AgNO3 + Ni = Ag + Ni(NO3)2

AgNO_3 silver nitrate + Ni nickel ⟶ Ag silver + Ni(NO_3)_2 nickel(II) nitrate

Balance the chemical equation algebraically: AgNO_3 + Ni ⟶ Ag + Ni(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 Ni ⟶ c_3 Ag + c_4 Ni(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O and Ni: Ag: | c_1 = c_3 N: | c_1 = 2 c_4 O: | 3 c_1 = 6 c_4 Ni: | c_2 = 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 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 AgNO_3 + Ni ⟶ 2 Ag + Ni(NO_3)_2

+ ⟶ +

silver nitrate + nickel ⟶ silver + nickel(II) nitrate

Construct the equilibrium constant, K, expression for: AgNO_3 + Ni ⟶ Ag + Ni(NO_3)_2 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 + Ni ⟶ 2 Ag + Ni(NO_3)_2 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 Ni | 1 | -1 Ag | 2 | 2 Ni(NO_3)_2 | 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 | 2 | -2 | ([AgNO3])^(-2) Ni | 1 | -1 | ([Ni])^(-1) Ag | 2 | 2 | ([Ag])^2 Ni(NO_3)_2 | 1 | 1 | [Ni(NO3)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) ([Ni])^(-1) ([Ag])^2 [Ni(NO3)2] = (([Ag])^2 [Ni(NO3)2])/(([AgNO3])^2 [Ni])

Construct the rate of reaction expression for: AgNO_3 + Ni ⟶ Ag + Ni(NO_3)_2 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 + Ni ⟶ 2 Ag + Ni(NO_3)_2 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 Ni | 1 | -1 Ag | 2 | 2 Ni(NO_3)_2 | 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 | 2 | -2 | -1/2 (Δ[AgNO3])/(Δt) Ni | 1 | -1 | -(Δ[Ni])/(Δt) Ag | 2 | 2 | 1/2 (Δ[Ag])/(Δt) Ni(NO_3)_2 | 1 | 1 | (Δ[Ni(NO3)2])/(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[Ni])/(Δt) = 1/2 (Δ[Ag])/(Δt) = (Δ[Ni(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| silver nitrate | nickel | silver | nickel(II) nitrate formula | AgNO_3 | Ni | Ag | Ni(NO_3)_2 Hill formula | AgNO_3 | Ni | Ag | N_2NiO_6 name | silver nitrate | nickel | silver | nickel(II) nitrate IUPAC name | silver nitrate | nickel | silver | nickel(+2) dinitrate

| silver nitrate | nickel | silver | nickel(II) nitrate molar mass | 169.87 g/mol | 58.6934 g/mol | 107.8682 g/mol | 182.7 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 212 °C | 1453 °C | 960 °C | 57 °C boiling point | | 2732 °C | 2212 °C | 137 °C density | | 8.908 g/cm^3 | 10.49 g/cm^3 | 1.77 g/cm^3 solubility in water | soluble | insoluble | insoluble | odor | odorless | odorless | |