KCl + AgNO3 = ClNO3 + KAg

KCl potassium chloride + AgNO_3 silver nitrate ⟶ ClNO3 + KAg

Balance the chemical equation algebraically: KCl + AgNO_3 ⟶ ClNO3 + KAg Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KCl + c_2 AgNO_3 ⟶ c_3 ClNO3 + c_4 KAg Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, K, Ag, N and O: Cl: | c_1 = c_3 K: | c_1 = c_4 Ag: | c_2 = c_4 N: | c_2 = c_3 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 + AgNO_3 ⟶ ClNO3 + KAg

+ ⟶ ClNO3 + KAg

potassium chloride + silver nitrate ⟶ ClNO3 + KAg

Construct the equilibrium constant, K, expression for: KCl + AgNO_3 ⟶ ClNO3 + KAg 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 + AgNO_3 ⟶ ClNO3 + KAg 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 AgNO_3 | 1 | -1 ClNO3 | 1 | 1 KAg | 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) AgNO_3 | 1 | -1 | ([AgNO3])^(-1) ClNO3 | 1 | 1 | [ClNO3] KAg | 1 | 1 | [KAg] 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) ([AgNO3])^(-1) [ClNO3] [KAg] = ([ClNO3] [KAg])/([KCl] [AgNO3])

Construct the rate of reaction expression for: KCl + AgNO_3 ⟶ ClNO3 + KAg 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 + AgNO_3 ⟶ ClNO3 + KAg 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 AgNO_3 | 1 | -1 ClNO3 | 1 | 1 KAg | 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) AgNO_3 | 1 | -1 | -(Δ[AgNO3])/(Δt) ClNO3 | 1 | 1 | (Δ[ClNO3])/(Δt) KAg | 1 | 1 | (Δ[KAg])/(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[AgNO3])/(Δt) = (Δ[ClNO3])/(Δt) = (Δ[KAg])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium chloride | silver nitrate | ClNO3 | KAg formula | KCl | AgNO_3 | ClNO3 | KAg Hill formula | ClK | AgNO_3 | ClNO3 | AgK name | potassium chloride | silver nitrate | |

| potassium chloride | silver nitrate | ClNO3 | KAg molar mass | 74.55 g/mol | 169.87 g/mol | 97.45 g/mol | 146.967 g/mol phase | solid (at STP) | solid (at STP) | | melting point | 770 °C | 212 °C | | boiling point | 1420 °C | | | density | 1.98 g/cm^3 | | | solubility in water | soluble | soluble | | odor | odorless | odorless | |