NaCl + Ag = Na + AgCl

NaCl sodium chloride + Ag silver ⟶ Na sodium + AgCl silver chloride

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

+ ⟶ +

sodium chloride + silver ⟶ sodium + silver chloride

| sodium chloride | silver | sodium | silver chloride molecular enthalpy | -411.2 kJ/mol | 0 kJ/mol | 0 kJ/mol | -127 kJ/mol total enthalpy | -411.2 kJ/mol | 0 kJ/mol | 0 kJ/mol | -127 kJ/mol | H_initial = -411.2 kJ/mol | | H_final = -127 kJ/mol | ΔH_rxn^0 | -127 kJ/mol - -411.2 kJ/mol = 284.2 kJ/mol (endothermic) | | |

| sodium chloride | silver | sodium | silver chloride molecular entropy | 72 J/(mol K) | 42.6 J/(mol K) | 51 J/(mol K) | 96.3 J/(mol K) total entropy | 72 J/(mol K) | 42.6 J/(mol K) | 51 J/(mol K) | 96.3 J/(mol K) | S_initial = 114.6 J/(mol K) | | S_final = 147.3 J/(mol K) | ΔS_rxn^0 | 147.3 J/(mol K) - 114.6 J/(mol K) = 32.7 J/(mol K) (endoentropic) | | |

Construct the equilibrium constant, K, expression for: NaCl + Ag ⟶ Na + 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 + Ag ⟶ Na + 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 Ag | 1 | -1 Na | 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) Ag | 1 | -1 | ([Ag])^(-1) Na | 1 | 1 | [Na] 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) ([Ag])^(-1) [Na] [AgCl] = ([Na] [AgCl])/([NaCl] [Ag])

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

| sodium chloride | silver | sodium | silver chloride formula | NaCl | Ag | Na | AgCl Hill formula | ClNa | Ag | Na | AgCl name | sodium chloride | silver | sodium | silver chloride IUPAC name | sodium chloride | silver | sodium | chlorosilver

| sodium chloride | silver | sodium | silver chloride molar mass | 58.44 g/mol | 107.8682 g/mol | 22.98976928 g/mol | 143.32 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 801 °C | 960 °C | 97.8 °C | 455 °C boiling point | 1413 °C | 2212 °C | 883 °C | 1554 °C density | 2.16 g/cm^3 | 10.49 g/cm^3 | 0.968 g/cm^3 | 5.56 g/cm^3 solubility in water | soluble | insoluble | decomposes | dynamic viscosity | | | 1.413×10^-5 Pa s (at 527 °C) | odor | odorless | | |