Ca(NO3)2 = O2 + Ca(NO2)2

Ca(NO_3)_2 calcium nitrate ⟶ O_2 oxygen + Ca(NO_2)_2 calcium nitrite

Balance the chemical equation algebraically: Ca(NO_3)_2 ⟶ O_2 + Ca(NO_2)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca(NO_3)_2 ⟶ c_2 O_2 + c_3 Ca(NO_2)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, N and O: Ca: | c_1 = c_3 N: | 2 c_1 = 2 c_3 O: | 6 c_1 = 2 c_2 + 4 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: | | Ca(NO_3)_2 ⟶ O_2 + Ca(NO_2)_2

⟶ +

calcium nitrate ⟶ oxygen + calcium nitrite

Construct the equilibrium constant, K, expression for: Ca(NO_3)_2 ⟶ O_2 + Ca(NO_2)_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: Ca(NO_3)_2 ⟶ O_2 + Ca(NO_2)_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 Ca(NO_3)_2 | 1 | -1 O_2 | 1 | 1 Ca(NO_2)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ca(NO_3)_2 | 1 | -1 | ([Ca(NO3)2])^(-1) O_2 | 1 | 1 | [O2] Ca(NO_2)_2 | 1 | 1 | [Ca(NO2)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 = ([Ca(NO3)2])^(-1) [O2] [Ca(NO2)2] = ([O2] [Ca(NO2)2])/([Ca(NO3)2])

Construct the rate of reaction expression for: Ca(NO_3)_2 ⟶ O_2 + Ca(NO_2)_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: Ca(NO_3)_2 ⟶ O_2 + Ca(NO_2)_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 Ca(NO_3)_2 | 1 | -1 O_2 | 1 | 1 Ca(NO_2)_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 Ca(NO_3)_2 | 1 | -1 | -(Δ[Ca(NO3)2])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) Ca(NO_2)_2 | 1 | 1 | (Δ[Ca(NO2)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 = -(Δ[Ca(NO3)2])/(Δt) = (Δ[O2])/(Δt) = (Δ[Ca(NO2)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| calcium nitrate | oxygen | calcium nitrite formula | Ca(NO_3)_2 | O_2 | Ca(NO_2)_2 Hill formula | CaN_2O_6 | O_2 | CaN_2O_4 name | calcium nitrate | oxygen | calcium nitrite IUPAC name | calcium dinitrate | molecular oxygen | calcium dinitrite

| calcium nitrate | oxygen | calcium nitrite molar mass | 164.09 g/mol | 31.998 g/mol | 132.09 g/mol phase | solid (at STP) | gas (at STP) | solid (at STP) melting point | 562 °C | -218 °C | 390 °C boiling point | | -183 °C | density | 2.5 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 2.265 g/cm^3 solubility in water | soluble | | very soluble surface tension | | 0.01347 N/m | dynamic viscosity | | 2.055×10^-5 Pa s (at 25 °C) | odor | | odorless |