KNO3 + AgCl = KCl + AgNO3

KNO_3 potassium nitrate + AgCl silver chloride ⟶ KCl potassium chloride + AgNO_3 silver nitrate

Balance the chemical equation algebraically: KNO_3 + AgCl ⟶ KCl + AgNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KNO_3 + c_2 AgCl ⟶ c_3 KCl + c_4 AgNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for K, N, O, Ag and Cl: K: | c_1 = c_3 N: | c_1 = c_4 O: | 3 c_1 = 3 c_4 Ag: | c_2 = c_4 Cl: | c_2 = 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: | | KNO_3 + AgCl ⟶ KCl + AgNO_3

+ ⟶ +

potassium nitrate + silver chloride ⟶ potassium chloride + silver nitrate

| potassium nitrate | silver chloride | potassium chloride | silver nitrate molecular enthalpy | -494.6 kJ/mol | -127 kJ/mol | -436.5 kJ/mol | -124.4 kJ/mol total enthalpy | -494.6 kJ/mol | -127 kJ/mol | -436.5 kJ/mol | -124.4 kJ/mol | H_initial = -621.6 kJ/mol | | H_final = -560.9 kJ/mol | ΔH_rxn^0 | -560.9 kJ/mol - -621.6 kJ/mol = 60.7 kJ/mol (endothermic) | | |

| potassium nitrate | silver chloride | potassium chloride | silver nitrate molecular free energy | -394.9 kJ/mol | -109.8 kJ/mol | -408.5 kJ/mol | -33.4 kJ/mol total free energy | -394.9 kJ/mol | -109.8 kJ/mol | -408.5 kJ/mol | -33.4 kJ/mol | G_initial = -504.7 kJ/mol | | G_final = -441.9 kJ/mol | ΔG_rxn^0 | -441.9 kJ/mol - -504.7 kJ/mol = 62.8 kJ/mol (endergonic) | | |

Construct the equilibrium constant, K, expression for: KNO_3 + AgCl ⟶ KCl + AgNO_3 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: KNO_3 + AgCl ⟶ KCl + AgNO_3 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 KNO_3 | 1 | -1 AgCl | 1 | -1 KCl | 1 | 1 AgNO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KNO_3 | 1 | -1 | ([KNO3])^(-1) AgCl | 1 | -1 | ([AgCl])^(-1) KCl | 1 | 1 | [KCl] AgNO_3 | 1 | 1 | [AgNO3] 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 = ([KNO3])^(-1) ([AgCl])^(-1) [KCl] [AgNO3] = ([KCl] [AgNO3])/([KNO3] [AgCl])

Construct the rate of reaction expression for: KNO_3 + AgCl ⟶ KCl + AgNO_3 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: KNO_3 + AgCl ⟶ KCl + AgNO_3 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 KNO_3 | 1 | -1 AgCl | 1 | -1 KCl | 1 | 1 AgNO_3 | 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 KNO_3 | 1 | -1 | -(Δ[KNO3])/(Δt) AgCl | 1 | -1 | -(Δ[AgCl])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(Δt) AgNO_3 | 1 | 1 | (Δ[AgNO3])/(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[KNO3])/(Δt) = -(Δ[AgCl])/(Δt) = (Δ[KCl])/(Δt) = (Δ[AgNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium nitrate | silver chloride | potassium chloride | silver nitrate formula | KNO_3 | AgCl | KCl | AgNO_3 Hill formula | KNO_3 | AgCl | ClK | AgNO_3 name | potassium nitrate | silver chloride | potassium chloride | silver nitrate IUPAC name | potassium nitrate | chlorosilver | potassium chloride | silver nitrate

| potassium nitrate | silver chloride | potassium chloride | silver nitrate molar mass | 101.1 g/mol | 143.32 g/mol | 74.55 g/mol | 169.87 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 334 °C | 455 °C | 770 °C | 212 °C boiling point | | 1554 °C | 1420 °C | density | | 5.56 g/cm^3 | 1.98 g/cm^3 | solubility in water | soluble | | soluble | soluble odor | odorless | | odorless | odorless