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HNO3 + HI = H2O + NO + HIO3

Input interpretation

HNO_3 nitric acid + HI hydrogen iodide ⟶ H_2O water + NO nitric oxide + HIO_3 iodic acid
HNO_3 nitric acid + HI hydrogen iodide ⟶ H_2O water + NO nitric oxide + HIO_3 iodic acid

Balanced equation

Balance the chemical equation algebraically: HNO_3 + HI ⟶ H_2O + NO + HIO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 HI ⟶ c_3 H_2O + c_4 NO + c_5 HIO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and I: H: | c_1 + c_2 = 2 c_3 + c_5 N: | c_1 = c_4 O: | 3 c_1 = c_3 + c_4 + 3 c_5 I: | c_2 = c_5 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HNO_3 + HI ⟶ H_2O + 2 NO + HIO_3
Balance the chemical equation algebraically: HNO_3 + HI ⟶ H_2O + NO + HIO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 HI ⟶ c_3 H_2O + c_4 NO + c_5 HIO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and I: H: | c_1 + c_2 = 2 c_3 + c_5 N: | c_1 = c_4 O: | 3 c_1 = c_3 + c_4 + 3 c_5 I: | c_2 = c_5 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HNO_3 + HI ⟶ H_2O + 2 NO + HIO_3

Structures

+ ⟶ + +
+ ⟶ + +

Names

nitric acid + hydrogen iodide ⟶ water + nitric oxide + iodic acid
nitric acid + hydrogen iodide ⟶ water + nitric oxide + iodic acid

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + HI ⟶ H_2O + NO + HIO_3 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 HNO_3 + HI ⟶ H_2O + 2 NO + HIO_3 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 HNO_3 | 2 | -2 HI | 1 | -1 H_2O | 1 | 1 NO | 2 | 2 HIO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 2 | -2 | ([HNO3])^(-2) HI | 1 | -1 | ([HI])^(-1) H_2O | 1 | 1 | [H2O] NO | 2 | 2 | ([NO])^2 HIO_3 | 1 | 1 | [HIO3] 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 = ([HNO3])^(-2) ([HI])^(-1) [H2O] ([NO])^2 [HIO3] = ([H2O] ([NO])^2 [HIO3])/(([HNO3])^2 [HI])
Construct the equilibrium constant, K, expression for: HNO_3 + HI ⟶ H_2O + NO + HIO_3 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 HNO_3 + HI ⟶ H_2O + 2 NO + HIO_3 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 HNO_3 | 2 | -2 HI | 1 | -1 H_2O | 1 | 1 NO | 2 | 2 HIO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 2 | -2 | ([HNO3])^(-2) HI | 1 | -1 | ([HI])^(-1) H_2O | 1 | 1 | [H2O] NO | 2 | 2 | ([NO])^2 HIO_3 | 1 | 1 | [HIO3] 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 = ([HNO3])^(-2) ([HI])^(-1) [H2O] ([NO])^2 [HIO3] = ([H2O] ([NO])^2 [HIO3])/(([HNO3])^2 [HI])

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + HI ⟶ H_2O + NO + HIO_3 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 HNO_3 + HI ⟶ H_2O + 2 NO + HIO_3 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 HNO_3 | 2 | -2 HI | 1 | -1 H_2O | 1 | 1 NO | 2 | 2 HIO_3 | 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 HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) HI | 1 | -1 | -(Δ[HI])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) HIO_3 | 1 | 1 | (Δ[HIO3])/(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[HNO3])/(Δt) = -(Δ[HI])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[NO])/(Δt) = (Δ[HIO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_3 + HI ⟶ H_2O + NO + HIO_3 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 HNO_3 + HI ⟶ H_2O + 2 NO + HIO_3 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 HNO_3 | 2 | -2 HI | 1 | -1 H_2O | 1 | 1 NO | 2 | 2 HIO_3 | 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 HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) HI | 1 | -1 | -(Δ[HI])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) HIO_3 | 1 | 1 | (Δ[HIO3])/(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[HNO3])/(Δt) = -(Δ[HI])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[NO])/(Δt) = (Δ[HIO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | hydrogen iodide | water | nitric oxide | iodic acid formula | HNO_3 | HI | H_2O | NO | HIO_3 name | nitric acid | hydrogen iodide | water | nitric oxide | iodic acid
| nitric acid | hydrogen iodide | water | nitric oxide | iodic acid formula | HNO_3 | HI | H_2O | NO | HIO_3 name | nitric acid | hydrogen iodide | water | nitric oxide | iodic acid

Substance properties

| nitric acid | hydrogen iodide | water | nitric oxide | iodic acid molar mass | 63.012 g/mol | 127.912 g/mol | 18.015 g/mol | 30.006 g/mol | 175.91 g/mol phase | liquid (at STP) | gas (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -41.6 °C | -50.76 °C | 0 °C | -163.6 °C | 110 °C boiling point | 83 °C | -35.55 °C | 99.9839 °C | -151.7 °C | density | 1.5129 g/cm^3 | 0.005228 g/cm^3 (at 25 °C) | 1 g/cm^3 | 0.001226 g/cm^3 (at 25 °C) | 4.629 g/cm^3 solubility in water | miscible | very soluble | | | very soluble surface tension | | | 0.0728 N/m | | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | 0.001321 Pa s (at -39 °C) | 8.9×10^-4 Pa s (at 25 °C) | 1.911×10^-5 Pa s (at 25 °C) | odor | | | odorless | |
| nitric acid | hydrogen iodide | water | nitric oxide | iodic acid molar mass | 63.012 g/mol | 127.912 g/mol | 18.015 g/mol | 30.006 g/mol | 175.91 g/mol phase | liquid (at STP) | gas (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -41.6 °C | -50.76 °C | 0 °C | -163.6 °C | 110 °C boiling point | 83 °C | -35.55 °C | 99.9839 °C | -151.7 °C | density | 1.5129 g/cm^3 | 0.005228 g/cm^3 (at 25 °C) | 1 g/cm^3 | 0.001226 g/cm^3 (at 25 °C) | 4.629 g/cm^3 solubility in water | miscible | very soluble | | | very soluble surface tension | | | 0.0728 N/m | | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | 0.001321 Pa s (at -39 °C) | 8.9×10^-4 Pa s (at 25 °C) | 1.911×10^-5 Pa s (at 25 °C) | odor | | | odorless | |

Units

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