NaCl + AgNO3 = NaNO3 + AgCl

NaCl (sodium chloride) + AgNO_3 (silver nitrate) ⟶ NaNO_3 (sodium nitrate) + AgCl (silver chloride)

Balance the chemical equation algebraically: NaCl + AgNO_3 ⟶ NaNO_3 + AgCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaCl + c_2 AgNO_3 ⟶ c_3 NaNO_3 + c_4 AgCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Na, Ag, N and O: Cl: | c_1 = c_4 Na: | 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: | | NaCl + AgNO_3 ⟶ NaNO_3 + AgCl

+ ⟶ +

sodium chloride + silver nitrate ⟶ sodium nitrate + silver chloride

| sodium chloride | silver nitrate | sodium nitrate | silver chloride molecular enthalpy | -411.2 kJ/mol | -124.4 kJ/mol | -467.9 kJ/mol | -127 kJ/mol total enthalpy | -411.2 kJ/mol | -124.4 kJ/mol | -467.9 kJ/mol | -127 kJ/mol | H_initial = -535.6 kJ/mol | | H_final = -594.9 kJ/mol | ΔH_rxn^0 | -594.9 kJ/mol - -535.6 kJ/mol = -59.3 kJ/mol (exothermic) | | |

| sodium chloride | silver nitrate | sodium nitrate | silver chloride molecular free energy | -384.1 kJ/mol | -33.4 kJ/mol | -366 kJ/mol | -109.8 kJ/mol total free energy | -384.1 kJ/mol | -33.4 kJ/mol | -366 kJ/mol | -109.8 kJ/mol | G_initial = -417.5 kJ/mol | | G_final = -475.8 kJ/mol | ΔG_rxn^0 | -475.8 kJ/mol - -417.5 kJ/mol = -58.3 kJ/mol (exergonic) | | |

| sodium chloride | silver nitrate | sodium nitrate | silver chloride molecular entropy | 72 J/(mol K) | 140.9 J/(mol K) | 116 J/(mol K) | 96.3 J/(mol K) total entropy | 72 J/(mol K) | 140.9 J/(mol K) | 116 J/(mol K) | 96.3 J/(mol K) | S_initial = 212.9 J/(mol K) | | S_final = 212.3 J/(mol K) | ΔS_rxn^0 | 212.3 J/(mol K) - 212.9 J/(mol K) = -0.6 J/(mol K) (exoentropic) | | |

Construct the equilibrium constant, K, expression for: NaCl + AgNO_3 ⟶ NaNO_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: NaCl + AgNO_3 ⟶ NaNO_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 NaCl | 1 | -1 AgNO_3 | 1 | -1 NaNO_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 NaCl | 1 | -1 | ([NaCl])^(-1) AgNO_3 | 1 | -1 | ([AgNO3])^(-1) NaNO_3 | 1 | 1 | [NaNO3] 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 = ([NaCl])^(-1) ([AgNO3])^(-1) [NaNO3] [AgCl] = ([NaNO3] [AgCl])/([NaCl] [AgNO3])

Construct the rate of reaction expression for: NaCl + AgNO_3 ⟶ NaNO_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: NaCl + AgNO_3 ⟶ NaNO_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 NaCl | 1 | -1 AgNO_3 | 1 | -1 NaNO_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 NaCl | 1 | -1 | -(Δ[NaCl])/(Δt) AgNO_3 | 1 | -1 | -(Δ[AgNO3])/(Δt) NaNO_3 | 1 | 1 | (Δ[NaNO3])/(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[NaCl])/(Δt) = -(Δ[AgNO3])/(Δt) = (Δ[NaNO3])/(Δt) = (Δ[AgCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sodium chloride | silver nitrate | sodium nitrate | silver chloride formula | NaCl | AgNO_3 | NaNO_3 | AgCl Hill formula | ClNa | AgNO_3 | NNaO_3 | AgCl name | sodium chloride | silver nitrate | sodium nitrate | silver chloride IUPAC name | sodium chloride | silver nitrate | sodium nitrate | chlorosilver

| sodium chloride | silver nitrate | sodium nitrate | silver chloride molar mass | 58.44 g/mol | 169.87 g/mol | 84.994 g/mol | 143.32 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 801 °C | 212 °C | 306 °C | 455 °C boiling point | 1413 °C | | | 1554 °C density | 2.16 g/cm^3 | | 2.26 g/cm^3 | 5.56 g/cm^3 solubility in water | soluble | soluble | soluble | dynamic viscosity | | | 0.003 Pa s (at 250 °C) | odor | odorless | odorless | |