KNO3 + AgNO3 = KAg(NO3)2

KNO_3 potassium nitrate + AgNO_3 silver nitrate ⟶ KAg(NO3)2

Balance the chemical equation algebraically: KNO_3 + AgNO_3 ⟶ KAg(NO3)2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KNO_3 + c_2 AgNO_3 ⟶ c_3 KAg(NO3)2 Set the number of atoms in the reactants equal to the number of atoms in the products for K, N, O and Ag: K: | c_1 = c_3 N: | c_1 + c_2 = 2 c_3 O: | 3 c_1 + 3 c_2 = 6 c_3 Ag: | 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | KNO_3 + AgNO_3 ⟶ KAg(NO3)2

+ ⟶ KAg(NO3)2

potassium nitrate + silver nitrate ⟶ KAg(NO3)2

Construct the equilibrium constant, K, expression for: KNO_3 + AgNO_3 ⟶ KAg(NO3)2 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 + AgNO_3 ⟶ KAg(NO3)2 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 AgNO_3 | 1 | -1 KAg(NO3)2 | 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) AgNO_3 | 1 | -1 | ([AgNO3])^(-1) KAg(NO3)2 | 1 | 1 | [KAg(NO3)2] 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) ([AgNO3])^(-1) [KAg(NO3)2] = ([KAg(NO3)2])/([KNO3] [AgNO3])

Construct the rate of reaction expression for: KNO_3 + AgNO_3 ⟶ KAg(NO3)2 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 + AgNO_3 ⟶ KAg(NO3)2 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 AgNO_3 | 1 | -1 KAg(NO3)2 | 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) AgNO_3 | 1 | -1 | -(Δ[AgNO3])/(Δt) KAg(NO3)2 | 1 | 1 | (Δ[KAg(NO3)2])/(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[AgNO3])/(Δt) = (Δ[KAg(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium nitrate | silver nitrate | KAg(NO3)2 formula | KNO_3 | AgNO_3 | KAg(NO3)2 Hill formula | KNO_3 | AgNO_3 | AgKN2O6 name | potassium nitrate | silver nitrate |

| potassium nitrate | silver nitrate | KAg(NO3)2 molar mass | 101.1 g/mol | 169.87 g/mol | 270.97 g/mol phase | solid (at STP) | solid (at STP) | melting point | 334 °C | 212 °C | solubility in water | soluble | soluble | odor | odorless | odorless |