Search

HNO3 + Na = H2O + N2 + NaNO3

Input interpretation

HNO_3 nitric acid + Na sodium ⟶ H_2O water + N_2 nitrogen + NaNO_3 sodium nitrate
HNO_3 nitric acid + Na sodium ⟶ H_2O water + N_2 nitrogen + NaNO_3 sodium nitrate

Balanced equation

Balance the chemical equation algebraically: HNO_3 + Na ⟶ H_2O + N_2 + NaNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Na ⟶ c_3 H_2O + c_4 N_2 + c_5 NaNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Na: H: | c_1 = 2 c_3 N: | c_1 = 2 c_4 + c_5 O: | 3 c_1 = c_3 + 3 c_5 Na: | 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 12 c_2 = 10 c_3 = 6 c_4 = 1 c_5 = 10 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 12 HNO_3 + 10 Na ⟶ 6 H_2O + N_2 + 10 NaNO_3
Balance the chemical equation algebraically: HNO_3 + Na ⟶ H_2O + N_2 + NaNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Na ⟶ c_3 H_2O + c_4 N_2 + c_5 NaNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Na: H: | c_1 = 2 c_3 N: | c_1 = 2 c_4 + c_5 O: | 3 c_1 = c_3 + 3 c_5 Na: | 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 12 c_2 = 10 c_3 = 6 c_4 = 1 c_5 = 10 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 12 HNO_3 + 10 Na ⟶ 6 H_2O + N_2 + 10 NaNO_3

Structures

+ ⟶ + +
+ ⟶ + +

Names

nitric acid + sodium ⟶ water + nitrogen + sodium nitrate
nitric acid + sodium ⟶ water + nitrogen + sodium nitrate

Reaction thermodynamics

Entropy

| nitric acid | sodium | water | nitrogen | sodium nitrate molecular entropy | 156 J/(mol K) | 51 J/(mol K) | 69.91 J/(mol K) | 192 J/(mol K) | 116 J/(mol K) total entropy | 1872 J/(mol K) | 510 J/(mol K) | 419.5 J/(mol K) | 192 J/(mol K) | 1160 J/(mol K) | S_initial = 2382 J/(mol K) | | S_final = 1771 J/(mol K) | | ΔS_rxn^0 | 1771 J/(mol K) - 2382 J/(mol K) = -610.5 J/(mol K) (exoentropic) | | | |
| nitric acid | sodium | water | nitrogen | sodium nitrate molecular entropy | 156 J/(mol K) | 51 J/(mol K) | 69.91 J/(mol K) | 192 J/(mol K) | 116 J/(mol K) total entropy | 1872 J/(mol K) | 510 J/(mol K) | 419.5 J/(mol K) | 192 J/(mol K) | 1160 J/(mol K) | S_initial = 2382 J/(mol K) | | S_final = 1771 J/(mol K) | | ΔS_rxn^0 | 1771 J/(mol K) - 2382 J/(mol K) = -610.5 J/(mol K) (exoentropic) | | | |

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + Na ⟶ H_2O + N_2 + NaNO_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: 12 HNO_3 + 10 Na ⟶ 6 H_2O + N_2 + 10 NaNO_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 | 12 | -12 Na | 10 | -10 H_2O | 6 | 6 N_2 | 1 | 1 NaNO_3 | 10 | 10 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 12 | -12 | ([HNO3])^(-12) Na | 10 | -10 | ([Na])^(-10) H_2O | 6 | 6 | ([H2O])^6 N_2 | 1 | 1 | [N2] NaNO_3 | 10 | 10 | ([NaNO3])^10 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])^(-12) ([Na])^(-10) ([H2O])^6 [N2] ([NaNO3])^10 = (([H2O])^6 [N2] ([NaNO3])^10)/(([HNO3])^12 ([Na])^10)
Construct the equilibrium constant, K, expression for: HNO_3 + Na ⟶ H_2O + N_2 + NaNO_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: 12 HNO_3 + 10 Na ⟶ 6 H_2O + N_2 + 10 NaNO_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 | 12 | -12 Na | 10 | -10 H_2O | 6 | 6 N_2 | 1 | 1 NaNO_3 | 10 | 10 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 12 | -12 | ([HNO3])^(-12) Na | 10 | -10 | ([Na])^(-10) H_2O | 6 | 6 | ([H2O])^6 N_2 | 1 | 1 | [N2] NaNO_3 | 10 | 10 | ([NaNO3])^10 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])^(-12) ([Na])^(-10) ([H2O])^6 [N2] ([NaNO3])^10 = (([H2O])^6 [N2] ([NaNO3])^10)/(([HNO3])^12 ([Na])^10)

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + Na ⟶ H_2O + N_2 + NaNO_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: 12 HNO_3 + 10 Na ⟶ 6 H_2O + N_2 + 10 NaNO_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 | 12 | -12 Na | 10 | -10 H_2O | 6 | 6 N_2 | 1 | 1 NaNO_3 | 10 | 10 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 | 12 | -12 | -1/12 (Δ[HNO3])/(Δt) Na | 10 | -10 | -1/10 (Δ[Na])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) N_2 | 1 | 1 | (Δ[N2])/(Δt) NaNO_3 | 10 | 10 | 1/10 (Δ[NaNO3])/(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 = -1/12 (Δ[HNO3])/(Δt) = -1/10 (Δ[Na])/(Δt) = 1/6 (Δ[H2O])/(Δt) = (Δ[N2])/(Δt) = 1/10 (Δ[NaNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_3 + Na ⟶ H_2O + N_2 + NaNO_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: 12 HNO_3 + 10 Na ⟶ 6 H_2O + N_2 + 10 NaNO_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 | 12 | -12 Na | 10 | -10 H_2O | 6 | 6 N_2 | 1 | 1 NaNO_3 | 10 | 10 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 | 12 | -12 | -1/12 (Δ[HNO3])/(Δt) Na | 10 | -10 | -1/10 (Δ[Na])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) N_2 | 1 | 1 | (Δ[N2])/(Δt) NaNO_3 | 10 | 10 | 1/10 (Δ[NaNO3])/(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 = -1/12 (Δ[HNO3])/(Δt) = -1/10 (Δ[Na])/(Δt) = 1/6 (Δ[H2O])/(Δt) = (Δ[N2])/(Δt) = 1/10 (Δ[NaNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | sodium | water | nitrogen | sodium nitrate formula | HNO_3 | Na | H_2O | N_2 | NaNO_3 Hill formula | HNO_3 | Na | H_2O | N_2 | NNaO_3 name | nitric acid | sodium | water | nitrogen | sodium nitrate IUPAC name | nitric acid | sodium | water | molecular nitrogen | sodium nitrate
| nitric acid | sodium | water | nitrogen | sodium nitrate formula | HNO_3 | Na | H_2O | N_2 | NaNO_3 Hill formula | HNO_3 | Na | H_2O | N_2 | NNaO_3 name | nitric acid | sodium | water | nitrogen | sodium nitrate IUPAC name | nitric acid | sodium | water | molecular nitrogen | sodium nitrate

Random Queries

chemical types of 2-bromo-6-chloro-4-fluoroaniline
density of manganese dioxide vs potassium fluoride dihydrate
name of potassium chloride vs rubidium nitrate
ion class of iodide anion vs fluoride anion
molar mass of chromium selenide vs ammonium-d 8sulfate
melting point of sodium nitrate vs sodium
molar mass of tetrachloroaurate(III) anion vs dichloroaurate(I) anion
neutron mass absorption of f-block elements
Al + HClO3 = H2O + AlCl3 + Al(ClO3)3
C + Fe3O4 = Fe + CO