Search

H2SO4 + HI + KIO3 = H2O + K2SO4 + I2

Input interpretation

H_2SO_4 sulfuric acid + HI hydrogen iodide + KIO_3 potassium iodate ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine
H_2SO_4 sulfuric acid + HI hydrogen iodide + KIO_3 potassium iodate ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + HI + KIO_3 ⟶ H_2O + K_2SO_4 + I_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 HI + c_3 KIO_3 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 I_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, I and K: H: | 2 c_1 + c_2 = 2 c_4 O: | 4 c_1 + 3 c_3 = c_4 + 4 c_5 S: | c_1 = c_5 I: | c_2 + c_3 = 2 c_6 K: | c_3 = 2 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 = 10 c_3 = 2 c_4 = 6 c_5 = 1 c_6 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 10 HI + 2 KIO_3 ⟶ 6 H_2O + K_2SO_4 + 6 I_2
Balance the chemical equation algebraically: H_2SO_4 + HI + KIO_3 ⟶ H_2O + K_2SO_4 + I_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 HI + c_3 KIO_3 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 I_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, I and K: H: | 2 c_1 + c_2 = 2 c_4 O: | 4 c_1 + 3 c_3 = c_4 + 4 c_5 S: | c_1 = c_5 I: | c_2 + c_3 = 2 c_6 K: | c_3 = 2 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 = 10 c_3 = 2 c_4 = 6 c_5 = 1 c_6 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 10 HI + 2 KIO_3 ⟶ 6 H_2O + K_2SO_4 + 6 I_2

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

sulfuric acid + hydrogen iodide + potassium iodate ⟶ water + potassium sulfate + iodine
sulfuric acid + hydrogen iodide + potassium iodate ⟶ water + potassium sulfate + iodine

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + HI + KIO_3 ⟶ H_2O + K_2SO_4 + I_2 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: H_2SO_4 + 10 HI + 2 KIO_3 ⟶ 6 H_2O + K_2SO_4 + 6 I_2 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_2SO_4 | 1 | -1 HI | 10 | -10 KIO_3 | 2 | -2 H_2O | 6 | 6 K_2SO_4 | 1 | 1 I_2 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) HI | 10 | -10 | ([HI])^(-10) KIO_3 | 2 | -2 | ([KIO3])^(-2) H_2O | 6 | 6 | ([H2O])^6 K_2SO_4 | 1 | 1 | [K2SO4] I_2 | 6 | 6 | ([I2])^6 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 = ([H2SO4])^(-1) ([HI])^(-10) ([KIO3])^(-2) ([H2O])^6 [K2SO4] ([I2])^6 = (([H2O])^6 [K2SO4] ([I2])^6)/([H2SO4] ([HI])^10 ([KIO3])^2)
Construct the equilibrium constant, K, expression for: H_2SO_4 + HI + KIO_3 ⟶ H_2O + K_2SO_4 + I_2 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: H_2SO_4 + 10 HI + 2 KIO_3 ⟶ 6 H_2O + K_2SO_4 + 6 I_2 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_2SO_4 | 1 | -1 HI | 10 | -10 KIO_3 | 2 | -2 H_2O | 6 | 6 K_2SO_4 | 1 | 1 I_2 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) HI | 10 | -10 | ([HI])^(-10) KIO_3 | 2 | -2 | ([KIO3])^(-2) H_2O | 6 | 6 | ([H2O])^6 K_2SO_4 | 1 | 1 | [K2SO4] I_2 | 6 | 6 | ([I2])^6 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 = ([H2SO4])^(-1) ([HI])^(-10) ([KIO3])^(-2) ([H2O])^6 [K2SO4] ([I2])^6 = (([H2O])^6 [K2SO4] ([I2])^6)/([H2SO4] ([HI])^10 ([KIO3])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + HI + KIO_3 ⟶ H_2O + K_2SO_4 + I_2 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: H_2SO_4 + 10 HI + 2 KIO_3 ⟶ 6 H_2O + K_2SO_4 + 6 I_2 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_2SO_4 | 1 | -1 HI | 10 | -10 KIO_3 | 2 | -2 H_2O | 6 | 6 K_2SO_4 | 1 | 1 I_2 | 6 | 6 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_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) HI | 10 | -10 | -1/10 (Δ[HI])/(Δt) KIO_3 | 2 | -2 | -1/2 (Δ[KIO3])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) I_2 | 6 | 6 | 1/6 (Δ[I2])/(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[H2SO4])/(Δt) = -1/10 (Δ[HI])/(Δt) = -1/2 (Δ[KIO3])/(Δt) = 1/6 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/6 (Δ[I2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + HI + KIO_3 ⟶ H_2O + K_2SO_4 + I_2 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: H_2SO_4 + 10 HI + 2 KIO_3 ⟶ 6 H_2O + K_2SO_4 + 6 I_2 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_2SO_4 | 1 | -1 HI | 10 | -10 KIO_3 | 2 | -2 H_2O | 6 | 6 K_2SO_4 | 1 | 1 I_2 | 6 | 6 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_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) HI | 10 | -10 | -1/10 (Δ[HI])/(Δt) KIO_3 | 2 | -2 | -1/2 (Δ[KIO3])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) I_2 | 6 | 6 | 1/6 (Δ[I2])/(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[H2SO4])/(Δt) = -1/10 (Δ[HI])/(Δt) = -1/2 (Δ[KIO3])/(Δt) = 1/6 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/6 (Δ[I2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | hydrogen iodide | potassium iodate | water | potassium sulfate | iodine formula | H_2SO_4 | HI | KIO_3 | H_2O | K_2SO_4 | I_2 Hill formula | H_2O_4S | HI | IKO_3 | H_2O | K_2O_4S | I_2 name | sulfuric acid | hydrogen iodide | potassium iodate | water | potassium sulfate | iodine IUPAC name | sulfuric acid | hydrogen iodide | potassium iodate | water | dipotassium sulfate | molecular iodine
| sulfuric acid | hydrogen iodide | potassium iodate | water | potassium sulfate | iodine formula | H_2SO_4 | HI | KIO_3 | H_2O | K_2SO_4 | I_2 Hill formula | H_2O_4S | HI | IKO_3 | H_2O | K_2O_4S | I_2 name | sulfuric acid | hydrogen iodide | potassium iodate | water | potassium sulfate | iodine IUPAC name | sulfuric acid | hydrogen iodide | potassium iodate | water | dipotassium sulfate | molecular iodine

Substance properties

| sulfuric acid | hydrogen iodide | potassium iodate | water | potassium sulfate | iodine molar mass | 98.07 g/mol | 127.912 g/mol | 214 g/mol | 18.015 g/mol | 174.25 g/mol | 253.80894 g/mol phase | liquid (at STP) | gas (at STP) | solid (at STP) | liquid (at STP) | | solid (at STP) melting point | 10.371 °C | -50.76 °C | 560 °C | 0 °C | | 113 °C boiling point | 279.6 °C | -35.55 °C | | 99.9839 °C | | 184 °C density | 1.8305 g/cm^3 | 0.005228 g/cm^3 (at 25 °C) | 1.005 g/cm^3 | 1 g/cm^3 | | 4.94 g/cm^3 solubility in water | very soluble | very soluble | | | soluble | surface tension | 0.0735 N/m | | | 0.0728 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | 0.001321 Pa s (at -39 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | 0.00227 Pa s (at 116 °C) odor | odorless | | | odorless | |
| sulfuric acid | hydrogen iodide | potassium iodate | water | potassium sulfate | iodine molar mass | 98.07 g/mol | 127.912 g/mol | 214 g/mol | 18.015 g/mol | 174.25 g/mol | 253.80894 g/mol phase | liquid (at STP) | gas (at STP) | solid (at STP) | liquid (at STP) | | solid (at STP) melting point | 10.371 °C | -50.76 °C | 560 °C | 0 °C | | 113 °C boiling point | 279.6 °C | -35.55 °C | | 99.9839 °C | | 184 °C density | 1.8305 g/cm^3 | 0.005228 g/cm^3 (at 25 °C) | 1.005 g/cm^3 | 1 g/cm^3 | | 4.94 g/cm^3 solubility in water | very soluble | very soluble | | | soluble | surface tension | 0.0735 N/m | | | 0.0728 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | 0.001321 Pa s (at -39 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | 0.00227 Pa s (at 116 °C) odor | odorless | | | odorless | |

Units

Random Queries

IUPAC name of gold(I) chloride
CAS number of stannous chloride vs vanadium(II) oxide
connected components image parnauite
ion class of hexachloroselenate(IV) anion vs hexachlorogermanate(IV) anion
flash point of 1-hexyn-3-ol
atomic mass of radium vs francium
formula of aryl nitro functional group
molar mass of molybdic acid vs samarium(III) sulfate
PubChem CID number of potassium chloroplatinate
name of hexadecafluorophthalocyanine vs diphenylphosphino ferrocene anion