Ag + CuNO3 = CuAgNO3

Ag silver + CuNO3 ⟶ CuAgNO3

Balance the chemical equation algebraically: Ag + CuNO3 ⟶ CuAgNO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ag + c_2 CuNO3 ⟶ c_3 CuAgNO3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, Cu, N and O: Ag: | c_1 = c_3 Cu: | c_2 = c_3 N: | c_2 = c_3 O: | 3 c_2 = 3 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Ag + CuNO3 ⟶ CuAgNO3

+ CuNO3 ⟶ CuAgNO3

silver + CuNO3 ⟶ CuAgNO3

Construct the equilibrium constant, K, expression for: Ag + CuNO3 ⟶ CuAgNO3 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: Ag + CuNO3 ⟶ CuAgNO3 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 Ag | 1 | -1 CuNO3 | 1 | -1 CuAgNO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ag | 1 | -1 | ([Ag])^(-1) CuNO3 | 1 | -1 | ([CuNO3])^(-1) CuAgNO3 | 1 | 1 | [CuAgNO3] 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 = ([Ag])^(-1) ([CuNO3])^(-1) [CuAgNO3] = ([CuAgNO3])/([Ag] [CuNO3])

Construct the rate of reaction expression for: Ag + CuNO3 ⟶ CuAgNO3 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: Ag + CuNO3 ⟶ CuAgNO3 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 Ag | 1 | -1 CuNO3 | 1 | -1 CuAgNO3 | 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 Ag | 1 | -1 | -(Δ[Ag])/(Δt) CuNO3 | 1 | -1 | -(Δ[CuNO3])/(Δt) CuAgNO3 | 1 | 1 | (Δ[CuAgNO3])/(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[Ag])/(Δt) = -(Δ[CuNO3])/(Δt) = (Δ[CuAgNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| silver | CuNO3 | CuAgNO3 formula | Ag | CuNO3 | CuAgNO3 Hill formula | Ag | CuNO3 | AgCuNO3 name | silver | |

| silver | CuNO3 | CuAgNO3 molar mass | 107.8682 g/mol | 125.55 g/mol | 233.42 g/mol phase | solid (at STP) | | melting point | 960 °C | | boiling point | 2212 °C | | density | 10.49 g/cm^3 | | solubility in water | insoluble | |