H2SO4 + KI = H2O + K2SO4 + I2 + H2S

H_2SO_4 (sulfuric acid) + KI (potassium iodide) ⟶ H_2O (water) + K_2SO_4 (potassium sulfate) + I_2 (iodine) + H_2S (hydrogen sulfide)

Balance the chemical equation algebraically: H_2SO_4 + KI ⟶ H_2O + K_2SO_4 + I_2 + H_2S 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 H_2S 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 + 2 c_6 O: | 4 c_1 = c_3 + 4 c_4 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_6 = 1 and solve the system of equations for the remaining coefficients: c_1 = 5 c_2 = 8 c_3 = 4 c_4 = 4 c_5 = 4 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 5 H_2SO_4 + 8 KI ⟶ 4 H_2O + 4 K_2SO_4 + 4 I_2 + H_2S

+ ⟶ + + +

sulfuric acid + potassium iodide ⟶ water + potassium sulfate + iodine + hydrogen sulfide

Construct the equilibrium constant, K, expression for: H_2SO_4 + KI ⟶ H_2O + K_2SO_4 + I_2 + H_2S 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: 5 H_2SO_4 + 8 KI ⟶ 4 H_2O + 4 K_2SO_4 + 4 I_2 + H_2S 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 | 5 | -5 KI | 8 | -8 H_2O | 4 | 4 K_2SO_4 | 4 | 4 I_2 | 4 | 4 H_2S | 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 | 5 | -5 | ([H2SO4])^(-5) KI | 8 | -8 | ([KI])^(-8) H_2O | 4 | 4 | ([H2O])^4 K_2SO_4 | 4 | 4 | ([K2SO4])^4 I_2 | 4 | 4 | ([I2])^4 H_2S | 1 | 1 | [H2S] 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])^(-5) ([KI])^(-8) ([H2O])^4 ([K2SO4])^4 ([I2])^4 [H2S] = (([H2O])^4 ([K2SO4])^4 ([I2])^4 [H2S])/(([H2SO4])^5 ([KI])^8)

Construct the rate of reaction expression for: H_2SO_4 + KI ⟶ H_2O + K_2SO_4 + I_2 + H_2S 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: 5 H_2SO_4 + 8 KI ⟶ 4 H_2O + 4 K_2SO_4 + 4 I_2 + H_2S 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 | 5 | -5 KI | 8 | -8 H_2O | 4 | 4 K_2SO_4 | 4 | 4 I_2 | 4 | 4 H_2S | 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 | 5 | -5 | -1/5 (Δ[H2SO4])/(Δt) KI | 8 | -8 | -1/8 (Δ[KI])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) K_2SO_4 | 4 | 4 | 1/4 (Δ[K2SO4])/(Δt) I_2 | 4 | 4 | 1/4 (Δ[I2])/(Δt) H_2S | 1 | 1 | (Δ[H2S])/(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 = -1/5 (Δ[H2SO4])/(Δt) = -1/8 (Δ[KI])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/4 (Δ[K2SO4])/(Δt) = 1/4 (Δ[I2])/(Δt) = (Δ[H2S])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | potassium iodide | water | potassium sulfate | iodine | hydrogen sulfide formula | H_2SO_4 | KI | H_2O | K_2SO_4 | I_2 | H_2S Hill formula | H_2O_4S | IK | H_2O | K_2O_4S | I_2 | H_2S name | sulfuric acid | potassium iodide | water | potassium sulfate | iodine | hydrogen sulfide IUPAC name | sulfuric acid | potassium iodide | water | dipotassium sulfate | molecular iodine | hydrogen sulfide

| sulfuric acid | potassium iodide | water | potassium sulfate | iodine | hydrogen sulfide molar mass | 98.07 g/mol | 166.0028 g/mol | 18.015 g/mol | 174.25 g/mol | 253.80894 g/mol | 34.08 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 | -85 °C boiling point | 279.6 °C | 1330 °C | 99.9839 °C | | 184 °C | -60 °C density | 1.8305 g/cm^3 | 3.123 g/cm^3 | 1 g/cm^3 | | 4.94 g/cm^3 | 0.001393 g/cm^3 (at 25 °C) 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) | 1.239×10^-5 Pa s (at 25 °C) odor | odorless | | odorless | | |