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H2SO4 + KI + Na3AsO4 = H2O + K2SO4 + I2 + Na3AsO3

Input interpretation

H_2SO_4 sulfuric acid + KI potassium iodide + AsNa_3O_4 arsenic acid, trisodium salt ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine + Na3AsO3
H_2SO_4 sulfuric acid + KI potassium iodide + AsNa_3O_4 arsenic acid, trisodium salt ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine + Na3AsO3

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + KI + AsNa_3O_4 ⟶ H_2O + K_2SO_4 + I_2 + Na3AsO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KI + c_3 AsNa_3O_4 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 I_2 + c_7 Na3AsO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, I, K, As and Na: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 4 c_3 = c_4 + 4 c_5 + 3 c_7 S: | c_1 = c_5 I: | c_2 = 2 c_6 K: | c_2 = 2 c_5 As: | c_3 = c_7 Na: | 3 c_3 = 3 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 1 c_6 = 1 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 2 KI + AsNa_3O_4 ⟶ H_2O + K_2SO_4 + I_2 + Na3AsO3
Balance the chemical equation algebraically: H_2SO_4 + KI + AsNa_3O_4 ⟶ H_2O + K_2SO_4 + I_2 + Na3AsO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KI + c_3 AsNa_3O_4 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 I_2 + c_7 Na3AsO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, I, K, As and Na: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 4 c_3 = c_4 + 4 c_5 + 3 c_7 S: | c_1 = c_5 I: | c_2 = 2 c_6 K: | c_2 = 2 c_5 As: | c_3 = c_7 Na: | 3 c_3 = 3 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 1 c_6 = 1 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 2 KI + AsNa_3O_4 ⟶ H_2O + K_2SO_4 + I_2 + Na3AsO3

Structures

+ + ⟶ + + + Na3AsO3
+ + ⟶ + + + Na3AsO3

Names

sulfuric acid + potassium iodide + arsenic acid, trisodium salt ⟶ water + potassium sulfate + iodine + Na3AsO3
sulfuric acid + potassium iodide + arsenic acid, trisodium salt ⟶ water + potassium sulfate + iodine + Na3AsO3

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + KI + AsNa_3O_4 ⟶ H_2O + K_2SO_4 + I_2 + Na3AsO3 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 + 2 KI + AsNa_3O_4 ⟶ H_2O + K_2SO_4 + I_2 + Na3AsO3 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 KI | 2 | -2 AsNa_3O_4 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 I_2 | 1 | 1 Na3AsO3 | 1 | 1 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) KI | 2 | -2 | ([KI])^(-2) AsNa_3O_4 | 1 | -1 | ([AsNa3O4])^(-1) H_2O | 1 | 1 | [H2O] K_2SO_4 | 1 | 1 | [K2SO4] I_2 | 1 | 1 | [I2] Na3AsO3 | 1 | 1 | [Na3AsO3] 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) ([KI])^(-2) ([AsNa3O4])^(-1) [H2O] [K2SO4] [I2] [Na3AsO3] = ([H2O] [K2SO4] [I2] [Na3AsO3])/([H2SO4] ([KI])^2 [AsNa3O4])
Construct the equilibrium constant, K, expression for: H_2SO_4 + KI + AsNa_3O_4 ⟶ H_2O + K_2SO_4 + I_2 + Na3AsO3 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 + 2 KI + AsNa_3O_4 ⟶ H_2O + K_2SO_4 + I_2 + Na3AsO3 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 KI | 2 | -2 AsNa_3O_4 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 I_2 | 1 | 1 Na3AsO3 | 1 | 1 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) KI | 2 | -2 | ([KI])^(-2) AsNa_3O_4 | 1 | -1 | ([AsNa3O4])^(-1) H_2O | 1 | 1 | [H2O] K_2SO_4 | 1 | 1 | [K2SO4] I_2 | 1 | 1 | [I2] Na3AsO3 | 1 | 1 | [Na3AsO3] 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) ([KI])^(-2) ([AsNa3O4])^(-1) [H2O] [K2SO4] [I2] [Na3AsO3] = ([H2O] [K2SO4] [I2] [Na3AsO3])/([H2SO4] ([KI])^2 [AsNa3O4])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + KI + AsNa_3O_4 ⟶ H_2O + K_2SO_4 + I_2 + Na3AsO3 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 + 2 KI + AsNa_3O_4 ⟶ H_2O + K_2SO_4 + I_2 + Na3AsO3 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 KI | 2 | -2 AsNa_3O_4 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 I_2 | 1 | 1 Na3AsO3 | 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_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) KI | 2 | -2 | -1/2 (Δ[KI])/(Δt) AsNa_3O_4 | 1 | -1 | -(Δ[AsNa3O4])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) Na3AsO3 | 1 | 1 | (Δ[Na3AsO3])/(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) = -1/2 (Δ[KI])/(Δt) = -(Δ[AsNa3O4])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[I2])/(Δt) = (Δ[Na3AsO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + KI + AsNa_3O_4 ⟶ H_2O + K_2SO_4 + I_2 + Na3AsO3 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 + 2 KI + AsNa_3O_4 ⟶ H_2O + K_2SO_4 + I_2 + Na3AsO3 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 KI | 2 | -2 AsNa_3O_4 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 I_2 | 1 | 1 Na3AsO3 | 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_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) KI | 2 | -2 | -1/2 (Δ[KI])/(Δt) AsNa_3O_4 | 1 | -1 | -(Δ[AsNa3O4])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) Na3AsO3 | 1 | 1 | (Δ[Na3AsO3])/(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) = -1/2 (Δ[KI])/(Δt) = -(Δ[AsNa3O4])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[I2])/(Δt) = (Δ[Na3AsO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | potassium iodide | arsenic acid, trisodium salt | water | potassium sulfate | iodine | Na3AsO3 formula | H_2SO_4 | KI | AsNa_3O_4 | H_2O | K_2SO_4 | I_2 | Na3AsO3 Hill formula | H_2O_4S | IK | AsNa_3O_4 | H_2O | K_2O_4S | I_2 | AsNa3O3 name | sulfuric acid | potassium iodide | arsenic acid, trisodium salt | water | potassium sulfate | iodine | IUPAC name | sulfuric acid | potassium iodide | | water | dipotassium sulfate | molecular iodine |
| sulfuric acid | potassium iodide | arsenic acid, trisodium salt | water | potassium sulfate | iodine | Na3AsO3 formula | H_2SO_4 | KI | AsNa_3O_4 | H_2O | K_2SO_4 | I_2 | Na3AsO3 Hill formula | H_2O_4S | IK | AsNa_3O_4 | H_2O | K_2O_4S | I_2 | AsNa3O3 name | sulfuric acid | potassium iodide | arsenic acid, trisodium salt | water | potassium sulfate | iodine | IUPAC name | sulfuric acid | potassium iodide | | water | dipotassium sulfate | molecular iodine |

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