NaCl + AgF = AgCl + NaF

NaCl sodium chloride + AgF silver fluoride ⟶ AgCl silver chloride + NaF sodium fluoride

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

+ ⟶ +

sodium chloride + silver fluoride ⟶ silver chloride + sodium fluoride

| sodium chloride | silver fluoride | silver chloride | sodium fluoride molecular enthalpy | -411.2 kJ/mol | -204.6 kJ/mol | -127 kJ/mol | -576.6 kJ/mol total enthalpy | -411.2 kJ/mol | -204.6 kJ/mol | -127 kJ/mol | -576.6 kJ/mol | H_initial = -615.8 kJ/mol | | H_final = -703.6 kJ/mol | ΔH_rxn^0 | -703.6 kJ/mol - -615.8 kJ/mol = -87.8 kJ/mol (exothermic) | | |

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

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

| sodium chloride | silver fluoride | silver chloride | sodium fluoride formula | NaCl | AgF | AgCl | NaF Hill formula | ClNa | AgF | AgCl | FNa name | sodium chloride | silver fluoride | silver chloride | sodium fluoride IUPAC name | sodium chloride | fluorosilver | chlorosilver | sodium fluoride

| sodium chloride | silver fluoride | silver chloride | sodium fluoride molar mass | 58.44 g/mol | 126.8666 g/mol | 143.32 g/mol | 41.98817244 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 801 °C | 300 °C | 455 °C | 993 °C boiling point | 1413 °C | 1150 °C | 1554 °C | 1700 °C density | 2.16 g/cm^3 | 5.852 g/cm^3 | 5.56 g/cm^3 | 2.558 g/cm^3 solubility in water | soluble | | | dynamic viscosity | | | | 0.00105 Pa s (at 1160 °C) odor | odorless | | | odorless