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NO + NO2 + Ba(OH)2 = H2O + Ba(NO2)2

Input interpretation

NO nitric oxide + NO_2 nitrogen dioxide + Ba(OH)_2 barium hydroxide ⟶ H_2O water + BaN_2O_4 barium nitrite
NO nitric oxide + NO_2 nitrogen dioxide + Ba(OH)_2 barium hydroxide ⟶ H_2O water + BaN_2O_4 barium nitrite

Balanced equation

Balance the chemical equation algebraically: NO + NO_2 + Ba(OH)_2 ⟶ H_2O + BaN_2O_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NO + c_2 NO_2 + c_3 Ba(OH)_2 ⟶ c_4 H_2O + c_5 BaN_2O_4 Set the number of atoms in the reactants equal to the number of atoms in the products for N, O, Ba and H: N: | c_1 + c_2 = 2 c_5 O: | c_1 + 2 c_2 + 2 c_3 = c_4 + 4 c_5 Ba: | c_3 = c_5 H: | 2 c_3 = 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NO + NO_2 + Ba(OH)_2 ⟶ H_2O + BaN_2O_4
Balance the chemical equation algebraically: NO + NO_2 + Ba(OH)_2 ⟶ H_2O + BaN_2O_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NO + c_2 NO_2 + c_3 Ba(OH)_2 ⟶ c_4 H_2O + c_5 BaN_2O_4 Set the number of atoms in the reactants equal to the number of atoms in the products for N, O, Ba and H: N: | c_1 + c_2 = 2 c_5 O: | c_1 + 2 c_2 + 2 c_3 = c_4 + 4 c_5 Ba: | c_3 = c_5 H: | 2 c_3 = 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NO + NO_2 + Ba(OH)_2 ⟶ H_2O + BaN_2O_4

Structures

+ + ⟶ +
+ + ⟶ +

Names

nitric oxide + nitrogen dioxide + barium hydroxide ⟶ water + barium nitrite
nitric oxide + nitrogen dioxide + barium hydroxide ⟶ water + barium nitrite

Reaction thermodynamics

Enthalpy

| nitric oxide | nitrogen dioxide | barium hydroxide | water | barium nitrite molecular enthalpy | 91.3 kJ/mol | 33.2 kJ/mol | -944.7 kJ/mol | -285.8 kJ/mol | -768.2 kJ/mol total enthalpy | 91.3 kJ/mol | 33.2 kJ/mol | -944.7 kJ/mol | -285.8 kJ/mol | -768.2 kJ/mol | H_initial = -820.2 kJ/mol | | | H_final = -1054 kJ/mol | ΔH_rxn^0 | -1054 kJ/mol - -820.2 kJ/mol = -233.8 kJ/mol (exothermic) | | | |
| nitric oxide | nitrogen dioxide | barium hydroxide | water | barium nitrite molecular enthalpy | 91.3 kJ/mol | 33.2 kJ/mol | -944.7 kJ/mol | -285.8 kJ/mol | -768.2 kJ/mol total enthalpy | 91.3 kJ/mol | 33.2 kJ/mol | -944.7 kJ/mol | -285.8 kJ/mol | -768.2 kJ/mol | H_initial = -820.2 kJ/mol | | | H_final = -1054 kJ/mol | ΔH_rxn^0 | -1054 kJ/mol - -820.2 kJ/mol = -233.8 kJ/mol (exothermic) | | | |

Equilibrium constant

Construct the equilibrium constant, K, expression for: NO + NO_2 + Ba(OH)_2 ⟶ H_2O + BaN_2O_4 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: NO + NO_2 + Ba(OH)_2 ⟶ H_2O + BaN_2O_4 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 NO | 1 | -1 NO_2 | 1 | -1 Ba(OH)_2 | 1 | -1 H_2O | 1 | 1 BaN_2O_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NO | 1 | -1 | ([NO])^(-1) NO_2 | 1 | -1 | ([NO2])^(-1) Ba(OH)_2 | 1 | -1 | ([Ba(OH)2])^(-1) H_2O | 1 | 1 | [H2O] BaN_2O_4 | 1 | 1 | [BaN2O4] 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 = ([NO])^(-1) ([NO2])^(-1) ([Ba(OH)2])^(-1) [H2O] [BaN2O4] = ([H2O] [BaN2O4])/([NO] [NO2] [Ba(OH)2])
Construct the equilibrium constant, K, expression for: NO + NO_2 + Ba(OH)_2 ⟶ H_2O + BaN_2O_4 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: NO + NO_2 + Ba(OH)_2 ⟶ H_2O + BaN_2O_4 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 NO | 1 | -1 NO_2 | 1 | -1 Ba(OH)_2 | 1 | -1 H_2O | 1 | 1 BaN_2O_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NO | 1 | -1 | ([NO])^(-1) NO_2 | 1 | -1 | ([NO2])^(-1) Ba(OH)_2 | 1 | -1 | ([Ba(OH)2])^(-1) H_2O | 1 | 1 | [H2O] BaN_2O_4 | 1 | 1 | [BaN2O4] 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 = ([NO])^(-1) ([NO2])^(-1) ([Ba(OH)2])^(-1) [H2O] [BaN2O4] = ([H2O] [BaN2O4])/([NO] [NO2] [Ba(OH)2])

Rate of reaction

Construct the rate of reaction expression for: NO + NO_2 + Ba(OH)_2 ⟶ H_2O + BaN_2O_4 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: NO + NO_2 + Ba(OH)_2 ⟶ H_2O + BaN_2O_4 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 NO | 1 | -1 NO_2 | 1 | -1 Ba(OH)_2 | 1 | -1 H_2O | 1 | 1 BaN_2O_4 | 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 NO | 1 | -1 | -(Δ[NO])/(Δt) NO_2 | 1 | -1 | -(Δ[NO2])/(Δt) Ba(OH)_2 | 1 | -1 | -(Δ[Ba(OH)2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) BaN_2O_4 | 1 | 1 | (Δ[BaN2O4])/(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 = -(Δ[NO])/(Δt) = -(Δ[NO2])/(Δt) = -(Δ[Ba(OH)2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[BaN2O4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NO + NO_2 + Ba(OH)_2 ⟶ H_2O + BaN_2O_4 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: NO + NO_2 + Ba(OH)_2 ⟶ H_2O + BaN_2O_4 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 NO | 1 | -1 NO_2 | 1 | -1 Ba(OH)_2 | 1 | -1 H_2O | 1 | 1 BaN_2O_4 | 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 NO | 1 | -1 | -(Δ[NO])/(Δt) NO_2 | 1 | -1 | -(Δ[NO2])/(Δt) Ba(OH)_2 | 1 | -1 | -(Δ[Ba(OH)2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) BaN_2O_4 | 1 | 1 | (Δ[BaN2O4])/(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 = -(Δ[NO])/(Δt) = -(Δ[NO2])/(Δt) = -(Δ[Ba(OH)2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[BaN2O4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric oxide | nitrogen dioxide | barium hydroxide | water | barium nitrite formula | NO | NO_2 | Ba(OH)_2 | H_2O | BaN_2O_4 Hill formula | NO | NO_2 | BaH_2O_2 | H_2O | BaN_2O_4 name | nitric oxide | nitrogen dioxide | barium hydroxide | water | barium nitrite IUPAC name | nitric oxide | Nitrogen dioxide | barium(+2) cation dihydroxide | water | barium(+2) cation dinitrite
| nitric oxide | nitrogen dioxide | barium hydroxide | water | barium nitrite formula | NO | NO_2 | Ba(OH)_2 | H_2O | BaN_2O_4 Hill formula | NO | NO_2 | BaH_2O_2 | H_2O | BaN_2O_4 name | nitric oxide | nitrogen dioxide | barium hydroxide | water | barium nitrite IUPAC name | nitric oxide | Nitrogen dioxide | barium(+2) cation dihydroxide | water | barium(+2) cation dinitrite

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