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H2O + I2 + Na3AsO3 = HI + Na3AsO4

Input interpretation

H_2O water + I_2 iodine + Na3AsO3 ⟶ HI hydrogen iodide + AsNa_3O_4 arsenic acid, trisodium salt
H_2O water + I_2 iodine + Na3AsO3 ⟶ HI hydrogen iodide + AsNa_3O_4 arsenic acid, trisodium salt

Balanced equation

Balance the chemical equation algebraically: H_2O + I_2 + Na3AsO3 ⟶ HI + AsNa_3O_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 I_2 + c_3 Na3AsO3 ⟶ c_4 HI + c_5 AsNa_3O_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, I, Na and As: H: | 2 c_1 = c_4 O: | c_1 + 3 c_3 = 4 c_5 I: | 2 c_2 = c_4 Na: | 3 c_3 = 3 c_5 As: | c_3 = 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 = 1 c_3 = 1 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + I_2 + Na3AsO3 ⟶ 2 HI + AsNa_3O_4
Balance the chemical equation algebraically: H_2O + I_2 + Na3AsO3 ⟶ HI + AsNa_3O_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 I_2 + c_3 Na3AsO3 ⟶ c_4 HI + c_5 AsNa_3O_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, I, Na and As: H: | 2 c_1 = c_4 O: | c_1 + 3 c_3 = 4 c_5 I: | 2 c_2 = c_4 Na: | 3 c_3 = 3 c_5 As: | c_3 = 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 = 1 c_3 = 1 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + I_2 + Na3AsO3 ⟶ 2 HI + AsNa_3O_4

Structures

+ + Na3AsO3 ⟶ +
+ + Na3AsO3 ⟶ +

Names

water + iodine + Na3AsO3 ⟶ hydrogen iodide + arsenic acid, trisodium salt
water + iodine + Na3AsO3 ⟶ hydrogen iodide + arsenic acid, trisodium salt

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + I_2 + Na3AsO3 ⟶ HI + AsNa_3O_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: H_2O + I_2 + Na3AsO3 ⟶ 2 HI + AsNa_3O_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 H_2O | 1 | -1 I_2 | 1 | -1 Na3AsO3 | 1 | -1 HI | 2 | 2 AsNa_3O_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) I_2 | 1 | -1 | ([I2])^(-1) Na3AsO3 | 1 | -1 | ([Na3AsO3])^(-1) HI | 2 | 2 | ([HI])^2 AsNa_3O_4 | 1 | 1 | [AsNa3O4] 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])^(-1) ([I2])^(-1) ([Na3AsO3])^(-1) ([HI])^2 [AsNa3O4] = (([HI])^2 [AsNa3O4])/([H2O] [I2] [Na3AsO3])
Construct the equilibrium constant, K, expression for: H_2O + I_2 + Na3AsO3 ⟶ HI + AsNa_3O_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: H_2O + I_2 + Na3AsO3 ⟶ 2 HI + AsNa_3O_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 H_2O | 1 | -1 I_2 | 1 | -1 Na3AsO3 | 1 | -1 HI | 2 | 2 AsNa_3O_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) I_2 | 1 | -1 | ([I2])^(-1) Na3AsO3 | 1 | -1 | ([Na3AsO3])^(-1) HI | 2 | 2 | ([HI])^2 AsNa_3O_4 | 1 | 1 | [AsNa3O4] 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])^(-1) ([I2])^(-1) ([Na3AsO3])^(-1) ([HI])^2 [AsNa3O4] = (([HI])^2 [AsNa3O4])/([H2O] [I2] [Na3AsO3])

Rate of reaction

Construct the rate of reaction expression for: H_2O + I_2 + Na3AsO3 ⟶ HI + AsNa_3O_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: H_2O + I_2 + Na3AsO3 ⟶ 2 HI + AsNa_3O_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 H_2O | 1 | -1 I_2 | 1 | -1 Na3AsO3 | 1 | -1 HI | 2 | 2 AsNa_3O_4 | 1 | 1 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 | 1 | -1 | -(Δ[H2O])/(Δt) I_2 | 1 | -1 | -(Δ[I2])/(Δt) Na3AsO3 | 1 | -1 | -(Δ[Na3AsO3])/(Δt) HI | 2 | 2 | 1/2 (Δ[HI])/(Δt) AsNa_3O_4 | 1 | 1 | (Δ[AsNa3O4])/(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[H2O])/(Δt) = -(Δ[I2])/(Δt) = -(Δ[Na3AsO3])/(Δt) = 1/2 (Δ[HI])/(Δt) = (Δ[AsNa3O4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + I_2 + Na3AsO3 ⟶ HI + AsNa_3O_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: H_2O + I_2 + Na3AsO3 ⟶ 2 HI + AsNa_3O_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 H_2O | 1 | -1 I_2 | 1 | -1 Na3AsO3 | 1 | -1 HI | 2 | 2 AsNa_3O_4 | 1 | 1 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 | 1 | -1 | -(Δ[H2O])/(Δt) I_2 | 1 | -1 | -(Δ[I2])/(Δt) Na3AsO3 | 1 | -1 | -(Δ[Na3AsO3])/(Δt) HI | 2 | 2 | 1/2 (Δ[HI])/(Δt) AsNa_3O_4 | 1 | 1 | (Δ[AsNa3O4])/(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[H2O])/(Δt) = -(Δ[I2])/(Δt) = -(Δ[Na3AsO3])/(Δt) = 1/2 (Δ[HI])/(Δt) = (Δ[AsNa3O4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | iodine | Na3AsO3 | hydrogen iodide | arsenic acid, trisodium salt formula | H_2O | I_2 | Na3AsO3 | HI | AsNa_3O_4 Hill formula | H_2O | I_2 | AsNa3O3 | HI | AsNa_3O_4 name | water | iodine | | hydrogen iodide | arsenic acid, trisodium salt IUPAC name | water | molecular iodine | | hydrogen iodide |
| water | iodine | Na3AsO3 | hydrogen iodide | arsenic acid, trisodium salt formula | H_2O | I_2 | Na3AsO3 | HI | AsNa_3O_4 Hill formula | H_2O | I_2 | AsNa3O3 | HI | AsNa_3O_4 name | water | iodine | | hydrogen iodide | arsenic acid, trisodium salt IUPAC name | water | molecular iodine | | hydrogen iodide |

Substance properties

| water | iodine | Na3AsO3 | hydrogen iodide | arsenic acid, trisodium salt molar mass | 18.015 g/mol | 253.80894 g/mol | 191.888 g/mol | 127.912 g/mol | 207.887 g/mol phase | liquid (at STP) | solid (at STP) | | gas (at STP) | solid (at STP) melting point | 0 °C | 113 °C | | -50.76 °C | 1260 °C boiling point | 99.9839 °C | 184 °C | | -35.55 °C | density | 1 g/cm^3 | 4.94 g/cm^3 | | 0.005228 g/cm^3 (at 25 °C) | 2.81 g/cm^3 solubility in water | | | | very soluble | surface tension | 0.0728 N/m | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 0.00227 Pa s (at 116 °C) | | 0.001321 Pa s (at -39 °C) | odor | odorless | | | |
| water | iodine | Na3AsO3 | hydrogen iodide | arsenic acid, trisodium salt molar mass | 18.015 g/mol | 253.80894 g/mol | 191.888 g/mol | 127.912 g/mol | 207.887 g/mol phase | liquid (at STP) | solid (at STP) | | gas (at STP) | solid (at STP) melting point | 0 °C | 113 °C | | -50.76 °C | 1260 °C boiling point | 99.9839 °C | 184 °C | | -35.55 °C | density | 1 g/cm^3 | 4.94 g/cm^3 | | 0.005228 g/cm^3 (at 25 °C) | 2.81 g/cm^3 solubility in water | | | | very soluble | surface tension | 0.0728 N/m | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 0.00227 Pa s (at 116 °C) | | 0.001321 Pa s (at -39 °C) | odor | odorless | | | |

Units

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