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H2SO4 + HI + KNO2 = H2O + K2SO4 + I2 + NO

Input interpretation

H_2SO_4 sulfuric acid + HI hydrogen iodide + KNO_2 potassium nitrite ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine + NO nitric oxide
H_2SO_4 sulfuric acid + HI hydrogen iodide + KNO_2 potassium nitrite ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine + NO nitric oxide

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + HI + KNO_2 ⟶ 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 HI + c_3 KNO_2 ⟶ 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 + c_2 = 2 c_4 O: | 4 c_1 + 2 c_3 = c_4 + 4 c_5 + c_7 S: | c_1 = c_5 I: | c_2 = 2 c_6 K: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 2 c_4 = 2 c_5 = 1 c_6 = 1 c_7 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 2 HI + 2 KNO_2 ⟶ 2 H_2O + K_2SO_4 + I_2 + 2 NO
Balance the chemical equation algebraically: H_2SO_4 + HI + KNO_2 ⟶ 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 HI + c_3 KNO_2 ⟶ 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 + c_2 = 2 c_4 O: | 4 c_1 + 2 c_3 = c_4 + 4 c_5 + c_7 S: | c_1 = c_5 I: | c_2 = 2 c_6 K: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 2 c_4 = 2 c_5 = 1 c_6 = 1 c_7 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 2 HI + 2 KNO_2 ⟶ 2 H_2O + K_2SO_4 + I_2 + 2 NO

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

sulfuric acid + hydrogen iodide + potassium nitrite ⟶ water + potassium sulfate + iodine + nitric oxide
sulfuric acid + hydrogen iodide + potassium nitrite ⟶ water + potassium sulfate + iodine + nitric oxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + HI + KNO_2 ⟶ 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: H_2SO_4 + 2 HI + 2 KNO_2 ⟶ 2 H_2O + K_2SO_4 + 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 | 1 | -1 HI | 2 | -2 KNO_2 | 2 | -2 H_2O | 2 | 2 K_2SO_4 | 1 | 1 I_2 | 1 | 1 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 | 1 | -1 | ([H2SO4])^(-1) HI | 2 | -2 | ([HI])^(-2) KNO_2 | 2 | -2 | ([KNO2])^(-2) H_2O | 2 | 2 | ([H2O])^2 K_2SO_4 | 1 | 1 | [K2SO4] I_2 | 1 | 1 | [I2] 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])^(-1) ([HI])^(-2) ([KNO2])^(-2) ([H2O])^2 [K2SO4] [I2] ([NO])^2 = (([H2O])^2 [K2SO4] [I2] ([NO])^2)/([H2SO4] ([HI])^2 ([KNO2])^2)
Construct the equilibrium constant, K, expression for: H_2SO_4 + HI + KNO_2 ⟶ 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: H_2SO_4 + 2 HI + 2 KNO_2 ⟶ 2 H_2O + K_2SO_4 + 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 | 1 | -1 HI | 2 | -2 KNO_2 | 2 | -2 H_2O | 2 | 2 K_2SO_4 | 1 | 1 I_2 | 1 | 1 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 | 1 | -1 | ([H2SO4])^(-1) HI | 2 | -2 | ([HI])^(-2) KNO_2 | 2 | -2 | ([KNO2])^(-2) H_2O | 2 | 2 | ([H2O])^2 K_2SO_4 | 1 | 1 | [K2SO4] I_2 | 1 | 1 | [I2] 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])^(-1) ([HI])^(-2) ([KNO2])^(-2) ([H2O])^2 [K2SO4] [I2] ([NO])^2 = (([H2O])^2 [K2SO4] [I2] ([NO])^2)/([H2SO4] ([HI])^2 ([KNO2])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + HI + KNO_2 ⟶ 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: H_2SO_4 + 2 HI + 2 KNO_2 ⟶ 2 H_2O + K_2SO_4 + 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 | 1 | -1 HI | 2 | -2 KNO_2 | 2 | -2 H_2O | 2 | 2 K_2SO_4 | 1 | 1 I_2 | 1 | 1 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 | 1 | -1 | -(Δ[H2SO4])/(Δt) HI | 2 | -2 | -1/2 (Δ[HI])/(Δt) KNO_2 | 2 | -2 | -1/2 (Δ[KNO2])/(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) 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 = -(Δ[H2SO4])/(Δt) = -1/2 (Δ[HI])/(Δt) = -1/2 (Δ[KNO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[I2])/(Δt) = 1/2 (Δ[NO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + HI + KNO_2 ⟶ 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: H_2SO_4 + 2 HI + 2 KNO_2 ⟶ 2 H_2O + K_2SO_4 + 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 | 1 | -1 HI | 2 | -2 KNO_2 | 2 | -2 H_2O | 2 | 2 K_2SO_4 | 1 | 1 I_2 | 1 | 1 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 | 1 | -1 | -(Δ[H2SO4])/(Δt) HI | 2 | -2 | -1/2 (Δ[HI])/(Δt) KNO_2 | 2 | -2 | -1/2 (Δ[KNO2])/(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) 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 = -(Δ[H2SO4])/(Δt) = -1/2 (Δ[HI])/(Δt) = -1/2 (Δ[KNO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[I2])/(Δt) = 1/2 (Δ[NO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | hydrogen iodide | potassium nitrite | water | potassium sulfate | iodine | nitric oxide formula | H_2SO_4 | HI | KNO_2 | H_2O | K_2SO_4 | I_2 | NO Hill formula | H_2O_4S | HI | KNO_2 | H_2O | K_2O_4S | I_2 | NO name | sulfuric acid | hydrogen iodide | potassium nitrite | water | potassium sulfate | iodine | nitric oxide IUPAC name | sulfuric acid | hydrogen iodide | potassium nitrite | water | dipotassium sulfate | molecular iodine | nitric oxide
| sulfuric acid | hydrogen iodide | potassium nitrite | water | potassium sulfate | iodine | nitric oxide formula | H_2SO_4 | HI | KNO_2 | H_2O | K_2SO_4 | I_2 | NO Hill formula | H_2O_4S | HI | KNO_2 | H_2O | K_2O_4S | I_2 | NO name | sulfuric acid | hydrogen iodide | potassium nitrite | water | potassium sulfate | iodine | nitric oxide IUPAC name | sulfuric acid | hydrogen iodide | potassium nitrite | water | dipotassium sulfate | molecular iodine | nitric oxide

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