Cu + Pd(NO3)2 = Cu(NO3)2 + Pd

Cu copper + Pd(NO3)2 ⟶ Cu(NO_3)_2 copper(II) nitrate + Pd palladium

Balance the chemical equation algebraically: Cu + Pd(NO3)2 ⟶ Cu(NO_3)_2 + Pd Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cu + c_2 Pd(NO3)2 ⟶ c_3 Cu(NO_3)_2 + c_4 Pd Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, Pd, N and O: Cu: | c_1 = c_3 Pd: | c_2 = c_4 N: | 2 c_2 = 2 c_3 O: | 6 c_2 = 6 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: | | Cu + Pd(NO3)2 ⟶ Cu(NO_3)_2 + Pd

+ Pd(NO3)2 ⟶ +

copper + Pd(NO3)2 ⟶ copper(II) nitrate + palladium

Construct the equilibrium constant, K, expression for: Cu + Pd(NO3)2 ⟶ Cu(NO_3)_2 + Pd 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: Cu + Pd(NO3)2 ⟶ Cu(NO_3)_2 + Pd 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 Cu | 1 | -1 Pd(NO3)2 | 1 | -1 Cu(NO_3)_2 | 1 | 1 Pd | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cu | 1 | -1 | ([Cu])^(-1) Pd(NO3)2 | 1 | -1 | ([Pd(NO3)2])^(-1) Cu(NO_3)_2 | 1 | 1 | [Cu(NO3)2] Pd | 1 | 1 | [Pd] 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 = ([Cu])^(-1) ([Pd(NO3)2])^(-1) [Cu(NO3)2] [Pd] = ([Cu(NO3)2] [Pd])/([Cu] [Pd(NO3)2])

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

| copper | Pd(NO3)2 | copper(II) nitrate | palladium formula | Cu | Pd(NO3)2 | Cu(NO_3)_2 | Pd Hill formula | Cu | N2O6Pd | CuN_2O_6 | Pd name | copper | | copper(II) nitrate | palladium

| copper | Pd(NO3)2 | copper(II) nitrate | palladium molar mass | 63.546 g/mol | 230.43 g/mol | 187.55 g/mol | 106.42 g/mol phase | solid (at STP) | | | solid (at STP) melting point | 1083 °C | | | 1554 °C boiling point | 2567 °C | | | 2970 °C density | 8.96 g/cm^3 | | | 12.023 g/cm^3 solubility in water | insoluble | | | insoluble odor | odorless | | |