb2O3])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(Δt) ICl | 1 | 1 | (Δ[ICl])/(Δt) HSb(OH)6 | 2 | 2 | 1/2 (Δ[HSb(OH)6])/(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 = -1/6 (Δ[H2O])/(Δt) = -1/2 (Δ[HCl])/(Δt) = -(Δ[KIO3])/(Δt) = -(Δ[Sb2O3])/(Δt) = (Δ[KCl])/(Δt) = (Δ[ICl])/(Δt) = 1/2 (Δ[HSb(OH)6])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + HCl + KIO_3 + Sb_2O_3 ⟶ KCl + ICl + HSb(OH)6 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: 6 H_2O + 2 HCl + KIO_3 + Sb_2O_3 ⟶ KCl + ICl + 2 HSb(OH)6 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 H_2O | 6 | -6 HCl | 2 | -2 KIO_3 | 1 | -1 Sb_2O_3 | 1 | -1 KCl | 1 | 1 ICl | 1 | 1 HSb(OH)6 | 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 H_2O | 6 | -6 | -1/6 (Δ[H2O])/(Δt) HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) KIO_3 | 1 | -1 | -(Δ[KIO3])/(Δt) Sb_2O_3 | 1 | -1 | -(Δ[Sb2O3])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(Δt) ICl | 1 | 1 | (Δ[ICl])/(Δt) HSb(OH)6 | 2 | 2 | 1/2 (Δ[HSb(OH)6])/(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 = -1/6 (Δ[H2O])/(Δt) = -1/2 (Δ[HCl])/(Δt) = -(Δ[KIO3])/(Δt) = -(Δ[Sb2O3])/(Δt) = (Δ[KCl])/(Δt) = (Δ[ICl])/(Δt) = 1/2 (Δ[HSb(OH)6])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | hydrogen chloride | potassium iodate | antimony trioxide | potassium chloride | iodine monochloride | HSb(OH)6 formula | H_2O | HCl | KIO_3 | Sb_2O_3 | KCl | ICl | HSb(OH)6 Hill formula | H_2O | ClH | IKO_3 | O_3Sb_2 | ClK | ClI | H7O6Sb name | water | hydrogen chloride | potassium iodate | antimony trioxide | potassium chloride | iodine monochloride | IUPAC name | water | hydrogen chloride | potassium iodate | oxo-oxostibanyloxystibane | potassium chloride | |
| water | hydrogen chloride | potassium iodate | antimony trioxide | potassium chloride | iodine monochloride | HSb(OH)6 formula | H_2O | HCl | KIO_3 | Sb_2O_3 | KCl | ICl | HSb(OH)6 Hill formula | H_2O | ClH | IKO_3 | O_3Sb_2 | ClK | ClI | H7O6Sb name | water | hydrogen chloride | potassium iodate | antimony trioxide | potassium chloride | iodine monochloride | IUPAC name | water | hydrogen chloride | potassium iodate | oxo-oxostibanyloxystibane | potassium chloride | |

Substance properties

| water | hydrogen chloride | potassium iodate | antimony trioxide | potassium chloride | iodine monochloride | HSb(OH)6 molar mass | 18.015 g/mol | 36.46 g/mol | 214 g/mol | 291.517 g/mol | 74.55 g/mol | 162.35 g/mol | 224.81 g/mol phase | liquid (at STP) | gas (at STP) | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 0 °C | -114.17 °C | 560 °C | 655 °C | 770 °C | 26 °C | boiling point | 99.9839 °C | -85 °C | | 1550 °C | 1420 °C | 97.4 °C | density | 1 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 1.005 g/cm^3 | 5.2 g/cm^3 | 1.98 g/cm^3 | 3.24 g/cm^3 | solubility in water | | miscible | | insoluble | soluble | decomposes | surface tension | 0.0728 N/m | | | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | | | | | odor | odorless | | | | odorless | |
| water | hydrogen chloride | potassium iodate | antimony trioxide | potassium chloride | iodine monochloride | HSb(OH)6 molar mass | 18.015 g/mol | 36.46 g/mol | 214 g/mol | 291.517 g/mol | 74.55 g/mol | 162.35 g/mol | 224.81 g/mol phase | liquid (at STP) | gas (at STP) | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 0 °C | -114.17 °C | 560 °C | 655 °C | 770 °C | 26 °C | boiling point | 99.9839 °C | -85 °C | | 1550 °C | 1420 °C | 97.4 °C | density | 1 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 1.005 g/cm^3 | 5.2 g/cm^3 | 1.98 g/cm^3 | 3.24 g/cm^3 | solubility in water | | miscible | | insoluble | soluble | decomposes | surface tension | 0.0728 N/m | | | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | | | | | odor | odorless | | | | odorless | |

Units

Random Queries

IUPAC name of magnesium oxide vs nickel
IUPAC name of caffeine
alternate names of group 7 elements
common compound names of lead
name of phenylselenyl halide functional group vs tertiary carbocation functional group
find watershed components image actinolite
molar mass of hexachloroselenate(IV) anion vs pentaamminechlorocobalt(II) cation
formula string of alkyl halide functional group vs D-threo-aldose functional group
enolate functional group
iron(II) oxide vs palladium oxide