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HCl + HNO3 + Ag = H2O + NO + AgCl

Input interpretation

HCl hydrogen chloride + HNO_3 nitric acid + Ag silver ⟶ H_2O water + NO nitric oxide + AgCl silver chloride
HCl hydrogen chloride + HNO_3 nitric acid + Ag silver ⟶ H_2O water + NO nitric oxide + AgCl silver chloride

Balanced equation

Balance the chemical equation algebraically: HCl + HNO_3 + Ag ⟶ H_2O + NO + AgCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 + c_3 Ag ⟶ c_4 H_2O + c_5 NO + c_6 AgCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, O and Ag: Cl: | c_1 = c_6 H: | c_1 + c_2 = 2 c_4 N: | c_2 = c_5 O: | 3 c_2 = c_4 + c_5 Ag: | c_3 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 3 c_4 = 2 c_5 = 1 c_6 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 HCl + HNO_3 + 3 Ag ⟶ 2 H_2O + NO + 3 AgCl
Balance the chemical equation algebraically: HCl + HNO_3 + Ag ⟶ H_2O + NO + AgCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 + c_3 Ag ⟶ c_4 H_2O + c_5 NO + c_6 AgCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, O and Ag: Cl: | c_1 = c_6 H: | c_1 + c_2 = 2 c_4 N: | c_2 = c_5 O: | 3 c_2 = c_4 + c_5 Ag: | c_3 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 3 c_4 = 2 c_5 = 1 c_6 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 HCl + HNO_3 + 3 Ag ⟶ 2 H_2O + NO + 3 AgCl

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

hydrogen chloride + nitric acid + silver ⟶ water + nitric oxide + silver chloride
hydrogen chloride + nitric acid + silver ⟶ water + nitric oxide + silver chloride

Reaction thermodynamics

Entropy

| hydrogen chloride | nitric acid | silver | water | nitric oxide | silver chloride molecular entropy | 187 J/(mol K) | 156 J/(mol K) | 42.6 J/(mol K) | 69.91 J/(mol K) | 211 J/(mol K) | 96.3 J/(mol K) total entropy | 561 J/(mol K) | 156 J/(mol K) | 127.8 J/(mol K) | 139.8 J/(mol K) | 211 J/(mol K) | 288.9 J/(mol K) | S_initial = 844.8 J/(mol K) | | | S_final = 639.7 J/(mol K) | | ΔS_rxn^0 | 639.7 J/(mol K) - 844.8 J/(mol K) = -205.1 J/(mol K) (exoentropic) | | | | |
| hydrogen chloride | nitric acid | silver | water | nitric oxide | silver chloride molecular entropy | 187 J/(mol K) | 156 J/(mol K) | 42.6 J/(mol K) | 69.91 J/(mol K) | 211 J/(mol K) | 96.3 J/(mol K) total entropy | 561 J/(mol K) | 156 J/(mol K) | 127.8 J/(mol K) | 139.8 J/(mol K) | 211 J/(mol K) | 288.9 J/(mol K) | S_initial = 844.8 J/(mol K) | | | S_final = 639.7 J/(mol K) | | ΔS_rxn^0 | 639.7 J/(mol K) - 844.8 J/(mol K) = -205.1 J/(mol K) (exoentropic) | | | | |

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + HNO_3 + Ag ⟶ H_2O + NO + AgCl 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: 3 HCl + HNO_3 + 3 Ag ⟶ 2 H_2O + NO + 3 AgCl 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 HCl | 3 | -3 HNO_3 | 1 | -1 Ag | 3 | -3 H_2O | 2 | 2 NO | 1 | 1 AgCl | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 3 | -3 | ([HCl])^(-3) HNO_3 | 1 | -1 | ([HNO3])^(-1) Ag | 3 | -3 | ([Ag])^(-3) H_2O | 2 | 2 | ([H2O])^2 NO | 1 | 1 | [NO] AgCl | 3 | 3 | ([AgCl])^3 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 = ([HCl])^(-3) ([HNO3])^(-1) ([Ag])^(-3) ([H2O])^2 [NO] ([AgCl])^3 = (([H2O])^2 [NO] ([AgCl])^3)/(([HCl])^3 [HNO3] ([Ag])^3)
Construct the equilibrium constant, K, expression for: HCl + HNO_3 + Ag ⟶ H_2O + NO + AgCl 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: 3 HCl + HNO_3 + 3 Ag ⟶ 2 H_2O + NO + 3 AgCl 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 HCl | 3 | -3 HNO_3 | 1 | -1 Ag | 3 | -3 H_2O | 2 | 2 NO | 1 | 1 AgCl | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 3 | -3 | ([HCl])^(-3) HNO_3 | 1 | -1 | ([HNO3])^(-1) Ag | 3 | -3 | ([Ag])^(-3) H_2O | 2 | 2 | ([H2O])^2 NO | 1 | 1 | [NO] AgCl | 3 | 3 | ([AgCl])^3 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 = ([HCl])^(-3) ([HNO3])^(-1) ([Ag])^(-3) ([H2O])^2 [NO] ([AgCl])^3 = (([H2O])^2 [NO] ([AgCl])^3)/(([HCl])^3 [HNO3] ([Ag])^3)

Rate of reaction

Construct the rate of reaction expression for: HCl + HNO_3 + Ag ⟶ H_2O + NO + AgCl 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: 3 HCl + HNO_3 + 3 Ag ⟶ 2 H_2O + NO + 3 AgCl 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 HCl | 3 | -3 HNO_3 | 1 | -1 Ag | 3 | -3 H_2O | 2 | 2 NO | 1 | 1 AgCl | 3 | 3 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 HCl | 3 | -3 | -1/3 (Δ[HCl])/(Δt) HNO_3 | 1 | -1 | -(Δ[HNO3])/(Δt) Ag | 3 | -3 | -1/3 (Δ[Ag])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NO | 1 | 1 | (Δ[NO])/(Δt) AgCl | 3 | 3 | 1/3 (Δ[AgCl])/(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 = -1/3 (Δ[HCl])/(Δt) = -(Δ[HNO3])/(Δt) = -1/3 (Δ[Ag])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[NO])/(Δt) = 1/3 (Δ[AgCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + HNO_3 + Ag ⟶ H_2O + NO + AgCl 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: 3 HCl + HNO_3 + 3 Ag ⟶ 2 H_2O + NO + 3 AgCl 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 HCl | 3 | -3 HNO_3 | 1 | -1 Ag | 3 | -3 H_2O | 2 | 2 NO | 1 | 1 AgCl | 3 | 3 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 HCl | 3 | -3 | -1/3 (Δ[HCl])/(Δt) HNO_3 | 1 | -1 | -(Δ[HNO3])/(Δt) Ag | 3 | -3 | -1/3 (Δ[Ag])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NO | 1 | 1 | (Δ[NO])/(Δt) AgCl | 3 | 3 | 1/3 (Δ[AgCl])/(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 = -1/3 (Δ[HCl])/(Δt) = -(Δ[HNO3])/(Δt) = -1/3 (Δ[Ag])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[NO])/(Δt) = 1/3 (Δ[AgCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | nitric acid | silver | water | nitric oxide | silver chloride formula | HCl | HNO_3 | Ag | H_2O | NO | AgCl Hill formula | ClH | HNO_3 | Ag | H_2O | NO | AgCl name | hydrogen chloride | nitric acid | silver | water | nitric oxide | silver chloride IUPAC name | hydrogen chloride | nitric acid | silver | water | nitric oxide | chlorosilver
| hydrogen chloride | nitric acid | silver | water | nitric oxide | silver chloride formula | HCl | HNO_3 | Ag | H_2O | NO | AgCl Hill formula | ClH | HNO_3 | Ag | H_2O | NO | AgCl name | hydrogen chloride | nitric acid | silver | water | nitric oxide | silver chloride IUPAC name | hydrogen chloride | nitric acid | silver | water | nitric oxide | chlorosilver

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