NaNO2 = NO + NO2 + Na2O

NaNO_2 sodium nitrite ⟶ NO nitric oxide + NO_2 nitrogen dioxide + Na_2O sodium oxide

Balance the chemical equation algebraically: NaNO_2 ⟶ NO + NO_2 + Na_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaNO_2 ⟶ c_2 NO + c_3 NO_2 + c_4 Na_2O Set the number of atoms in the reactants equal to the number of atoms in the products for N, Na and O: N: | c_1 = c_2 + c_3 Na: | c_1 = 2 c_4 O: | 2 c_1 = c_2 + 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NaNO_2 ⟶ NO + NO_2 + Na_2O

⟶ + +

sodium nitrite ⟶ nitric oxide + nitrogen dioxide + sodium oxide

Construct the equilibrium constant, K, expression for: NaNO_2 ⟶ NO + NO_2 + Na_2O 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 NaNO_2 ⟶ NO + NO_2 + Na_2O 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 NaNO_2 | 2 | -2 NO | 1 | 1 NO_2 | 1 | 1 Na_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaNO_2 | 2 | -2 | ([NaNO2])^(-2) NO | 1 | 1 | [NO] NO_2 | 1 | 1 | [NO2] Na_2O | 1 | 1 | [Na2O] 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 = ([NaNO2])^(-2) [NO] [NO2] [Na2O] = ([NO] [NO2] [Na2O])/([NaNO2])^2

Construct the rate of reaction expression for: NaNO_2 ⟶ NO + NO_2 + Na_2O 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 NaNO_2 ⟶ NO + NO_2 + Na_2O 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 NaNO_2 | 2 | -2 NO | 1 | 1 NO_2 | 1 | 1 Na_2O | 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 NaNO_2 | 2 | -2 | -1/2 (Δ[NaNO2])/(Δt) NO | 1 | 1 | (Δ[NO])/(Δt) NO_2 | 1 | 1 | (Δ[NO2])/(Δt) Na_2O | 1 | 1 | (Δ[Na2O])/(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[NaNO2])/(Δt) = (Δ[NO])/(Δt) = (Δ[NO2])/(Δt) = (Δ[Na2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sodium nitrite | nitric oxide | nitrogen dioxide | sodium oxide formula | NaNO_2 | NO | NO_2 | Na_2O Hill formula | NNaO_2 | NO | NO_2 | Na_2O name | sodium nitrite | nitric oxide | nitrogen dioxide | sodium oxide IUPAC name | sodium nitrite | nitric oxide | Nitrogen dioxide | disodium oxygen(-2) anion

| sodium nitrite | nitric oxide | nitrogen dioxide | sodium oxide molar mass | 68.995 g/mol | 30.006 g/mol | 46.005 g/mol | 61.979 g/mol phase | solid (at STP) | gas (at STP) | gas (at STP) | melting point | 271 °C | -163.6 °C | -11 °C | boiling point | | -151.7 °C | 21 °C | density | 2.168 g/cm^3 | 0.001226 g/cm^3 (at 25 °C) | 0.00188 g/cm^3 (at 25 °C) | 2.27 g/cm^3 solubility in water | | | reacts | dynamic viscosity | | 1.911×10^-5 Pa s (at 25 °C) | 4.02×10^-4 Pa s (at 25 °C) |