Search

NO2 = O2 + NO

Input interpretation

NO_2 (nitrogen dioxide) ⟶ O_2 (oxygen) + NO (nitric oxide)
NO_2 (nitrogen dioxide) ⟶ O_2 (oxygen) + NO (nitric oxide)

Balanced equation

Balance the chemical equation algebraically: NO_2 ⟶ O_2 + NO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NO_2 ⟶ c_2 O_2 + c_3 NO Set the number of atoms in the reactants equal to the number of atoms in the products for N and O: N: | c_1 = c_3 O: | 2 c_1 = 2 c_2 + c_3 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 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NO_2 ⟶ O_2 + 2 NO
Balance the chemical equation algebraically: NO_2 ⟶ O_2 + NO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NO_2 ⟶ c_2 O_2 + c_3 NO Set the number of atoms in the reactants equal to the number of atoms in the products for N and O: N: | c_1 = c_3 O: | 2 c_1 = 2 c_2 + c_3 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 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NO_2 ⟶ O_2 + 2 NO

Structures

⟶ +
⟶ +

Names

nitrogen dioxide ⟶ oxygen + nitric oxide
nitrogen dioxide ⟶ oxygen + nitric oxide

Reaction thermodynamics

Enthalpy

| nitrogen dioxide | oxygen | nitric oxide molecular enthalpy | 33.2 kJ/mol | 0 kJ/mol | 91.3 kJ/mol total enthalpy | 66.4 kJ/mol | 0 kJ/mol | 182.6 kJ/mol | H_initial = 66.4 kJ/mol | H_final = 182.6 kJ/mol | ΔH_rxn^0 | 182.6 kJ/mol - 66.4 kJ/mol = 116.2 kJ/mol (endothermic) | |
| nitrogen dioxide | oxygen | nitric oxide molecular enthalpy | 33.2 kJ/mol | 0 kJ/mol | 91.3 kJ/mol total enthalpy | 66.4 kJ/mol | 0 kJ/mol | 182.6 kJ/mol | H_initial = 66.4 kJ/mol | H_final = 182.6 kJ/mol | ΔH_rxn^0 | 182.6 kJ/mol - 66.4 kJ/mol = 116.2 kJ/mol (endothermic) | |

Gibbs free energy

| nitrogen dioxide | oxygen | nitric oxide molecular free energy | 51.3 kJ/mol | 231.7 kJ/mol | 87.6 kJ/mol total free energy | 102.6 kJ/mol | 231.7 kJ/mol | 175.2 kJ/mol | G_initial = 102.6 kJ/mol | G_final = 406.9 kJ/mol | ΔG_rxn^0 | 406.9 kJ/mol - 102.6 kJ/mol = 304.3 kJ/mol (endergonic) | |
| nitrogen dioxide | oxygen | nitric oxide molecular free energy | 51.3 kJ/mol | 231.7 kJ/mol | 87.6 kJ/mol total free energy | 102.6 kJ/mol | 231.7 kJ/mol | 175.2 kJ/mol | G_initial = 102.6 kJ/mol | G_final = 406.9 kJ/mol | ΔG_rxn^0 | 406.9 kJ/mol - 102.6 kJ/mol = 304.3 kJ/mol (endergonic) | |

Entropy

| nitrogen dioxide | oxygen | nitric oxide molecular entropy | 240 J/(mol K) | 205 J/(mol K) | 211 J/(mol K) total entropy | 480 J/(mol K) | 205 J/(mol K) | 422 J/(mol K) | S_initial = 480 J/(mol K) | S_final = 627 J/(mol K) | ΔS_rxn^0 | 627 J/(mol K) - 480 J/(mol K) = 147 J/(mol K) (endoentropic) | |
| nitrogen dioxide | oxygen | nitric oxide molecular entropy | 240 J/(mol K) | 205 J/(mol K) | 211 J/(mol K) total entropy | 480 J/(mol K) | 205 J/(mol K) | 422 J/(mol K) | S_initial = 480 J/(mol K) | S_final = 627 J/(mol K) | ΔS_rxn^0 | 627 J/(mol K) - 480 J/(mol K) = 147 J/(mol K) (endoentropic) | |

Equilibrium constant

K_c = ([O2] [NO]^2)/[NO2]^2
K_c = ([O2] [NO]^2)/[NO2]^2

Rate of reaction

rate = -1/2 (Δ[NO2])/(Δt) = (Δ[O2])/(Δt) = 1/2 (Δ[NO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
rate = -1/2 (Δ[NO2])/(Δt) = (Δ[O2])/(Δt) = 1/2 (Δ[NO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitrogen dioxide | oxygen | nitric oxide formula | NO_2 | O_2 | NO name | nitrogen dioxide | oxygen | nitric oxide IUPAC name | Nitrogen dioxide | molecular oxygen | nitric oxide
| nitrogen dioxide | oxygen | nitric oxide formula | NO_2 | O_2 | NO name | nitrogen dioxide | oxygen | nitric oxide IUPAC name | Nitrogen dioxide | molecular oxygen | nitric oxide

Substance properties

| nitrogen dioxide | oxygen | nitric oxide molar mass | 46.005 g/mol | 31.998 g/mol | 30.006 g/mol phase | gas (at STP) | gas (at STP) | gas (at STP) melting point | -11 °C | -218 °C | -163.6 °C boiling point | 21 °C | -183 °C | -151.7 °C density | 0.00188 g/cm^3 (at 25 °C) | 0.001429 g/cm^3 (at 0 °C) | 0.001226 g/cm^3 (at 25 °C) solubility in water | reacts | | surface tension | | 0.01347 N/m | dynamic viscosity | 4.02×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | 1.911×10^-5 Pa s (at 25 °C) odor | | odorless |
| nitrogen dioxide | oxygen | nitric oxide molar mass | 46.005 g/mol | 31.998 g/mol | 30.006 g/mol phase | gas (at STP) | gas (at STP) | gas (at STP) melting point | -11 °C | -218 °C | -163.6 °C boiling point | 21 °C | -183 °C | -151.7 °C density | 0.00188 g/cm^3 (at 25 °C) | 0.001429 g/cm^3 (at 0 °C) | 0.001226 g/cm^3 (at 25 °C) solubility in water | reacts | | surface tension | | 0.01347 N/m | dynamic viscosity | 4.02×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | 1.911×10^-5 Pa s (at 25 °C) odor | | odorless |

Units

Random Queries

chemical types of sodium bromate
ionic radius of gallium(III) cation
formula of krypton vs 1-chloro-2,2,2-trifluoroethane
atomic number of americium
IUPAC name of scandium chloride vs beryllium iodide
Hill formula of sodium metatungstate hydrate vs (ethylenediamine)palladium(II) chloride
vanadyl dichloride vs aluminum fluoride
aromatic atom count of Brønsted-Lowry acids
low pressure boiling point of aqueous compounds
name of copper(II) cation