H2SO4 + KI + KNO3 = H2O + K2SO4 + I2 + NO

H_2SO_4 sulfuric acid + KI potassium iodide + KNO_3 potassium nitrate ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine + NO nitric oxide

Balance the chemical equation algebraically: H_2SO_4 + KI + KNO_3 ⟶ H_2O + K_2SO_4 + I_2 + NO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KI + c_3 KNO_3 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 I_2 + c_7 NO Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, I, K and N: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 3 c_3 = c_4 + 4 c_5 + c_7 S: | c_1 = c_5 I: | c_2 = 2 c_6 K: | c_2 + c_3 = 2 c_5 N: | 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 1 c_4 = 2 c_5 = 2 c_6 = 3/2 c_7 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 4 c_2 = 6 c_3 = 2 c_4 = 4 c_5 = 4 c_6 = 3 c_7 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2SO_4 + 6 KI + 2 KNO_3 ⟶ 4 H_2O + 4 K_2SO_4 + 3 I_2 + 2 NO

+ + ⟶ + + +

sulfuric acid + potassium iodide + potassium nitrate ⟶ water + potassium sulfate + iodine + nitric oxide

Construct the equilibrium constant, K, expression for: H_2SO_4 + KI + KNO_3 ⟶ H_2O + K_2SO_4 + I_2 + NO 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: 4 H_2SO_4 + 6 KI + 2 KNO_3 ⟶ 4 H_2O + 4 K_2SO_4 + 3 I_2 + 2 NO 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 | 4 | -4 KI | 6 | -6 KNO_3 | 2 | -2 H_2O | 4 | 4 K_2SO_4 | 4 | 4 I_2 | 3 | 3 NO | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 4 | -4 | ([H2SO4])^(-4) KI | 6 | -6 | ([KI])^(-6) KNO_3 | 2 | -2 | ([KNO3])^(-2) H_2O | 4 | 4 | ([H2O])^4 K_2SO_4 | 4 | 4 | ([K2SO4])^4 I_2 | 3 | 3 | ([I2])^3 NO | 2 | 2 | ([NO])^2 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])^(-4) ([KI])^(-6) ([KNO3])^(-2) ([H2O])^4 ([K2SO4])^4 ([I2])^3 ([NO])^2 = (([H2O])^4 ([K2SO4])^4 ([I2])^3 ([NO])^2)/(([H2SO4])^4 ([KI])^6 ([KNO3])^2)

Construct the rate of reaction expression for: H_2SO_4 + KI + KNO_3 ⟶ H_2O + K_2SO_4 + I_2 + NO 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: 4 H_2SO_4 + 6 KI + 2 KNO_3 ⟶ 4 H_2O + 4 K_2SO_4 + 3 I_2 + 2 NO 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 | 4 | -4 KI | 6 | -6 KNO_3 | 2 | -2 H_2O | 4 | 4 K_2SO_4 | 4 | 4 I_2 | 3 | 3 NO | 2 | 2 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 | 4 | -4 | -1/4 (Δ[H2SO4])/(Δt) KI | 6 | -6 | -1/6 (Δ[KI])/(Δt) KNO_3 | 2 | -2 | -1/2 (Δ[KNO3])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) K_2SO_4 | 4 | 4 | 1/4 (Δ[K2SO4])/(Δt) I_2 | 3 | 3 | 1/3 (Δ[I2])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(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 = -1/4 (Δ[H2SO4])/(Δt) = -1/6 (Δ[KI])/(Δt) = -1/2 (Δ[KNO3])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/4 (Δ[K2SO4])/(Δt) = 1/3 (Δ[I2])/(Δt) = 1/2 (Δ[NO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | potassium iodide | potassium nitrate | water | potassium sulfate | iodine | nitric oxide formula | H_2SO_4 | KI | KNO_3 | H_2O | K_2SO_4 | I_2 | NO Hill formula | H_2O_4S | IK | KNO_3 | H_2O | K_2O_4S | I_2 | NO name | sulfuric acid | potassium iodide | potassium nitrate | water | potassium sulfate | iodine | nitric oxide IUPAC name | sulfuric acid | potassium iodide | potassium nitrate | water | dipotassium sulfate | molecular iodine | nitric oxide

| sulfuric acid | potassium iodide | potassium nitrate | water | potassium sulfate | iodine | nitric oxide molar mass | 98.07 g/mol | 166.0028 g/mol | 101.1 g/mol | 18.015 g/mol | 174.25 g/mol | 253.80894 g/mol | 30.006 g/mol phase | liquid (at STP) | solid (at STP) | solid (at STP) | liquid (at STP) | | solid (at STP) | gas (at STP) melting point | 10.371 °C | 681 °C | 334 °C | 0 °C | | 113 °C | -163.6 °C boiling point | 279.6 °C | 1330 °C | | 99.9839 °C | | 184 °C | -151.7 °C density | 1.8305 g/cm^3 | 3.123 g/cm^3 | | 1 g/cm^3 | | 4.94 g/cm^3 | 0.001226 g/cm^3 (at 25 °C) solubility in water | very soluble | | 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) | 1.911×10^-5 Pa s (at 25 °C) odor | odorless | | odorless | odorless | | |