AgNO3 + ZnCl2 = Zn(NO3)2 + AgCl

AgNO_3 (silver nitrate) + ZnCl_2 (zinc chloride) ⟶ Zn(NO3)2 + AgCl (silver chloride)

Balance the chemical equation algebraically: AgNO_3 + ZnCl_2 ⟶ Zn(NO3)2 + AgCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 ZnCl_2 ⟶ c_3 Zn(NO3)2 + c_4 AgCl 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 = 2 c_3 O: | 3 c_1 = 6 c_3 Cl: | 2 c_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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 AgNO_3 + ZnCl_2 ⟶ Zn(NO3)2 + 2 AgCl

+ ⟶ Zn(NO3)2 +

silver nitrate + zinc chloride ⟶ Zn(NO3)2 + silver chloride

Construct the equilibrium constant, K, expression for: AgNO_3 + ZnCl_2 ⟶ Zn(NO3)2 + AgCl 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: 2 AgNO_3 + ZnCl_2 ⟶ Zn(NO3)2 + 2 AgCl 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 | 2 | -2 ZnCl_2 | 1 | -1 Zn(NO3)2 | 1 | 1 AgCl | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression AgNO_3 | 2 | -2 | ([AgNO3])^(-2) ZnCl_2 | 1 | -1 | ([ZnCl2])^(-1) Zn(NO3)2 | 1 | 1 | [Zn(NO3)2] AgCl | 2 | 2 | ([AgCl])^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 = ([AgNO3])^(-2) ([ZnCl2])^(-1) [Zn(NO3)2] ([AgCl])^2 = ([Zn(NO3)2] ([AgCl])^2)/(([AgNO3])^2 [ZnCl2])

Construct the rate of reaction expression for: AgNO_3 + ZnCl_2 ⟶ Zn(NO3)2 + AgCl 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: 2 AgNO_3 + ZnCl_2 ⟶ Zn(NO3)2 + 2 AgCl 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 | 2 | -2 ZnCl_2 | 1 | -1 Zn(NO3)2 | 1 | 1 AgCl | 2 | 2 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 | 2 | -2 | -1/2 (Δ[AgNO3])/(Δt) ZnCl_2 | 1 | -1 | -(Δ[ZnCl2])/(Δt) Zn(NO3)2 | 1 | 1 | (Δ[Zn(NO3)2])/(Δt) AgCl | 2 | 2 | 1/2 (Δ[AgCl])/(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 = -1/2 (Δ[AgNO3])/(Δt) = -(Δ[ZnCl2])/(Δt) = (Δ[Zn(NO3)2])/(Δt) = 1/2 (Δ[AgCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| silver nitrate | zinc chloride | Zn(NO3)2 | silver chloride formula | AgNO_3 | ZnCl_2 | Zn(NO3)2 | AgCl Hill formula | AgNO_3 | Cl_2Zn | N2O6Zn | AgCl name | silver nitrate | zinc chloride | | silver chloride IUPAC name | silver nitrate | zinc dichloride | | chlorosilver

| silver nitrate | zinc chloride | Zn(NO3)2 | silver chloride molar mass | 169.87 g/mol | 136.3 g/mol | 189.4 g/mol | 143.32 g/mol phase | solid (at STP) | solid (at STP) | | solid (at STP) melting point | 212 °C | 293 °C | | 455 °C boiling point | | | | 1554 °C density | | | | 5.56 g/cm^3 solubility in water | soluble | soluble | | odor | odorless | odorless | |