AgNO3 + KF = KNO3 + AgF

AgNO_3 silver nitrate + KF potassium fluoride ⟶ KNO_3 potassium nitrate + AgF silver fluoride

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

+ ⟶ +

silver nitrate + potassium fluoride ⟶ potassium nitrate + silver fluoride

| silver nitrate | potassium fluoride | potassium nitrate | silver fluoride molecular enthalpy | -124.4 kJ/mol | -567.3 kJ/mol | -494.6 kJ/mol | -204.6 kJ/mol total enthalpy | -124.4 kJ/mol | -567.3 kJ/mol | -494.6 kJ/mol | -204.6 kJ/mol | H_initial = -691.7 kJ/mol | | H_final = -699.2 kJ/mol | ΔH_rxn^0 | -699.2 kJ/mol - -691.7 kJ/mol = -7.5 kJ/mol (exothermic) | | |

Construct the equilibrium constant, K, expression for: AgNO_3 + KF ⟶ KNO_3 + AgF 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 + KF ⟶ KNO_3 + AgF 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 KF | 1 | -1 KNO_3 | 1 | 1 AgF | 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) KF | 1 | -1 | ([KF])^(-1) KNO_3 | 1 | 1 | [KNO3] AgF | 1 | 1 | [AgF] 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) ([KF])^(-1) [KNO3] [AgF] = ([KNO3] [AgF])/([AgNO3] [KF])

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

| silver nitrate | potassium fluoride | potassium nitrate | silver fluoride formula | AgNO_3 | KF | KNO_3 | AgF Hill formula | AgNO_3 | FK | KNO_3 | AgF name | silver nitrate | potassium fluoride | potassium nitrate | silver fluoride IUPAC name | silver nitrate | potassium fluoride | potassium nitrate | fluorosilver

| silver nitrate | potassium fluoride | potassium nitrate | silver fluoride molar mass | 169.87 g/mol | 58.0967 g/mol | 101.1 g/mol | 126.8666 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 212 °C | 858 °C | 334 °C | 300 °C boiling point | | 1505 °C | | 1150 °C density | | 1.89 g/cm^3 | | 5.852 g/cm^3 solubility in water | soluble | | soluble | odor | odorless | | odorless |