I2 + AgNO3 = AgI + INO3

I_2 iodine + AgNO_3 silver nitrate ⟶ AgI silver(I) iodide + INO3

Balance the chemical equation algebraically: I_2 + AgNO_3 ⟶ AgI + INO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 I_2 + c_2 AgNO_3 ⟶ c_3 AgI + c_4 INO3 Set the number of atoms in the reactants equal to the number of atoms in the products for I, Ag, N and O: I: | 2 c_1 = c_3 + c_4 Ag: | c_2 = c_3 N: | c_2 = c_4 O: | 3 c_2 = 3 c_4 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: | | I_2 + AgNO_3 ⟶ AgI + INO3

+ ⟶ + INO3

iodine + silver nitrate ⟶ silver(I) iodide + INO3

Construct the equilibrium constant, K, expression for: I_2 + AgNO_3 ⟶ AgI + INO3 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: I_2 + AgNO_3 ⟶ AgI + INO3 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 I_2 | 1 | -1 AgNO_3 | 1 | -1 AgI | 1 | 1 INO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression I_2 | 1 | -1 | ([I2])^(-1) AgNO_3 | 1 | -1 | ([AgNO3])^(-1) AgI | 1 | 1 | [AgI] INO3 | 1 | 1 | [INO3] 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 = ([I2])^(-1) ([AgNO3])^(-1) [AgI] [INO3] = ([AgI] [INO3])/([I2] [AgNO3])

Construct the rate of reaction expression for: I_2 + AgNO_3 ⟶ AgI + INO3 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: I_2 + AgNO_3 ⟶ AgI + INO3 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 I_2 | 1 | -1 AgNO_3 | 1 | -1 AgI | 1 | 1 INO3 | 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 I_2 | 1 | -1 | -(Δ[I2])/(Δt) AgNO_3 | 1 | -1 | -(Δ[AgNO3])/(Δt) AgI | 1 | 1 | (Δ[AgI])/(Δt) INO3 | 1 | 1 | (Δ[INO3])/(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[I2])/(Δt) = -(Δ[AgNO3])/(Δt) = (Δ[AgI])/(Δt) = (Δ[INO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| iodine | silver nitrate | silver(I) iodide | INO3 formula | I_2 | AgNO_3 | AgI | INO3 name | iodine | silver nitrate | silver(I) iodide | IUPAC name | molecular iodine | silver nitrate | silver iodide |

| iodine | silver nitrate | silver(I) iodide | INO3 molar mass | 253.80894 g/mol | 169.87 g/mol | 234.7727 g/mol | 188.91 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 113 °C | 212 °C | 557 °C | boiling point | 184 °C | | 1506 °C | density | 4.94 g/cm^3 | | 5.68 g/cm^3 | solubility in water | | soluble | slightly soluble | dynamic viscosity | 0.00227 Pa s (at 116 °C) | | | odor | | odorless | |