Search

HCl + Na2S2O3 + KIO3 = H2O + NaCl + KI + Na2S4O6

Input interpretation

HCl hydrogen chloride + Na_2S_2O_3 sodium hyposulfite + KIO_3 potassium iodate ⟶ H_2O water + NaCl sodium chloride + KI potassium iodide + Na2S4O6
HCl hydrogen chloride + Na_2S_2O_3 sodium hyposulfite + KIO_3 potassium iodate ⟶ H_2O water + NaCl sodium chloride + KI potassium iodide + Na2S4O6

Balanced equation

Balance the chemical equation algebraically: HCl + Na_2S_2O_3 + KIO_3 ⟶ H_2O + NaCl + KI + Na2S4O6 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Na_2S_2O_3 + c_3 KIO_3 ⟶ c_4 H_2O + c_5 NaCl + c_6 KI + c_7 Na2S4O6 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Na, O, S, I and K: Cl: | c_1 = c_5 H: | c_1 = 2 c_4 Na: | 2 c_2 = c_5 + 2 c_7 O: | 3 c_2 + 3 c_3 = c_4 + 6 c_7 S: | 2 c_2 = 4 c_7 I: | c_3 = c_6 K: | 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 6 c_3 = 1 c_4 = 3 c_5 = 6 c_6 = 1 c_7 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HCl + 6 Na_2S_2O_3 + KIO_3 ⟶ 3 H_2O + 6 NaCl + KI + 3 Na2S4O6
Balance the chemical equation algebraically: HCl + Na_2S_2O_3 + KIO_3 ⟶ H_2O + NaCl + KI + Na2S4O6 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Na_2S_2O_3 + c_3 KIO_3 ⟶ c_4 H_2O + c_5 NaCl + c_6 KI + c_7 Na2S4O6 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Na, O, S, I and K: Cl: | c_1 = c_5 H: | c_1 = 2 c_4 Na: | 2 c_2 = c_5 + 2 c_7 O: | 3 c_2 + 3 c_3 = c_4 + 6 c_7 S: | 2 c_2 = 4 c_7 I: | c_3 = c_6 K: | 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 6 c_3 = 1 c_4 = 3 c_5 = 6 c_6 = 1 c_7 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HCl + 6 Na_2S_2O_3 + KIO_3 ⟶ 3 H_2O + 6 NaCl + KI + 3 Na2S4O6

Structures

+ + ⟶ + + + Na2S4O6
+ + ⟶ + + + Na2S4O6

Names

hydrogen chloride + sodium hyposulfite + potassium iodate ⟶ water + sodium chloride + potassium iodide + Na2S4O6
hydrogen chloride + sodium hyposulfite + potassium iodate ⟶ water + sodium chloride + potassium iodide + Na2S4O6

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + Na_2S_2O_3 + KIO_3 ⟶ H_2O + NaCl + KI + Na2S4O6 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 HCl + 6 Na_2S_2O_3 + KIO_3 ⟶ 3 H_2O + 6 NaCl + KI + 3 Na2S4O6 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 HCl | 6 | -6 Na_2S_2O_3 | 6 | -6 KIO_3 | 1 | -1 H_2O | 3 | 3 NaCl | 6 | 6 KI | 1 | 1 Na2S4O6 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) Na_2S_2O_3 | 6 | -6 | ([Na2S2O3])^(-6) KIO_3 | 1 | -1 | ([KIO3])^(-1) H_2O | 3 | 3 | ([H2O])^3 NaCl | 6 | 6 | ([NaCl])^6 KI | 1 | 1 | [KI] Na2S4O6 | 3 | 3 | ([Na2S4O6])^3 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 = ([HCl])^(-6) ([Na2S2O3])^(-6) ([KIO3])^(-1) ([H2O])^3 ([NaCl])^6 [KI] ([Na2S4O6])^3 = (([H2O])^3 ([NaCl])^6 [KI] ([Na2S4O6])^3)/(([HCl])^6 ([Na2S2O3])^6 [KIO3])
Construct the equilibrium constant, K, expression for: HCl + Na_2S_2O_3 + KIO_3 ⟶ H_2O + NaCl + KI + Na2S4O6 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 HCl + 6 Na_2S_2O_3 + KIO_3 ⟶ 3 H_2O + 6 NaCl + KI + 3 Na2S4O6 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 HCl | 6 | -6 Na_2S_2O_3 | 6 | -6 KIO_3 | 1 | -1 H_2O | 3 | 3 NaCl | 6 | 6 KI | 1 | 1 Na2S4O6 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) Na_2S_2O_3 | 6 | -6 | ([Na2S2O3])^(-6) KIO_3 | 1 | -1 | ([KIO3])^(-1) H_2O | 3 | 3 | ([H2O])^3 NaCl | 6 | 6 | ([NaCl])^6 KI | 1 | 1 | [KI] Na2S4O6 | 3 | 3 | ([Na2S4O6])^3 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 = ([HCl])^(-6) ([Na2S2O3])^(-6) ([KIO3])^(-1) ([H2O])^3 ([NaCl])^6 [KI] ([Na2S4O6])^3 = (([H2O])^3 ([NaCl])^6 [KI] ([Na2S4O6])^3)/(([HCl])^6 ([Na2S2O3])^6 [KIO3])

Rate of reaction

Construct the rate of reaction expression for: HCl + Na_2S_2O_3 + KIO_3 ⟶ H_2O + NaCl + KI + Na2S4O6 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 HCl + 6 Na_2S_2O_3 + KIO_3 ⟶ 3 H_2O + 6 NaCl + KI + 3 Na2S4O6 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 HCl | 6 | -6 Na_2S_2O_3 | 6 | -6 KIO_3 | 1 | -1 H_2O | 3 | 3 NaCl | 6 | 6 KI | 1 | 1 Na2S4O6 | 3 | 3 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 HCl | 6 | -6 | -1/6 (Δ[HCl])/(Δt) Na_2S_2O_3 | 6 | -6 | -1/6 (Δ[Na2S2O3])/(Δt) KIO_3 | 1 | -1 | -(Δ[KIO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) NaCl | 6 | 6 | 1/6 (Δ[NaCl])/(Δt) KI | 1 | 1 | (Δ[KI])/(Δt) Na2S4O6 | 3 | 3 | 1/3 (Δ[Na2S4O6])/(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[HCl])/(Δt) = -1/6 (Δ[Na2S2O3])/(Δt) = -(Δ[KIO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/6 (Δ[NaCl])/(Δt) = (Δ[KI])/(Δt) = 1/3 (Δ[Na2S4O6])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + Na_2S_2O_3 + KIO_3 ⟶ H_2O + NaCl + KI + Na2S4O6 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 HCl + 6 Na_2S_2O_3 + KIO_3 ⟶ 3 H_2O + 6 NaCl + KI + 3 Na2S4O6 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 HCl | 6 | -6 Na_2S_2O_3 | 6 | -6 KIO_3 | 1 | -1 H_2O | 3 | 3 NaCl | 6 | 6 KI | 1 | 1 Na2S4O6 | 3 | 3 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 HCl | 6 | -6 | -1/6 (Δ[HCl])/(Δt) Na_2S_2O_3 | 6 | -6 | -1/6 (Δ[Na2S2O3])/(Δt) KIO_3 | 1 | -1 | -(Δ[KIO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) NaCl | 6 | 6 | 1/6 (Δ[NaCl])/(Δt) KI | 1 | 1 | (Δ[KI])/(Δt) Na2S4O6 | 3 | 3 | 1/3 (Δ[Na2S4O6])/(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[HCl])/(Δt) = -1/6 (Δ[Na2S2O3])/(Δt) = -(Δ[KIO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/6 (Δ[NaCl])/(Δt) = (Δ[KI])/(Δt) = 1/3 (Δ[Na2S4O6])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | sodium hyposulfite | potassium iodate | water | sodium chloride | potassium iodide | Na2S4O6 formula | HCl | Na_2S_2O_3 | KIO_3 | H_2O | NaCl | KI | Na2S4O6 Hill formula | ClH | Na_2O_3S_2 | IKO_3 | H_2O | ClNa | IK | Na2O6S4 name | hydrogen chloride | sodium hyposulfite | potassium iodate | water | sodium chloride | potassium iodide |
| hydrogen chloride | sodium hyposulfite | potassium iodate | water | sodium chloride | potassium iodide | Na2S4O6 formula | HCl | Na_2S_2O_3 | KIO_3 | H_2O | NaCl | KI | Na2S4O6 Hill formula | ClH | Na_2O_3S_2 | IKO_3 | H_2O | ClNa | IK | Na2O6S4 name | hydrogen chloride | sodium hyposulfite | potassium iodate | water | sodium chloride | potassium iodide |

Random Queries

IUPAC name of strontium iodide
formula of ammonium ferrous sulfate
formal charges of oxide anion vs chloride anion
chemical types of diisobutylaluminum hydride vs bis(tributylstannyl)acetylene
Hill formula string of benzo[a]pyrene-d 12
PubChem CID number of lutetium(III) oxalate hydrate
CAS number of osmium(V) fluoride
H2O + P4O6 = H3PO4 + PH3
KOH + KHCO3 = H2O + K2CO3
name of tetrahydrogenorthotellurate anion