AgNO3 + NH4Cl = NH4NO3 + AgCl

AgNO_3 silver nitrate + NH_4Cl ammonium chloride ⟶ NH_4NO_3 ammonium nitrate + AgCl silver chloride

Balance the chemical equation algebraically: AgNO_3 + NH_4Cl ⟶ NH_4NO_3 + AgCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 NH_4Cl ⟶ c_3 NH_4NO_3 + c_4 AgCl Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O, Cl and H: Ag: | c_1 = c_4 N: | c_1 + c_2 = 2 c_3 O: | 3 c_1 = 3 c_3 Cl: | c_2 = c_4 H: | 4 c_2 = 4 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: | | AgNO_3 + NH_4Cl ⟶ NH_4NO_3 + AgCl

+ ⟶ +

silver nitrate + ammonium chloride ⟶ ammonium nitrate + silver chloride

| silver nitrate | ammonium chloride | ammonium nitrate | silver chloride molecular free energy | -33.4 kJ/mol | -202.9 kJ/mol | -183.9 kJ/mol | -109.8 kJ/mol total free energy | -33.4 kJ/mol | -202.9 kJ/mol | -183.9 kJ/mol | -109.8 kJ/mol | G_initial = -236.3 kJ/mol | | G_final = -293.7 kJ/mol | ΔG_rxn^0 | -293.7 kJ/mol - -236.3 kJ/mol = -57.4 kJ/mol (exergonic) | | |

Construct the equilibrium constant, K, expression for: AgNO_3 + NH_4Cl ⟶ NH_4NO_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: AgNO_3 + NH_4Cl ⟶ NH_4NO_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 AgNO_3 | 1 | -1 NH_4Cl | 1 | -1 NH_4NO_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 AgNO_3 | 1 | -1 | ([AgNO3])^(-1) NH_4Cl | 1 | -1 | ([NH4Cl])^(-1) NH_4NO_3 | 1 | 1 | [NH4NO3] 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 = ([AgNO3])^(-1) ([NH4Cl])^(-1) [NH4NO3] [AgCl] = ([NH4NO3] [AgCl])/([AgNO3] [NH4Cl])

Construct the rate of reaction expression for: AgNO_3 + NH_4Cl ⟶ NH_4NO_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: AgNO_3 + NH_4Cl ⟶ NH_4NO_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 AgNO_3 | 1 | -1 NH_4Cl | 1 | -1 NH_4NO_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 AgNO_3 | 1 | -1 | -(Δ[AgNO3])/(Δt) NH_4Cl | 1 | -1 | -(Δ[NH4Cl])/(Δt) NH_4NO_3 | 1 | 1 | (Δ[NH4NO3])/(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[AgNO3])/(Δt) = -(Δ[NH4Cl])/(Δt) = (Δ[NH4NO3])/(Δt) = (Δ[AgCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| silver nitrate | ammonium chloride | ammonium nitrate | silver chloride formula | AgNO_3 | NH_4Cl | NH_4NO_3 | AgCl Hill formula | AgNO_3 | ClH_4N | H_4N_2O_3 | AgCl name | silver nitrate | ammonium chloride | ammonium nitrate | silver chloride IUPAC name | silver nitrate | ammonium chloride | | chlorosilver

| silver nitrate | ammonium chloride | ammonium nitrate | silver chloride molar mass | 169.87 g/mol | 53.49 g/mol | 80.04 g/mol | 143.32 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 212 °C | 340 °C | 169 °C | 455 °C boiling point | | | 210 °C | 1554 °C density | | 1.5256 g/cm^3 | 1.73 g/cm^3 | 5.56 g/cm^3 solubility in water | soluble | soluble | | odor | odorless | | odorless |