Search

HCl + HNO3 = H2O + Cl2 + NOCl

Input interpretation

HCl (hydrogen chloride) + HNO_3 (nitric acid) ⟶ H_2O (water) + Cl_2 (chlorine) + ClH_2NO
HCl (hydrogen chloride) + HNO_3 (nitric acid) ⟶ H_2O (water) + Cl_2 (chlorine) + ClH_2NO

Balanced equation

Balance the chemical equation algebraically: HCl + HNO_3 ⟶ H_2O + Cl_2 + ClH_2NO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 ⟶ c_3 H_2O + c_4 Cl_2 + c_5 ClH_2NO Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N and O: Cl: | c_1 = 2 c_4 + c_5 H: | c_1 + c_2 = 2 c_3 + 2 c_5 N: | c_2 = c_5 O: | 3 c_2 = c_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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 5 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 5 HCl + HNO_3 ⟶ 2 H_2O + 2 Cl_2 + ClH_2NO
Balance the chemical equation algebraically: HCl + HNO_3 ⟶ H_2O + Cl_2 + ClH_2NO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 ⟶ c_3 H_2O + c_4 Cl_2 + c_5 ClH_2NO Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N and O: Cl: | c_1 = 2 c_4 + c_5 H: | c_1 + c_2 = 2 c_3 + 2 c_5 N: | c_2 = c_5 O: | 3 c_2 = c_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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 5 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 5 HCl + HNO_3 ⟶ 2 H_2O + 2 Cl_2 + ClH_2NO

Structures

+ ⟶ + +
+ ⟶ + +

Names

hydrogen chloride + nitric acid ⟶ water + chlorine + ClH_2NO
hydrogen chloride + nitric acid ⟶ water + chlorine + ClH_2NO

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + HNO_3 ⟶ H_2O + Cl_2 + ClH_2NO 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: 5 HCl + HNO_3 ⟶ 2 H_2O + 2 Cl_2 + ClH_2NO 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 | 5 | -5 HNO_3 | 1 | -1 H_2O | 2 | 2 Cl_2 | 2 | 2 ClH_2NO | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 5 | -5 | ([HCl])^(-5) HNO_3 | 1 | -1 | ([HNO3])^(-1) H_2O | 2 | 2 | ([H2O])^2 Cl_2 | 2 | 2 | ([Cl2])^2 ClH_2NO | 1 | 1 | [ClH2NO] 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])^(-5) ([HNO3])^(-1) ([H2O])^2 ([Cl2])^2 [ClH2NO] = (([H2O])^2 ([Cl2])^2 [ClH2NO])/(([HCl])^5 [HNO3])
Construct the equilibrium constant, K, expression for: HCl + HNO_3 ⟶ H_2O + Cl_2 + ClH_2NO 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: 5 HCl + HNO_3 ⟶ 2 H_2O + 2 Cl_2 + ClH_2NO 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 | 5 | -5 HNO_3 | 1 | -1 H_2O | 2 | 2 Cl_2 | 2 | 2 ClH_2NO | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 5 | -5 | ([HCl])^(-5) HNO_3 | 1 | -1 | ([HNO3])^(-1) H_2O | 2 | 2 | ([H2O])^2 Cl_2 | 2 | 2 | ([Cl2])^2 ClH_2NO | 1 | 1 | [ClH2NO] 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])^(-5) ([HNO3])^(-1) ([H2O])^2 ([Cl2])^2 [ClH2NO] = (([H2O])^2 ([Cl2])^2 [ClH2NO])/(([HCl])^5 [HNO3])

Rate of reaction

Construct the rate of reaction expression for: HCl + HNO_3 ⟶ H_2O + Cl_2 + ClH_2NO 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: 5 HCl + HNO_3 ⟶ 2 H_2O + 2 Cl_2 + ClH_2NO 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 | 5 | -5 HNO_3 | 1 | -1 H_2O | 2 | 2 Cl_2 | 2 | 2 ClH_2NO | 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 | 5 | -5 | -1/5 (Δ[HCl])/(Δt) HNO_3 | 1 | -1 | -(Δ[HNO3])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) Cl_2 | 2 | 2 | 1/2 (Δ[Cl2])/(Δt) ClH_2NO | 1 | 1 | (Δ[ClH2NO])/(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 = -1/5 (Δ[HCl])/(Δt) = -(Δ[HNO3])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[Cl2])/(Δt) = (Δ[ClH2NO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + HNO_3 ⟶ H_2O + Cl_2 + ClH_2NO 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: 5 HCl + HNO_3 ⟶ 2 H_2O + 2 Cl_2 + ClH_2NO 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 | 5 | -5 HNO_3 | 1 | -1 H_2O | 2 | 2 Cl_2 | 2 | 2 ClH_2NO | 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 | 5 | -5 | -1/5 (Δ[HCl])/(Δt) HNO_3 | 1 | -1 | -(Δ[HNO3])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) Cl_2 | 2 | 2 | 1/2 (Δ[Cl2])/(Δt) ClH_2NO | 1 | 1 | (Δ[ClH2NO])/(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 = -1/5 (Δ[HCl])/(Δt) = -(Δ[HNO3])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[Cl2])/(Δt) = (Δ[ClH2NO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | nitric acid | water | chlorine | SMILES | NOCl formula | HCl | HNO_3 | H_2O | Cl_2 | ClH_2NO Hill formula | ClH | HNO_3 | H_2O | Cl_2 | ClH_2NO name | hydrogen chloride | nitric acid | water | chlorine | IUPAC name | hydrogen chloride | nitric acid | water | molecular chlorine |
| hydrogen chloride | nitric acid | water | chlorine | SMILES | NOCl formula | HCl | HNO_3 | H_2O | Cl_2 | ClH_2NO Hill formula | ClH | HNO_3 | H_2O | Cl_2 | ClH_2NO name | hydrogen chloride | nitric acid | water | chlorine | IUPAC name | hydrogen chloride | nitric acid | water | molecular chlorine |

Substance properties

| hydrogen chloride | nitric acid | water | chlorine | SMILES | NOCl molar mass | 36.46 g/mol | 63.012 g/mol | 18.015 g/mol | 70.9 g/mol | 67.47 g/mol phase | gas (at STP) | liquid (at STP) | liquid (at STP) | gas (at STP) | melting point | -114.17 °C | -41.6 °C | 0 °C | -101 °C | -47.98 °C boiling point | -85 °C | 83 °C | 99.9839 °C | -34 °C | 58.63 °C density | 0.00149 g/cm^3 (at 25 °C) | 1.5129 g/cm^3 | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | solubility in water | miscible | 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) | | odor | | | odorless | |
| hydrogen chloride | nitric acid | water | chlorine | SMILES | NOCl molar mass | 36.46 g/mol | 63.012 g/mol | 18.015 g/mol | 70.9 g/mol | 67.47 g/mol phase | gas (at STP) | liquid (at STP) | liquid (at STP) | gas (at STP) | melting point | -114.17 °C | -41.6 °C | 0 °C | -101 °C | -47.98 °C boiling point | -85 °C | 83 °C | 99.9839 °C | -34 °C | 58.63 °C density | 0.00149 g/cm^3 (at 25 °C) | 1.5129 g/cm^3 | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | solubility in water | miscible | 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) | | odor | | | odorless | |

Units

Random Queries

ionic radius of manganese(IV) cation
density of calcium nitrate vs germanium telluride
molar mass of (3-chloropropyl)triethoxysilane
net ionic charge of cobalt ions
lead(IV) cation vs carbonate anion vs hydrogen carbonate anion
molar mass of sulfate anion vs chromium(III) cation
ion electron configuration of iodine(I) cation vs bromine(IV) cation
blocks of precious metals
CAS number of 4-bromo-2-fluorophenylzinc iodide
atomic mass of livermorium vs darmstadtium