AgNO3 + ZnCl2 = ZnNO3 + AgCl2

AgNO_3 silver nitrate + ZnCl_2 zinc chloride ⟶ ZnNO3 + AgCl2

Balance the chemical equation algebraically: AgNO_3 + ZnCl_2 ⟶ ZnNO3 + AgCl2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 ZnCl_2 ⟶ c_3 ZnNO3 + c_4 AgCl2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O, Cl and Zn: Ag: | c_1 = c_4 N: | c_1 = c_3 O: | 3 c_1 = 3 c_3 Cl: | 2 c_2 = 2 c_4 Zn: | 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 + ZnCl_2 ⟶ ZnNO3 + AgCl2

+ ⟶ ZnNO3 + AgCl2

silver nitrate + zinc chloride ⟶ ZnNO3 + AgCl2

Construct the equilibrium constant, K, expression for: AgNO_3 + ZnCl_2 ⟶ ZnNO3 + AgCl2 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 + ZnCl_2 ⟶ ZnNO3 + AgCl2 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 ZnCl_2 | 1 | -1 ZnNO3 | 1 | 1 AgCl2 | 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) ZnCl_2 | 1 | -1 | ([ZnCl2])^(-1) ZnNO3 | 1 | 1 | [ZnNO3] AgCl2 | 1 | 1 | [AgCl2] 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) ([ZnCl2])^(-1) [ZnNO3] [AgCl2] = ([ZnNO3] [AgCl2])/([AgNO3] [ZnCl2])

Construct the rate of reaction expression for: AgNO_3 + ZnCl_2 ⟶ ZnNO3 + AgCl2 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 + ZnCl_2 ⟶ ZnNO3 + AgCl2 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 ZnCl_2 | 1 | -1 ZnNO3 | 1 | 1 AgCl2 | 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) ZnCl_2 | 1 | -1 | -(Δ[ZnCl2])/(Δt) ZnNO3 | 1 | 1 | (Δ[ZnNO3])/(Δt) AgCl2 | 1 | 1 | (Δ[AgCl2])/(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[ZnCl2])/(Δt) = (Δ[ZnNO3])/(Δt) = (Δ[AgCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| silver nitrate | zinc chloride | ZnNO3 | AgCl2 formula | AgNO_3 | ZnCl_2 | ZnNO3 | AgCl2 Hill formula | AgNO_3 | Cl_2Zn | NO3Zn | AgCl2 name | silver nitrate | zinc chloride | | IUPAC name | silver nitrate | zinc dichloride | |

| silver nitrate | zinc chloride | ZnNO3 | AgCl2 molar mass | 169.87 g/mol | 136.3 g/mol | 127.4 g/mol | 178.8 g/mol phase | solid (at STP) | solid (at STP) | | melting point | 212 °C | 293 °C | | solubility in water | soluble | soluble | | odor | odorless | odorless | |