Au(NO3)3 = O2 + N2 + Au

Au(NO3)3 ⟶ O_2 oxygen + N_2 nitrogen + Au gold

Balance the chemical equation algebraically: Au(NO3)3 ⟶ O_2 + N_2 + Au Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Au(NO3)3 ⟶ c_2 O_2 + c_3 N_2 + c_4 Au Set the number of atoms in the reactants equal to the number of atoms in the products for Au, N and O: Au: | c_1 = c_4 N: | 3 c_1 = 2 c_3 O: | 9 c_1 = 2 c_2 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 = 9/2 c_3 = 3/2 c_4 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 2 c_2 = 9 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Au(NO3)3 ⟶ 9 O_2 + 3 N_2 + 2 Au

Au(NO3)3 ⟶ + +

Au(NO3)3 ⟶ oxygen + nitrogen + gold

Construct the equilibrium constant, K, expression for: Au(NO3)3 ⟶ O_2 + N_2 + Au 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 Au(NO3)3 ⟶ 9 O_2 + 3 N_2 + 2 Au 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 Au(NO3)3 | 2 | -2 O_2 | 9 | 9 N_2 | 3 | 3 Au | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Au(NO3)3 | 2 | -2 | ([Au(NO3)3])^(-2) O_2 | 9 | 9 | ([O2])^9 N_2 | 3 | 3 | ([N2])^3 Au | 2 | 2 | ([Au])^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 = ([Au(NO3)3])^(-2) ([O2])^9 ([N2])^3 ([Au])^2 = (([O2])^9 ([N2])^3 ([Au])^2)/([Au(NO3)3])^2

Construct the rate of reaction expression for: Au(NO3)3 ⟶ O_2 + N_2 + Au 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 Au(NO3)3 ⟶ 9 O_2 + 3 N_2 + 2 Au 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 Au(NO3)3 | 2 | -2 O_2 | 9 | 9 N_2 | 3 | 3 Au | 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 Au(NO3)3 | 2 | -2 | -1/2 (Δ[Au(NO3)3])/(Δt) O_2 | 9 | 9 | 1/9 (Δ[O2])/(Δt) N_2 | 3 | 3 | 1/3 (Δ[N2])/(Δt) Au | 2 | 2 | 1/2 (Δ[Au])/(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[Au(NO3)3])/(Δt) = 1/9 (Δ[O2])/(Δt) = 1/3 (Δ[N2])/(Δt) = 1/2 (Δ[Au])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| Au(NO3)3 | oxygen | nitrogen | gold formula | Au(NO3)3 | O_2 | N_2 | Au Hill formula | AuN3O9 | O_2 | N_2 | Au name | | oxygen | nitrogen | gold IUPAC name | | molecular oxygen | molecular nitrogen | gold

| Au(NO3)3 | oxygen | nitrogen | gold molar mass | 382.98 g/mol | 31.998 g/mol | 28.014 g/mol | 196.966569 g/mol phase | | gas (at STP) | gas (at STP) | solid (at STP) melting point | | -218 °C | -210 °C | 1063 °C boiling point | | -183 °C | -195.79 °C | 2856 °C density | | 0.001429 g/cm^3 (at 0 °C) | 0.001251 g/cm^3 (at 0 °C) | 19.3 g/cm^3 solubility in water | | | insoluble | insoluble surface tension | | 0.01347 N/m | 0.0066 N/m | dynamic viscosity | | 2.055×10^-5 Pa s (at 25 °C) | 1.78×10^-5 Pa s (at 25 °C) | odor | | odorless | odorless |