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HCl + AgNO3 = HNO3 + AgCl

Input interpretation

HCl (hydrogen chloride) + AgNO_3 (silver nitrate) ⟶ HNO_3 (nitric acid) + AgCl (silver chloride)
HCl (hydrogen chloride) + AgNO_3 (silver nitrate) ⟶ HNO_3 (nitric acid) + AgCl (silver chloride)

Balanced equation

Balance the chemical equation algebraically: HCl + AgNO_3 ⟶ HNO_3 + AgCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 AgNO_3 ⟶ c_3 HNO_3 + c_4 AgCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Ag, N and O: Cl: | c_1 = c_4 H: | c_1 = c_3 Ag: | c_2 = c_4 N: | c_2 = c_3 O: | 3 c_2 = 3 c_3 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: |   | HCl + AgNO_3 ⟶ HNO_3 + AgCl
Balance the chemical equation algebraically: HCl + AgNO_3 ⟶ HNO_3 + AgCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 AgNO_3 ⟶ c_3 HNO_3 + c_4 AgCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Ag, N and O: Cl: | c_1 = c_4 H: | c_1 = c_3 Ag: | c_2 = c_4 N: | c_2 = c_3 O: | 3 c_2 = 3 c_3 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | HCl + AgNO_3 ⟶ HNO_3 + AgCl

Structures

 + ⟶ +
+ ⟶ +

Names

hydrogen chloride + silver nitrate ⟶ nitric acid + silver chloride
hydrogen chloride + silver nitrate ⟶ nitric acid + silver chloride

Reaction thermodynamics

Gibbs free energy

 | hydrogen chloride | silver nitrate | nitric acid | silver chloride molecular free energy | -95.3 kJ/mol | -33.4 kJ/mol | -80.7 kJ/mol | -109.8 kJ/mol total free energy | -95.3 kJ/mol | -33.4 kJ/mol | -80.7 kJ/mol | -109.8 kJ/mol  | G_initial = -128.7 kJ/mol | | G_final = -190.5 kJ/mol |  ΔG_rxn^0 | -190.5 kJ/mol - -128.7 kJ/mol = -61.8 kJ/mol (exergonic) | | |
| hydrogen chloride | silver nitrate | nitric acid | silver chloride molecular free energy | -95.3 kJ/mol | -33.4 kJ/mol | -80.7 kJ/mol | -109.8 kJ/mol total free energy | -95.3 kJ/mol | -33.4 kJ/mol | -80.7 kJ/mol | -109.8 kJ/mol | G_initial = -128.7 kJ/mol | | G_final = -190.5 kJ/mol | ΔG_rxn^0 | -190.5 kJ/mol - -128.7 kJ/mol = -61.8 kJ/mol (exergonic) | | |

Entropy

 | hydrogen chloride | silver nitrate | nitric acid | silver chloride molecular entropy | 187 J/(mol K) | 140.9 J/(mol K) | 156 J/(mol K) | 96.3 J/(mol K) total entropy | 187 J/(mol K) | 140.9 J/(mol K) | 156 J/(mol K) | 96.3 J/(mol K)  | S_initial = 327.9 J/(mol K) | | S_final = 252.3 J/(mol K) |  ΔS_rxn^0 | 252.3 J/(mol K) - 327.9 J/(mol K) = -75.6 J/(mol K) (exoentropic) | | |
| hydrogen chloride | silver nitrate | nitric acid | silver chloride molecular entropy | 187 J/(mol K) | 140.9 J/(mol K) | 156 J/(mol K) | 96.3 J/(mol K) total entropy | 187 J/(mol K) | 140.9 J/(mol K) | 156 J/(mol K) | 96.3 J/(mol K) | S_initial = 327.9 J/(mol K) | | S_final = 252.3 J/(mol K) | ΔS_rxn^0 | 252.3 J/(mol K) - 327.9 J/(mol K) = -75.6 J/(mol K) (exoentropic) | | |

Equilibrium constant

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

Rate of reaction

Construct the rate of reaction expression for: HCl + AgNO_3 ⟶ HNO_3 + 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: HCl + AgNO_3 ⟶ HNO_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 | 1 | -1 AgNO_3 | 1 | -1 HNO_3 | 1 | 1 AgCl | 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 HCl | 1 | -1 | -(Δ[HCl])/(Δt) AgNO_3 | 1 | -1 | -(Δ[AgNO3])/(Δt) HNO_3 | 1 | 1 | (Δ[HNO3])/(Δt) AgCl | 1 | 1 | (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 = -(Δ[HCl])/(Δt) = -(Δ[AgNO3])/(Δt) = (Δ[HNO3])/(Δt) = (Δ[AgCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + AgNO_3 ⟶ HNO_3 + 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: HCl + AgNO_3 ⟶ HNO_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 | 1 | -1 AgNO_3 | 1 | -1 HNO_3 | 1 | 1 AgCl | 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 HCl | 1 | -1 | -(Δ[HCl])/(Δt) AgNO_3 | 1 | -1 | -(Δ[AgNO3])/(Δt) HNO_3 | 1 | 1 | (Δ[HNO3])/(Δt) AgCl | 1 | 1 | (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 = -(Δ[HCl])/(Δt) = -(Δ[AgNO3])/(Δt) = (Δ[HNO3])/(Δt) = (Δ[AgCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

 | hydrogen chloride | silver nitrate | nitric acid | silver chloride formula | HCl | AgNO_3 | HNO_3 | AgCl Hill formula | ClH | AgNO_3 | HNO_3 | AgCl name | hydrogen chloride | silver nitrate | nitric acid | silver chloride IUPAC name | hydrogen chloride | silver nitrate | nitric acid | chlorosilver
| hydrogen chloride | silver nitrate | nitric acid | silver chloride formula | HCl | AgNO_3 | HNO_3 | AgCl Hill formula | ClH | AgNO_3 | HNO_3 | AgCl name | hydrogen chloride | silver nitrate | nitric acid | silver chloride IUPAC name | hydrogen chloride | silver nitrate | nitric acid | chlorosilver

Substance properties

 | hydrogen chloride | silver nitrate | nitric acid | silver chloride molar mass | 36.46 g/mol | 169.87 g/mol | 63.012 g/mol | 143.32 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | -114.17 °C | 212 °C | -41.6 °C | 455 °C boiling point | -85 °C | | 83 °C | 1554 °C density | 0.00149 g/cm^3 (at 25 °C) | | 1.5129 g/cm^3 | 5.56 g/cm^3 solubility in water | miscible | soluble | miscible |  dynamic viscosity | | | 7.6×10^-4 Pa s (at 25 °C) |  odor | | odorless | |
| hydrogen chloride | silver nitrate | nitric acid | silver chloride molar mass | 36.46 g/mol | 169.87 g/mol | 63.012 g/mol | 143.32 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | -114.17 °C | 212 °C | -41.6 °C | 455 °C boiling point | -85 °C | | 83 °C | 1554 °C density | 0.00149 g/cm^3 (at 25 °C) | | 1.5129 g/cm^3 | 5.56 g/cm^3 solubility in water | miscible | soluble | miscible | dynamic viscosity | | | 7.6×10^-4 Pa s (at 25 °C) | odor | | odorless | |

Units