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HNO3 + Ag = H2O + NO + NO2 + Ag(NO3)

Input interpretation

HNO_3 nitric acid + Ag silver ⟶ H_2O water + NO nitric oxide + NO_2 nitrogen dioxide + AgNO_3 silver nitrate
HNO_3 nitric acid + Ag silver ⟶ H_2O water + NO nitric oxide + NO_2 nitrogen dioxide + AgNO_3 silver nitrate

Balanced equation

Balance the chemical equation algebraically: HNO_3 + Ag ⟶ H_2O + NO + NO_2 + AgNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Ag ⟶ c_3 H_2O + c_4 NO + c_5 NO_2 + c_6 AgNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Ag: H: | c_1 = 2 c_3 N: | c_1 = c_4 + c_5 + c_6 O: | 3 c_1 = c_3 + c_4 + 2 c_5 + 3 c_6 Ag: | c_2 = c_6 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_2 = c_1/2 + 1 c_3 = c_1/2 c_4 = 1 c_5 = c_1/2 - 2 c_6 = c_1/2 + 1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 10 and solve for the remaining coefficients: c_1 = 10 c_2 = 6 c_3 = 5 c_4 = 1 c_5 = 3 c_6 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 HNO_3 + 6 Ag ⟶ 5 H_2O + NO + 3 NO_2 + 6 AgNO_3
Balance the chemical equation algebraically: HNO_3 + Ag ⟶ H_2O + NO + NO_2 + AgNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Ag ⟶ c_3 H_2O + c_4 NO + c_5 NO_2 + c_6 AgNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Ag: H: | c_1 = 2 c_3 N: | c_1 = c_4 + c_5 + c_6 O: | 3 c_1 = c_3 + c_4 + 2 c_5 + 3 c_6 Ag: | c_2 = c_6 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_2 = c_1/2 + 1 c_3 = c_1/2 c_4 = 1 c_5 = c_1/2 - 2 c_6 = c_1/2 + 1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 10 and solve for the remaining coefficients: c_1 = 10 c_2 = 6 c_3 = 5 c_4 = 1 c_5 = 3 c_6 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 HNO_3 + 6 Ag ⟶ 5 H_2O + NO + 3 NO_2 + 6 AgNO_3

Structures

+ ⟶ + + +
+ ⟶ + + +

Names

nitric acid + silver ⟶ water + nitric oxide + nitrogen dioxide + silver nitrate
nitric acid + silver ⟶ water + nitric oxide + nitrogen dioxide + silver nitrate

Reaction thermodynamics

Entropy

| nitric acid | silver | water | nitric oxide | nitrogen dioxide | silver nitrate molecular entropy | 156 J/(mol K) | 42.6 J/(mol K) | 69.91 J/(mol K) | 211 J/(mol K) | 240 J/(mol K) | 140.9 J/(mol K) total entropy | 1560 J/(mol K) | 255.6 J/(mol K) | 349.6 J/(mol K) | 211 J/(mol K) | 720 J/(mol K) | 845.4 J/(mol K) | S_initial = 1816 J/(mol K) | | S_final = 2126 J/(mol K) | | | ΔS_rxn^0 | 2126 J/(mol K) - 1816 J/(mol K) = 310.3 J/(mol K) (endoentropic) | | | | |
| nitric acid | silver | water | nitric oxide | nitrogen dioxide | silver nitrate molecular entropy | 156 J/(mol K) | 42.6 J/(mol K) | 69.91 J/(mol K) | 211 J/(mol K) | 240 J/(mol K) | 140.9 J/(mol K) total entropy | 1560 J/(mol K) | 255.6 J/(mol K) | 349.6 J/(mol K) | 211 J/(mol K) | 720 J/(mol K) | 845.4 J/(mol K) | S_initial = 1816 J/(mol K) | | S_final = 2126 J/(mol K) | | | ΔS_rxn^0 | 2126 J/(mol K) - 1816 J/(mol K) = 310.3 J/(mol K) (endoentropic) | | | | |

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + Ag ⟶ H_2O + NO + NO_2 + AgNO_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: 10 HNO_3 + 6 Ag ⟶ 5 H_2O + NO + 3 NO_2 + 6 AgNO_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 | 10 | -10 Ag | 6 | -6 H_2O | 5 | 5 NO | 1 | 1 NO_2 | 3 | 3 AgNO_3 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 10 | -10 | ([HNO3])^(-10) Ag | 6 | -6 | ([Ag])^(-6) H_2O | 5 | 5 | ([H2O])^5 NO | 1 | 1 | [NO] NO_2 | 3 | 3 | ([NO2])^3 AgNO_3 | 6 | 6 | ([AgNO3])^6 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])^(-10) ([Ag])^(-6) ([H2O])^5 [NO] ([NO2])^3 ([AgNO3])^6 = (([H2O])^5 [NO] ([NO2])^3 ([AgNO3])^6)/(([HNO3])^10 ([Ag])^6)
Construct the equilibrium constant, K, expression for: HNO_3 + Ag ⟶ H_2O + NO + NO_2 + AgNO_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: 10 HNO_3 + 6 Ag ⟶ 5 H_2O + NO + 3 NO_2 + 6 AgNO_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 | 10 | -10 Ag | 6 | -6 H_2O | 5 | 5 NO | 1 | 1 NO_2 | 3 | 3 AgNO_3 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 10 | -10 | ([HNO3])^(-10) Ag | 6 | -6 | ([Ag])^(-6) H_2O | 5 | 5 | ([H2O])^5 NO | 1 | 1 | [NO] NO_2 | 3 | 3 | ([NO2])^3 AgNO_3 | 6 | 6 | ([AgNO3])^6 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])^(-10) ([Ag])^(-6) ([H2O])^5 [NO] ([NO2])^3 ([AgNO3])^6 = (([H2O])^5 [NO] ([NO2])^3 ([AgNO3])^6)/(([HNO3])^10 ([Ag])^6)

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + Ag ⟶ H_2O + NO + NO_2 + AgNO_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: 10 HNO_3 + 6 Ag ⟶ 5 H_2O + NO + 3 NO_2 + 6 AgNO_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 | 10 | -10 Ag | 6 | -6 H_2O | 5 | 5 NO | 1 | 1 NO_2 | 3 | 3 AgNO_3 | 6 | 6 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 | 10 | -10 | -1/10 (Δ[HNO3])/(Δt) Ag | 6 | -6 | -1/6 (Δ[Ag])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) NO | 1 | 1 | (Δ[NO])/(Δt) NO_2 | 3 | 3 | 1/3 (Δ[NO2])/(Δt) AgNO_3 | 6 | 6 | 1/6 (Δ[AgNO3])/(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 = -1/10 (Δ[HNO3])/(Δt) = -1/6 (Δ[Ag])/(Δt) = 1/5 (Δ[H2O])/(Δt) = (Δ[NO])/(Δt) = 1/3 (Δ[NO2])/(Δt) = 1/6 (Δ[AgNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_3 + Ag ⟶ H_2O + NO + NO_2 + AgNO_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: 10 HNO_3 + 6 Ag ⟶ 5 H_2O + NO + 3 NO_2 + 6 AgNO_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 | 10 | -10 Ag | 6 | -6 H_2O | 5 | 5 NO | 1 | 1 NO_2 | 3 | 3 AgNO_3 | 6 | 6 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 | 10 | -10 | -1/10 (Δ[HNO3])/(Δt) Ag | 6 | -6 | -1/6 (Δ[Ag])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) NO | 1 | 1 | (Δ[NO])/(Δt) NO_2 | 3 | 3 | 1/3 (Δ[NO2])/(Δt) AgNO_3 | 6 | 6 | 1/6 (Δ[AgNO3])/(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 = -1/10 (Δ[HNO3])/(Δt) = -1/6 (Δ[Ag])/(Δt) = 1/5 (Δ[H2O])/(Δt) = (Δ[NO])/(Δt) = 1/3 (Δ[NO2])/(Δt) = 1/6 (Δ[AgNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | silver | water | nitric oxide | nitrogen dioxide | silver nitrate formula | HNO_3 | Ag | H_2O | NO | NO_2 | AgNO_3 name | nitric acid | silver | water | nitric oxide | nitrogen dioxide | silver nitrate IUPAC name | nitric acid | silver | water | nitric oxide | Nitrogen dioxide | silver nitrate
| nitric acid | silver | water | nitric oxide | nitrogen dioxide | silver nitrate formula | HNO_3 | Ag | H_2O | NO | NO_2 | AgNO_3 name | nitric acid | silver | water | nitric oxide | nitrogen dioxide | silver nitrate IUPAC name | nitric acid | silver | water | nitric oxide | Nitrogen dioxide | silver nitrate

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