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H2SO4 + KI = H2O + K2SO4 + I2 + SO2

Input interpretation

H_2SO_4 sulfuric acid + KI potassium iodide ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine + SO_2 sulfur dioxide
H_2SO_4 sulfuric acid + KI potassium iodide ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine + SO_2 sulfur dioxide

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + KI ⟶ H_2O + K_2SO_4 + I_2 + SO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KI ⟶ c_3 H_2O + c_4 K_2SO_4 + c_5 I_2 + c_6 SO_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 = 2 c_3 O: | 4 c_1 = c_3 + 4 c_4 + 2 c_6 S: | c_1 = c_4 + c_6 I: | c_2 = 2 c_5 K: | c_2 = 2 c_4 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 2 c_4 = 1 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2SO_4 + 2 KI ⟶ 2 H_2O + K_2SO_4 + I_2 + SO_2
Balance the chemical equation algebraically: H_2SO_4 + KI ⟶ H_2O + K_2SO_4 + I_2 + SO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KI ⟶ c_3 H_2O + c_4 K_2SO_4 + c_5 I_2 + c_6 SO_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 = 2 c_3 O: | 4 c_1 = c_3 + 4 c_4 + 2 c_6 S: | c_1 = c_4 + c_6 I: | c_2 = 2 c_5 K: | c_2 = 2 c_4 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 2 c_4 = 1 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2SO_4 + 2 KI ⟶ 2 H_2O + K_2SO_4 + I_2 + SO_2

Structures

+ ⟶ + + +
+ ⟶ + + +

Names

sulfuric acid + potassium iodide ⟶ water + potassium sulfate + iodine + sulfur dioxide
sulfuric acid + potassium iodide ⟶ water + potassium sulfate + iodine + sulfur dioxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + KI ⟶ H_2O + K_2SO_4 + I_2 + SO_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: 2 H_2SO_4 + 2 KI ⟶ 2 H_2O + K_2SO_4 + I_2 + SO_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 | 2 | -2 KI | 2 | -2 H_2O | 2 | 2 K_2SO_4 | 1 | 1 I_2 | 1 | 1 SO_2 | 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 | 2 | -2 | ([H2SO4])^(-2) KI | 2 | -2 | ([KI])^(-2) H_2O | 2 | 2 | ([H2O])^2 K_2SO_4 | 1 | 1 | [K2SO4] I_2 | 1 | 1 | [I2] SO_2 | 1 | 1 | [SO2] 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])^(-2) ([KI])^(-2) ([H2O])^2 [K2SO4] [I2] [SO2] = (([H2O])^2 [K2SO4] [I2] [SO2])/(([H2SO4])^2 ([KI])^2)
Construct the equilibrium constant, K, expression for: H_2SO_4 + KI ⟶ H_2O + K_2SO_4 + I_2 + SO_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: 2 H_2SO_4 + 2 KI ⟶ 2 H_2O + K_2SO_4 + I_2 + SO_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 | 2 | -2 KI | 2 | -2 H_2O | 2 | 2 K_2SO_4 | 1 | 1 I_2 | 1 | 1 SO_2 | 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 | 2 | -2 | ([H2SO4])^(-2) KI | 2 | -2 | ([KI])^(-2) H_2O | 2 | 2 | ([H2O])^2 K_2SO_4 | 1 | 1 | [K2SO4] I_2 | 1 | 1 | [I2] SO_2 | 1 | 1 | [SO2] 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])^(-2) ([KI])^(-2) ([H2O])^2 [K2SO4] [I2] [SO2] = (([H2O])^2 [K2SO4] [I2] [SO2])/(([H2SO4])^2 ([KI])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + KI ⟶ H_2O + K_2SO_4 + I_2 + SO_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: 2 H_2SO_4 + 2 KI ⟶ 2 H_2O + K_2SO_4 + I_2 + SO_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 | 2 | -2 KI | 2 | -2 H_2O | 2 | 2 K_2SO_4 | 1 | 1 I_2 | 1 | 1 SO_2 | 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 | 2 | -2 | -1/2 (Δ[H2SO4])/(Δt) KI | 2 | -2 | -1/2 (Δ[KI])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) SO_2 | 1 | 1 | (Δ[SO2])/(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 = -1/2 (Δ[H2SO4])/(Δt) = -1/2 (Δ[KI])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[I2])/(Δt) = (Δ[SO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + KI ⟶ H_2O + K_2SO_4 + I_2 + SO_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: 2 H_2SO_4 + 2 KI ⟶ 2 H_2O + K_2SO_4 + I_2 + SO_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 | 2 | -2 KI | 2 | -2 H_2O | 2 | 2 K_2SO_4 | 1 | 1 I_2 | 1 | 1 SO_2 | 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 | 2 | -2 | -1/2 (Δ[H2SO4])/(Δt) KI | 2 | -2 | -1/2 (Δ[KI])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) SO_2 | 1 | 1 | (Δ[SO2])/(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 = -1/2 (Δ[H2SO4])/(Δt) = -1/2 (Δ[KI])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[I2])/(Δt) = (Δ[SO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | potassium iodide | water | potassium sulfate | iodine | sulfur dioxide formula | H_2SO_4 | KI | H_2O | K_2SO_4 | I_2 | SO_2 Hill formula | H_2O_4S | IK | H_2O | K_2O_4S | I_2 | O_2S name | sulfuric acid | potassium iodide | water | potassium sulfate | iodine | sulfur dioxide IUPAC name | sulfuric acid | potassium iodide | water | dipotassium sulfate | molecular iodine | sulfur dioxide
| sulfuric acid | potassium iodide | water | potassium sulfate | iodine | sulfur dioxide formula | H_2SO_4 | KI | H_2O | K_2SO_4 | I_2 | SO_2 Hill formula | H_2O_4S | IK | H_2O | K_2O_4S | I_2 | O_2S name | sulfuric acid | potassium iodide | water | potassium sulfate | iodine | sulfur dioxide IUPAC name | sulfuric acid | potassium iodide | water | dipotassium sulfate | molecular iodine | sulfur dioxide

Substance properties

| sulfuric acid | potassium iodide | water | potassium sulfate | iodine | sulfur dioxide molar mass | 98.07 g/mol | 166.0028 g/mol | 18.015 g/mol | 174.25 g/mol | 253.80894 g/mol | 64.06 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | | solid (at STP) | gas (at STP) melting point | 10.371 °C | 681 °C | 0 °C | | 113 °C | -73 °C boiling point | 279.6 °C | 1330 °C | 99.9839 °C | | 184 °C | -10 °C density | 1.8305 g/cm^3 | 3.123 g/cm^3 | 1 g/cm^3 | | 4.94 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) solubility in water | very soluble | | | soluble | | surface tension | 0.0735 N/m | | 0.0728 N/m | | | 0.02859 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) | 1.282×10^-5 Pa s (at 25 °C) odor | odorless | | odorless | | |
| sulfuric acid | potassium iodide | water | potassium sulfate | iodine | sulfur dioxide molar mass | 98.07 g/mol | 166.0028 g/mol | 18.015 g/mol | 174.25 g/mol | 253.80894 g/mol | 64.06 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | | solid (at STP) | gas (at STP) melting point | 10.371 °C | 681 °C | 0 °C | | 113 °C | -73 °C boiling point | 279.6 °C | 1330 °C | 99.9839 °C | | 184 °C | -10 °C density | 1.8305 g/cm^3 | 3.123 g/cm^3 | 1 g/cm^3 | | 4.94 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) solubility in water | very soluble | | | soluble | | surface tension | 0.0735 N/m | | 0.0728 N/m | | | 0.02859 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) | 1.282×10^-5 Pa s (at 25 °C) odor | odorless | | odorless | | |

Units

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