Zn(NO3)2 = O2 + NO2 + ZnO

Zn(NO3)2 ⟶ oxygen + nitrogen dioxide + zinc oxide

Balance the chemical equation algebraically: Zn(NO3)2 ⟶ + + Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Zn(NO3)2 ⟶ c_2 + c_3 + c_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Zn, N and O: Zn: | c_1 = c_4 N: | 2 c_1 = c_3 O: | 6 c_1 = 2 c_2 + 2 c_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 = 4 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Zn(NO3)2 ⟶ + 4 + 2

Zn(NO3)2 ⟶ + +

Zn(NO3)2 ⟶ oxygen + nitrogen dioxide + zinc oxide

K_c = ([O2] [NO2]^4 [ZnO]^2)/[Zn(NO3)2]^2

rate = -1/2 (Δ[Zn(NO3)2])/(Δt) = (Δ[O2])/(Δt) = 1/4 (Δ[NO2])/(Δt) = 1/2 (Δ[ZnO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| Zn(NO3)2 | oxygen | nitrogen dioxide | zinc oxide formula | Zn(NO3)2 | | | Hill formula | N2O6Zn | O_2 | NO_2 | OZn name | | oxygen | nitrogen dioxide | zinc oxide IUPAC name | | molecular oxygen | Nitrogen dioxide | oxozinc

| Zn(NO3)2 | oxygen | nitrogen dioxide | zinc oxide molar mass | 189.4 g/mol | 31.998 g/mol | 46.005 g/mol | 81.38 g/mol phase | | gas (at STP) | gas (at STP) | solid (at STP) melting point | | -218 °C | -11 °C | 1975 °C boiling point | | -183 °C | 21 °C | 2360 °C density | | 0.001429 g/cm^3 (at 0 °C) | 0.00188 g/cm^3 (at 25 °C) | 5.6 g/cm^3 solubility in water | | | reacts | surface tension | | 0.01347 N/m | | dynamic viscosity | | 2.055×10^-5 Pa s (at 25 °C) | 4.02×10^-4 Pa s (at 25 °C) | odor | | odorless | | odorless