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Cl2 + HNO3 = H2O + NO + HClO3

Input interpretation

Cl_2 chlorine + HNO_3 nitric acid ⟶ H_2O water + NO nitric oxide + HClO3
Cl_2 chlorine + HNO_3 nitric acid ⟶ H_2O water + NO nitric oxide + HClO3

Balanced equation

Balance the chemical equation algebraically: Cl_2 + HNO_3 ⟶ H_2O + NO + HClO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 HNO_3 ⟶ c_3 H_2O + c_4 NO + c_5 HClO3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N and O: Cl: | 2 c_1 = c_5 H: | c_2 = 2 c_3 + c_5 N: | c_2 = c_4 O: | 3 c_2 = c_3 + c_4 + 3 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3/2 c_2 = 5 c_3 = 1 c_4 = 5 c_5 = 3 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 10 c_3 = 2 c_4 = 10 c_5 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Cl_2 + 10 HNO_3 ⟶ 2 H_2O + 10 NO + 6 HClO3
Balance the chemical equation algebraically: Cl_2 + HNO_3 ⟶ H_2O + NO + HClO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 HNO_3 ⟶ c_3 H_2O + c_4 NO + c_5 HClO3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N and O: Cl: | 2 c_1 = c_5 H: | c_2 = 2 c_3 + c_5 N: | c_2 = c_4 O: | 3 c_2 = c_3 + c_4 + 3 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3/2 c_2 = 5 c_3 = 1 c_4 = 5 c_5 = 3 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 10 c_3 = 2 c_4 = 10 c_5 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Cl_2 + 10 HNO_3 ⟶ 2 H_2O + 10 NO + 6 HClO3

Structures

+ ⟶ + + HClO3
+ ⟶ + + HClO3

Names

chlorine + nitric acid ⟶ water + nitric oxide + HClO3
chlorine + nitric acid ⟶ water + nitric oxide + HClO3

Equilibrium constant

Construct the equilibrium constant, K, expression for: Cl_2 + HNO_3 ⟶ H_2O + NO + HClO3 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: 3 Cl_2 + 10 HNO_3 ⟶ 2 H_2O + 10 NO + 6 HClO3 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 Cl_2 | 3 | -3 HNO_3 | 10 | -10 H_2O | 2 | 2 NO | 10 | 10 HClO3 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 3 | -3 | ([Cl2])^(-3) HNO_3 | 10 | -10 | ([HNO3])^(-10) H_2O | 2 | 2 | ([H2O])^2 NO | 10 | 10 | ([NO])^10 HClO3 | 6 | 6 | ([HClO3])^6 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 = ([Cl2])^(-3) ([HNO3])^(-10) ([H2O])^2 ([NO])^10 ([HClO3])^6 = (([H2O])^2 ([NO])^10 ([HClO3])^6)/(([Cl2])^3 ([HNO3])^10)
Construct the equilibrium constant, K, expression for: Cl_2 + HNO_3 ⟶ H_2O + NO + HClO3 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: 3 Cl_2 + 10 HNO_3 ⟶ 2 H_2O + 10 NO + 6 HClO3 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 Cl_2 | 3 | -3 HNO_3 | 10 | -10 H_2O | 2 | 2 NO | 10 | 10 HClO3 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 3 | -3 | ([Cl2])^(-3) HNO_3 | 10 | -10 | ([HNO3])^(-10) H_2O | 2 | 2 | ([H2O])^2 NO | 10 | 10 | ([NO])^10 HClO3 | 6 | 6 | ([HClO3])^6 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 = ([Cl2])^(-3) ([HNO3])^(-10) ([H2O])^2 ([NO])^10 ([HClO3])^6 = (([H2O])^2 ([NO])^10 ([HClO3])^6)/(([Cl2])^3 ([HNO3])^10)

Rate of reaction

Construct the rate of reaction expression for: Cl_2 + HNO_3 ⟶ H_2O + NO + HClO3 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: 3 Cl_2 + 10 HNO_3 ⟶ 2 H_2O + 10 NO + 6 HClO3 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 Cl_2 | 3 | -3 HNO_3 | 10 | -10 H_2O | 2 | 2 NO | 10 | 10 HClO3 | 6 | 6 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 Cl_2 | 3 | -3 | -1/3 (Δ[Cl2])/(Δt) HNO_3 | 10 | -10 | -1/10 (Δ[HNO3])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NO | 10 | 10 | 1/10 (Δ[NO])/(Δt) HClO3 | 6 | 6 | 1/6 (Δ[HClO3])/(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 = -1/3 (Δ[Cl2])/(Δt) = -1/10 (Δ[HNO3])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/10 (Δ[NO])/(Δt) = 1/6 (Δ[HClO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Cl_2 + HNO_3 ⟶ H_2O + NO + HClO3 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: 3 Cl_2 + 10 HNO_3 ⟶ 2 H_2O + 10 NO + 6 HClO3 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 Cl_2 | 3 | -3 HNO_3 | 10 | -10 H_2O | 2 | 2 NO | 10 | 10 HClO3 | 6 | 6 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 Cl_2 | 3 | -3 | -1/3 (Δ[Cl2])/(Δt) HNO_3 | 10 | -10 | -1/10 (Δ[HNO3])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NO | 10 | 10 | 1/10 (Δ[NO])/(Δt) HClO3 | 6 | 6 | 1/6 (Δ[HClO3])/(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 = -1/3 (Δ[Cl2])/(Δt) = -1/10 (Δ[HNO3])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/10 (Δ[NO])/(Δt) = 1/6 (Δ[HClO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| chlorine | nitric acid | water | nitric oxide | HClO3 formula | Cl_2 | HNO_3 | H_2O | NO | HClO3 name | chlorine | nitric acid | water | nitric oxide | IUPAC name | molecular chlorine | nitric acid | water | nitric oxide |
| chlorine | nitric acid | water | nitric oxide | HClO3 formula | Cl_2 | HNO_3 | H_2O | NO | HClO3 name | chlorine | nitric acid | water | nitric oxide | IUPAC name | molecular chlorine | nitric acid | water | nitric oxide |

Substance properties

| chlorine | nitric acid | water | nitric oxide | HClO3 molar mass | 70.9 g/mol | 63.012 g/mol | 18.015 g/mol | 30.006 g/mol | 84.45 g/mol phase | gas (at STP) | liquid (at STP) | liquid (at STP) | gas (at STP) | melting point | -101 °C | -41.6 °C | 0 °C | -163.6 °C | boiling point | -34 °C | 83 °C | 99.9839 °C | -151.7 °C | density | 0.003214 g/cm^3 (at 0 °C) | 1.5129 g/cm^3 | 1 g/cm^3 | 0.001226 g/cm^3 (at 25 °C) | solubility in water | | miscible | | | surface tension | | | 0.0728 N/m | | dynamic viscosity | | 7.6×10^-4 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | 1.911×10^-5 Pa s (at 25 °C) | odor | | | odorless | |
| chlorine | nitric acid | water | nitric oxide | HClO3 molar mass | 70.9 g/mol | 63.012 g/mol | 18.015 g/mol | 30.006 g/mol | 84.45 g/mol phase | gas (at STP) | liquid (at STP) | liquid (at STP) | gas (at STP) | melting point | -101 °C | -41.6 °C | 0 °C | -163.6 °C | boiling point | -34 °C | 83 °C | 99.9839 °C | -151.7 °C | density | 0.003214 g/cm^3 (at 0 °C) | 1.5129 g/cm^3 | 1 g/cm^3 | 0.001226 g/cm^3 (at 25 °C) | solubility in water | | miscible | | | surface tension | | | 0.0728 N/m | | dynamic viscosity | | 7.6×10^-4 Pa s (at 25 °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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