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HNO3 + Ag = H2O + NO2 + AgNO3

Input interpretation

HNO_3 (nitric acid) + Ag (silver) ⟶ H_2O (water) + NO_2 (nitrogen dioxide) + AgNO_3 (silver nitrate)
HNO_3 (nitric acid) + Ag (silver) ⟶ H_2O (water) + NO_2 (nitrogen dioxide) + AgNO_3 (silver nitrate)

Balanced equation

Balance the chemical equation algebraically: HNO_3 + Ag ⟶ H_2O + 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_2 + c_5 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 O: | 3 c_1 = c_3 + 2 c_4 + 3 c_5 Ag: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 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: | | 2 HNO_3 + Ag ⟶ H_2O + NO_2 + AgNO_3
Balance the chemical equation algebraically: HNO_3 + Ag ⟶ H_2O + 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_2 + c_5 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 O: | 3 c_1 = c_3 + 2 c_4 + 3 c_5 Ag: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 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: | | 2 HNO_3 + Ag ⟶ H_2O + NO_2 + AgNO_3

Structures

+ ⟶ + +
+ ⟶ + +

Names

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

Reaction thermodynamics

Entropy

| nitric acid | silver | water | nitrogen dioxide | silver nitrate molecular entropy | 156 J/(mol K) | 42.6 J/(mol K) | 69.91 J/(mol K) | 240 J/(mol K) | 140.9 J/(mol K) total entropy | 312 J/(mol K) | 42.6 J/(mol K) | 69.91 J/(mol K) | 240 J/(mol K) | 140.9 J/(mol K) | S_initial = 354.6 J/(mol K) | | S_final = 450.8 J/(mol K) | | ΔS_rxn^0 | 450.8 J/(mol K) - 354.6 J/(mol K) = 96.21 J/(mol K) (endoentropic) | | | |
| nitric acid | silver | water | nitrogen dioxide | silver nitrate molecular entropy | 156 J/(mol K) | 42.6 J/(mol K) | 69.91 J/(mol K) | 240 J/(mol K) | 140.9 J/(mol K) total entropy | 312 J/(mol K) | 42.6 J/(mol K) | 69.91 J/(mol K) | 240 J/(mol K) | 140.9 J/(mol K) | S_initial = 354.6 J/(mol K) | | S_final = 450.8 J/(mol K) | | ΔS_rxn^0 | 450.8 J/(mol K) - 354.6 J/(mol K) = 96.21 J/(mol K) (endoentropic) | | | |

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + Ag ⟶ H_2O + 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: 2 HNO_3 + Ag ⟶ H_2O + NO_2 + 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 | 2 | -2 Ag | 1 | -1 H_2O | 1 | 1 NO_2 | 1 | 1 AgNO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 2 | -2 | ([HNO3])^(-2) Ag | 1 | -1 | ([Ag])^(-1) H_2O | 1 | 1 | [H2O] NO_2 | 1 | 1 | [NO2] AgNO_3 | 1 | 1 | [AgNO3] 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])^(-2) ([Ag])^(-1) [H2O] [NO2] [AgNO3] = ([H2O] [NO2] [AgNO3])/(([HNO3])^2 [Ag])
Construct the equilibrium constant, K, expression for: HNO_3 + Ag ⟶ H_2O + 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: 2 HNO_3 + Ag ⟶ H_2O + NO_2 + 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 | 2 | -2 Ag | 1 | -1 H_2O | 1 | 1 NO_2 | 1 | 1 AgNO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 2 | -2 | ([HNO3])^(-2) Ag | 1 | -1 | ([Ag])^(-1) H_2O | 1 | 1 | [H2O] NO_2 | 1 | 1 | [NO2] AgNO_3 | 1 | 1 | [AgNO3] 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])^(-2) ([Ag])^(-1) [H2O] [NO2] [AgNO3] = ([H2O] [NO2] [AgNO3])/(([HNO3])^2 [Ag])

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + Ag ⟶ H_2O + 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: 2 HNO_3 + Ag ⟶ H_2O + NO_2 + 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 | 2 | -2 Ag | 1 | -1 H_2O | 1 | 1 NO_2 | 1 | 1 AgNO_3 | 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 HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) Ag | 1 | -1 | -(Δ[Ag])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NO_2 | 1 | 1 | (Δ[NO2])/(Δt) AgNO_3 | 1 | 1 | (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 = -1/2 (Δ[HNO3])/(Δt) = -(Δ[Ag])/(Δt) = (Δ[H2O])/(Δt) = (Δ[NO2])/(Δt) = (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_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: 2 HNO_3 + Ag ⟶ H_2O + NO_2 + 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 | 2 | -2 Ag | 1 | -1 H_2O | 1 | 1 NO_2 | 1 | 1 AgNO_3 | 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 HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) Ag | 1 | -1 | -(Δ[Ag])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NO_2 | 1 | 1 | (Δ[NO2])/(Δt) AgNO_3 | 1 | 1 | (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 = -1/2 (Δ[HNO3])/(Δt) = -(Δ[Ag])/(Δt) = (Δ[H2O])/(Δt) = (Δ[NO2])/(Δt) = (Δ[AgNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | silver | water | nitrogen dioxide | silver nitrate formula | HNO_3 | Ag | H_2O | NO_2 | AgNO_3 name | nitric acid | silver | water | nitrogen dioxide | silver nitrate IUPAC name | nitric acid | silver | water | Nitrogen dioxide | silver nitrate
| nitric acid | silver | water | nitrogen dioxide | silver nitrate formula | HNO_3 | Ag | H_2O | NO_2 | AgNO_3 name | nitric acid | silver | water | nitrogen dioxide | silver nitrate IUPAC name | nitric acid | silver | water | Nitrogen dioxide | silver nitrate

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