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HCl + KI + HNO2 = H2O + I2 + KCl + N2

Input interpretation

HCl hydrogen chloride + KI potassium iodide + HNO_2 nitrous acid ⟶ H_2O water + I_2 iodine + KCl potassium chloride + N_2 nitrogen
HCl hydrogen chloride + KI potassium iodide + HNO_2 nitrous acid ⟶ H_2O water + I_2 iodine + KCl potassium chloride + N_2 nitrogen

Balanced equation

Balance the chemical equation algebraically: HCl + KI + HNO_2 ⟶ H_2O + I_2 + KCl + N_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KI + c_3 HNO_2 ⟶ c_4 H_2O + c_5 I_2 + c_6 KCl + c_7 N_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, I, K, N and O: Cl: | c_1 = c_6 H: | c_1 + c_3 = 2 c_4 I: | c_2 = 2 c_5 K: | c_2 = c_6 N: | c_3 = 2 c_7 O: | 2 c_3 = 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_7 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 6 c_3 = 2 c_4 = 4 c_5 = 3 c_6 = 6 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HCl + 6 KI + 2 HNO_2 ⟶ 4 H_2O + 3 I_2 + 6 KCl + N_2
Balance the chemical equation algebraically: HCl + KI + HNO_2 ⟶ H_2O + I_2 + KCl + N_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KI + c_3 HNO_2 ⟶ c_4 H_2O + c_5 I_2 + c_6 KCl + c_7 N_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, I, K, N and O: Cl: | c_1 = c_6 H: | c_1 + c_3 = 2 c_4 I: | c_2 = 2 c_5 K: | c_2 = c_6 N: | c_3 = 2 c_7 O: | 2 c_3 = 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_7 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 6 c_3 = 2 c_4 = 4 c_5 = 3 c_6 = 6 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HCl + 6 KI + 2 HNO_2 ⟶ 4 H_2O + 3 I_2 + 6 KCl + N_2

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

hydrogen chloride + potassium iodide + nitrous acid ⟶ water + iodine + potassium chloride + nitrogen
hydrogen chloride + potassium iodide + nitrous acid ⟶ water + iodine + potassium chloride + nitrogen

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + KI + HNO_2 ⟶ H_2O + I_2 + KCl + N_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: 6 HCl + 6 KI + 2 HNO_2 ⟶ 4 H_2O + 3 I_2 + 6 KCl + N_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 HCl | 6 | -6 KI | 6 | -6 HNO_2 | 2 | -2 H_2O | 4 | 4 I_2 | 3 | 3 KCl | 6 | 6 N_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) KI | 6 | -6 | ([KI])^(-6) HNO_2 | 2 | -2 | ([HNO2])^(-2) H_2O | 4 | 4 | ([H2O])^4 I_2 | 3 | 3 | ([I2])^3 KCl | 6 | 6 | ([KCl])^6 N_2 | 1 | 1 | [N2] 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 = ([HCl])^(-6) ([KI])^(-6) ([HNO2])^(-2) ([H2O])^4 ([I2])^3 ([KCl])^6 [N2] = (([H2O])^4 ([I2])^3 ([KCl])^6 [N2])/(([HCl])^6 ([KI])^6 ([HNO2])^2)
Construct the equilibrium constant, K, expression for: HCl + KI + HNO_2 ⟶ H_2O + I_2 + KCl + N_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: 6 HCl + 6 KI + 2 HNO_2 ⟶ 4 H_2O + 3 I_2 + 6 KCl + N_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 HCl | 6 | -6 KI | 6 | -6 HNO_2 | 2 | -2 H_2O | 4 | 4 I_2 | 3 | 3 KCl | 6 | 6 N_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) KI | 6 | -6 | ([KI])^(-6) HNO_2 | 2 | -2 | ([HNO2])^(-2) H_2O | 4 | 4 | ([H2O])^4 I_2 | 3 | 3 | ([I2])^3 KCl | 6 | 6 | ([KCl])^6 N_2 | 1 | 1 | [N2] 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 = ([HCl])^(-6) ([KI])^(-6) ([HNO2])^(-2) ([H2O])^4 ([I2])^3 ([KCl])^6 [N2] = (([H2O])^4 ([I2])^3 ([KCl])^6 [N2])/(([HCl])^6 ([KI])^6 ([HNO2])^2)

Rate of reaction

Construct the rate of reaction expression for: HCl + KI + HNO_2 ⟶ H_2O + I_2 + KCl + N_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: 6 HCl + 6 KI + 2 HNO_2 ⟶ 4 H_2O + 3 I_2 + 6 KCl + N_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 HCl | 6 | -6 KI | 6 | -6 HNO_2 | 2 | -2 H_2O | 4 | 4 I_2 | 3 | 3 KCl | 6 | 6 N_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 HCl | 6 | -6 | -1/6 (Δ[HCl])/(Δt) KI | 6 | -6 | -1/6 (Δ[KI])/(Δt) HNO_2 | 2 | -2 | -1/2 (Δ[HNO2])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) I_2 | 3 | 3 | 1/3 (Δ[I2])/(Δt) KCl | 6 | 6 | 1/6 (Δ[KCl])/(Δt) N_2 | 1 | 1 | (Δ[N2])/(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 = -1/6 (Δ[HCl])/(Δt) = -1/6 (Δ[KI])/(Δt) = -1/2 (Δ[HNO2])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/3 (Δ[I2])/(Δt) = 1/6 (Δ[KCl])/(Δt) = (Δ[N2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + KI + HNO_2 ⟶ H_2O + I_2 + KCl + N_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: 6 HCl + 6 KI + 2 HNO_2 ⟶ 4 H_2O + 3 I_2 + 6 KCl + N_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 HCl | 6 | -6 KI | 6 | -6 HNO_2 | 2 | -2 H_2O | 4 | 4 I_2 | 3 | 3 KCl | 6 | 6 N_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 HCl | 6 | -6 | -1/6 (Δ[HCl])/(Δt) KI | 6 | -6 | -1/6 (Δ[KI])/(Δt) HNO_2 | 2 | -2 | -1/2 (Δ[HNO2])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) I_2 | 3 | 3 | 1/3 (Δ[I2])/(Δt) KCl | 6 | 6 | 1/6 (Δ[KCl])/(Δt) N_2 | 1 | 1 | (Δ[N2])/(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 = -1/6 (Δ[HCl])/(Δt) = -1/6 (Δ[KI])/(Δt) = -1/2 (Δ[HNO2])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/3 (Δ[I2])/(Δt) = 1/6 (Δ[KCl])/(Δt) = (Δ[N2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | potassium iodide | nitrous acid | water | iodine | potassium chloride | nitrogen formula | HCl | KI | HNO_2 | H_2O | I_2 | KCl | N_2 Hill formula | ClH | IK | HNO_2 | H_2O | I_2 | ClK | N_2 name | hydrogen chloride | potassium iodide | nitrous acid | water | iodine | potassium chloride | nitrogen IUPAC name | hydrogen chloride | potassium iodide | nitrous acid | water | molecular iodine | potassium chloride | molecular nitrogen
| hydrogen chloride | potassium iodide | nitrous acid | water | iodine | potassium chloride | nitrogen formula | HCl | KI | HNO_2 | H_2O | I_2 | KCl | N_2 Hill formula | ClH | IK | HNO_2 | H_2O | I_2 | ClK | N_2 name | hydrogen chloride | potassium iodide | nitrous acid | water | iodine | potassium chloride | nitrogen IUPAC name | hydrogen chloride | potassium iodide | nitrous acid | water | molecular iodine | potassium chloride | molecular nitrogen

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