Zn + AgNO3 = Ag + Zn2NO3

Zn zinc + AgNO_3 silver nitrate ⟶ Ag silver + Zn2NO3

Balance the chemical equation algebraically: Zn + AgNO_3 ⟶ Ag + Zn2NO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Zn + c_2 AgNO_3 ⟶ c_3 Ag + c_4 Zn2NO3 Set the number of atoms in the reactants equal to the number of atoms in the products for Zn, Ag, N and O: Zn: | c_1 = 2 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Zn + AgNO_3 ⟶ Ag + Zn2NO3

+ ⟶ + Zn2NO3

zinc + silver nitrate ⟶ silver + Zn2NO3

Construct the equilibrium constant, K, expression for: Zn + AgNO_3 ⟶ Ag + Zn2NO3 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 Zn + AgNO_3 ⟶ Ag + Zn2NO3 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 Zn | 2 | -2 AgNO_3 | 1 | -1 Ag | 1 | 1 Zn2NO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Zn | 2 | -2 | ([Zn])^(-2) AgNO_3 | 1 | -1 | ([AgNO3])^(-1) Ag | 1 | 1 | [Ag] Zn2NO3 | 1 | 1 | [Zn2NO3] 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 = ([Zn])^(-2) ([AgNO3])^(-1) [Ag] [Zn2NO3] = ([Ag] [Zn2NO3])/(([Zn])^2 [AgNO3])

Construct the rate of reaction expression for: Zn + AgNO_3 ⟶ Ag + Zn2NO3 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 Zn + AgNO_3 ⟶ Ag + Zn2NO3 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 Zn | 2 | -2 AgNO_3 | 1 | -1 Ag | 1 | 1 Zn2NO3 | 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 Zn | 2 | -2 | -1/2 (Δ[Zn])/(Δt) AgNO_3 | 1 | -1 | -(Δ[AgNO3])/(Δt) Ag | 1 | 1 | (Δ[Ag])/(Δt) Zn2NO3 | 1 | 1 | (Δ[Zn2NO3])/(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[Zn])/(Δt) = -(Δ[AgNO3])/(Δt) = (Δ[Ag])/(Δt) = (Δ[Zn2NO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| zinc | silver nitrate | silver | Zn2NO3 formula | Zn | AgNO_3 | Ag | Zn2NO3 Hill formula | Zn | AgNO_3 | Ag | NO3Zn2 name | zinc | silver nitrate | silver |

| zinc | silver nitrate | silver | Zn2NO3 molar mass | 65.38 g/mol | 169.87 g/mol | 107.8682 g/mol | 192.8 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 420 °C | 212 °C | 960 °C | boiling point | 907 °C | | 2212 °C | density | 7.14 g/cm^3 | | 10.49 g/cm^3 | solubility in water | insoluble | soluble | insoluble | odor | odorless | odorless | |