KCl + NH4NO3 = KNO3 + NH4Cl

KCl potassium chloride + NH_4NO_3 ammonium nitrate ⟶ KNO_3 potassium nitrate + NH_4Cl ammonium chloride

Balance the chemical equation algebraically: KCl + NH_4NO_3 ⟶ KNO_3 + NH_4Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KCl + c_2 NH_4NO_3 ⟶ c_3 KNO_3 + c_4 NH_4Cl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, K, H, N and O: Cl: | c_1 = c_4 K: | c_1 = c_3 H: | 4 c_2 = 4 c_4 N: | 2 c_2 = c_3 + c_4 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: | | KCl + NH_4NO_3 ⟶ KNO_3 + NH_4Cl

+ ⟶ +

potassium chloride + ammonium nitrate ⟶ potassium nitrate + ammonium chloride

| potassium chloride | ammonium nitrate | potassium nitrate | ammonium chloride molecular free energy | -408.5 kJ/mol | -183.9 kJ/mol | -394.9 kJ/mol | -202.9 kJ/mol total free energy | -408.5 kJ/mol | -183.9 kJ/mol | -394.9 kJ/mol | -202.9 kJ/mol | G_initial = -592.4 kJ/mol | | G_final = -597.8 kJ/mol | ΔG_rxn^0 | -597.8 kJ/mol - -592.4 kJ/mol = -5.4 kJ/mol (exergonic) | | |

Construct the equilibrium constant, K, expression for: KCl + NH_4NO_3 ⟶ KNO_3 + NH_4Cl 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: KCl + NH_4NO_3 ⟶ KNO_3 + NH_4Cl 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 KCl | 1 | -1 NH_4NO_3 | 1 | -1 KNO_3 | 1 | 1 NH_4Cl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KCl | 1 | -1 | ([KCl])^(-1) NH_4NO_3 | 1 | -1 | ([NH4NO3])^(-1) KNO_3 | 1 | 1 | [KNO3] NH_4Cl | 1 | 1 | [NH4Cl] 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 = ([KCl])^(-1) ([NH4NO3])^(-1) [KNO3] [NH4Cl] = ([KNO3] [NH4Cl])/([KCl] [NH4NO3])

Construct the rate of reaction expression for: KCl + NH_4NO_3 ⟶ KNO_3 + NH_4Cl 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: KCl + NH_4NO_3 ⟶ KNO_3 + NH_4Cl 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 KCl | 1 | -1 NH_4NO_3 | 1 | -1 KNO_3 | 1 | 1 NH_4Cl | 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 KCl | 1 | -1 | -(Δ[KCl])/(Δt) NH_4NO_3 | 1 | -1 | -(Δ[NH4NO3])/(Δt) KNO_3 | 1 | 1 | (Δ[KNO3])/(Δt) NH_4Cl | 1 | 1 | (Δ[NH4Cl])/(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[KCl])/(Δt) = -(Δ[NH4NO3])/(Δt) = (Δ[KNO3])/(Δt) = (Δ[NH4Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium chloride | ammonium nitrate | potassium nitrate | ammonium chloride formula | KCl | NH_4NO_3 | KNO_3 | NH_4Cl Hill formula | ClK | H_4N_2O_3 | KNO_3 | ClH_4N name | potassium chloride | ammonium nitrate | potassium nitrate | ammonium chloride

| potassium chloride | ammonium nitrate | potassium nitrate | ammonium chloride molar mass | 74.55 g/mol | 80.04 g/mol | 101.1 g/mol | 53.49 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 770 °C | 169 °C | 334 °C | 340 °C boiling point | 1420 °C | 210 °C | | density | 1.98 g/cm^3 | 1.73 g/cm^3 | | 1.5256 g/cm^3 solubility in water | soluble | | soluble | soluble odor | odorless | odorless | odorless |