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H2SO4 + KI + K3AsO4 = H2O + K2SO4 + I2 + K3AsO3

Input interpretation

H_2SO_4 sulfuric acid + KI potassium iodide + K3AsO4 ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine + K3AsO3
H_2SO_4 sulfuric acid + KI potassium iodide + K3AsO4 ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine + K3AsO3

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + KI + K3AsO4 ⟶ H_2O + K_2SO_4 + I_2 + K3AsO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KI + c_3 K3AsO4 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 I_2 + c_7 K3AsO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, I, K and As: 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 + 3 c_3 = 2 c_5 + 3 c_7 As: | c_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 + K3AsO4 ⟶ H_2O + K_2SO_4 + I_2 + K3AsO3
Balance the chemical equation algebraically: H_2SO_4 + KI + K3AsO4 ⟶ H_2O + K_2SO_4 + I_2 + K3AsO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KI + c_3 K3AsO4 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 I_2 + c_7 K3AsO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, I, K and As: 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 + 3 c_3 = 2 c_5 + 3 c_7 As: | c_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 + K3AsO4 ⟶ H_2O + K_2SO_4 + I_2 + K3AsO3

Structures

+ + K3AsO4 ⟶ + + + K3AsO3
+ + K3AsO4 ⟶ + + + K3AsO3

Names

sulfuric acid + potassium iodide + K3AsO4 ⟶ water + potassium sulfate + iodine + K3AsO3
sulfuric acid + potassium iodide + K3AsO4 ⟶ water + potassium sulfate + iodine + K3AsO3

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + KI + K3AsO4 ⟶ H_2O + K_2SO_4 + I_2 + K3AsO3 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 + K3AsO4 ⟶ H_2O + K_2SO_4 + I_2 + K3AsO3 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 K3AsO4 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 I_2 | 1 | 1 K3AsO3 | 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) K3AsO4 | 1 | -1 | ([K3AsO4])^(-1) H_2O | 1 | 1 | [H2O] K_2SO_4 | 1 | 1 | [K2SO4] I_2 | 1 | 1 | [I2] K3AsO3 | 1 | 1 | [K3AsO3] 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) ([K3AsO4])^(-1) [H2O] [K2SO4] [I2] [K3AsO3] = ([H2O] [K2SO4] [I2] [K3AsO3])/([H2SO4] ([KI])^2 [K3AsO4])
Construct the equilibrium constant, K, expression for: H_2SO_4 + KI + K3AsO4 ⟶ H_2O + K_2SO_4 + I_2 + K3AsO3 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 + K3AsO4 ⟶ H_2O + K_2SO_4 + I_2 + K3AsO3 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 K3AsO4 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 I_2 | 1 | 1 K3AsO3 | 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) K3AsO4 | 1 | -1 | ([K3AsO4])^(-1) H_2O | 1 | 1 | [H2O] K_2SO_4 | 1 | 1 | [K2SO4] I_2 | 1 | 1 | [I2] K3AsO3 | 1 | 1 | [K3AsO3] 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) ([K3AsO4])^(-1) [H2O] [K2SO4] [I2] [K3AsO3] = ([H2O] [K2SO4] [I2] [K3AsO3])/([H2SO4] ([KI])^2 [K3AsO4])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + KI + K3AsO4 ⟶ H_2O + K_2SO_4 + I_2 + K3AsO3 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 + K3AsO4 ⟶ H_2O + K_2SO_4 + I_2 + K3AsO3 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 K3AsO4 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 I_2 | 1 | 1 K3AsO3 | 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) K3AsO4 | 1 | -1 | -(Δ[K3AsO4])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) K3AsO3 | 1 | 1 | (Δ[K3AsO3])/(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[K3AsO4])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[I2])/(Δt) = (Δ[K3AsO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + KI + K3AsO4 ⟶ H_2O + K_2SO_4 + I_2 + K3AsO3 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 + K3AsO4 ⟶ H_2O + K_2SO_4 + I_2 + K3AsO3 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 K3AsO4 | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 I_2 | 1 | 1 K3AsO3 | 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) K3AsO4 | 1 | -1 | -(Δ[K3AsO4])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) K3AsO3 | 1 | 1 | (Δ[K3AsO3])/(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[K3AsO4])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[I2])/(Δt) = (Δ[K3AsO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | potassium iodide | K3AsO4 | water | potassium sulfate | iodine | K3AsO3 formula | H_2SO_4 | KI | K3AsO4 | H_2O | K_2SO_4 | I_2 | K3AsO3 Hill formula | H_2O_4S | IK | AsK3O4 | H_2O | K_2O_4S | I_2 | AsK3O3 name | sulfuric acid | potassium iodide | | water | potassium sulfate | iodine | IUPAC name | sulfuric acid | potassium iodide | | water | dipotassium sulfate | molecular iodine |
| sulfuric acid | potassium iodide | K3AsO4 | water | potassium sulfate | iodine | K3AsO3 formula | H_2SO_4 | KI | K3AsO4 | H_2O | K_2SO_4 | I_2 | K3AsO3 Hill formula | H_2O_4S | IK | AsK3O4 | H_2O | K_2O_4S | I_2 | AsK3O3 name | sulfuric acid | potassium iodide | | water | potassium sulfate | iodine | IUPAC name | sulfuric acid | potassium iodide | | water | dipotassium sulfate | molecular iodine |

Substance properties

| sulfuric acid | potassium iodide | K3AsO4 | water | potassium sulfate | iodine | K3AsO3 molar mass | 98.07 g/mol | 166.0028 g/mol | 256.212 g/mol | 18.015 g/mol | 174.25 g/mol | 253.80894 g/mol | 240.213 g/mol phase | liquid (at STP) | solid (at STP) | | liquid (at STP) | | solid (at STP) | melting point | 10.371 °C | 681 °C | | 0 °C | | 113 °C | boiling point | 279.6 °C | 1330 °C | | 99.9839 °C | | 184 °C | density | 1.8305 g/cm^3 | 3.123 g/cm^3 | | 1 g/cm^3 | | 4.94 g/cm^3 | solubility in water | very soluble | | | | soluble | | surface tension | 0.0735 N/m | | | 0.0728 N/m | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | 0.0010227 Pa s (at 732.9 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | 0.00227 Pa s (at 116 °C) | odor | odorless | | | odorless | | |
| sulfuric acid | potassium iodide | K3AsO4 | water | potassium sulfate | iodine | K3AsO3 molar mass | 98.07 g/mol | 166.0028 g/mol | 256.212 g/mol | 18.015 g/mol | 174.25 g/mol | 253.80894 g/mol | 240.213 g/mol phase | liquid (at STP) | solid (at STP) | | liquid (at STP) | | solid (at STP) | melting point | 10.371 °C | 681 °C | | 0 °C | | 113 °C | boiling point | 279.6 °C | 1330 °C | | 99.9839 °C | | 184 °C | density | 1.8305 g/cm^3 | 3.123 g/cm^3 | | 1 g/cm^3 | | 4.94 g/cm^3 | solubility in water | very soluble | | | | soluble | | surface tension | 0.0735 N/m | | | 0.0728 N/m | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | 0.0010227 Pa s (at 732.9 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | 0.00227 Pa s (at 116 °C) | odor | odorless | | | odorless | | |

Units

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