NO2 + Ca(OH)2 = H2O + CaNO3

NO_2 nitrogen dioxide + Ca(OH)_2 calcium hydroxide ⟶ H_2O water + CaNO3

Balance the chemical equation algebraically: NO_2 + Ca(OH)_2 ⟶ H_2O + CaNO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NO_2 + c_2 Ca(OH)_2 ⟶ c_3 H_2O + c_4 CaNO3 Set the number of atoms in the reactants equal to the number of atoms in the products for N, O, Ca and H: N: | c_1 = c_4 O: | 2 c_1 + 2 c_2 = c_3 + 3 c_4 Ca: | c_2 = c_4 H: | 2 c_2 = 2 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: | | NO_2 + Ca(OH)_2 ⟶ H_2O + CaNO3

+ ⟶ + CaNO3

nitrogen dioxide + calcium hydroxide ⟶ water + CaNO3

Construct the equilibrium constant, K, expression for: NO_2 + Ca(OH)_2 ⟶ H_2O + CaNO3 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: NO_2 + Ca(OH)_2 ⟶ H_2O + CaNO3 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 NO_2 | 1 | -1 Ca(OH)_2 | 1 | -1 H_2O | 1 | 1 CaNO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NO_2 | 1 | -1 | ([NO2])^(-1) Ca(OH)_2 | 1 | -1 | ([Ca(OH)2])^(-1) H_2O | 1 | 1 | [H2O] CaNO3 | 1 | 1 | [CaNO3] 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 = ([NO2])^(-1) ([Ca(OH)2])^(-1) [H2O] [CaNO3] = ([H2O] [CaNO3])/([NO2] [Ca(OH)2])

Construct the rate of reaction expression for: NO_2 + Ca(OH)_2 ⟶ H_2O + CaNO3 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: NO_2 + Ca(OH)_2 ⟶ H_2O + CaNO3 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 NO_2 | 1 | -1 Ca(OH)_2 | 1 | -1 H_2O | 1 | 1 CaNO3 | 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 NO_2 | 1 | -1 | -(Δ[NO2])/(Δt) Ca(OH)_2 | 1 | -1 | -(Δ[Ca(OH)2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CaNO3 | 1 | 1 | (Δ[CaNO3])/(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[NO2])/(Δt) = -(Δ[Ca(OH)2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CaNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| nitrogen dioxide | calcium hydroxide | water | CaNO3 formula | NO_2 | Ca(OH)_2 | H_2O | CaNO3 Hill formula | NO_2 | CaH_2O_2 | H_2O | CaNO3 name | nitrogen dioxide | calcium hydroxide | water | IUPAC name | Nitrogen dioxide | calcium dihydroxide | water |

| nitrogen dioxide | calcium hydroxide | water | CaNO3 molar mass | 46.005 g/mol | 74.092 g/mol | 18.015 g/mol | 102.08 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | melting point | -11 °C | 550 °C | 0 °C | boiling point | 21 °C | | 99.9839 °C | density | 0.00188 g/cm^3 (at 25 °C) | 2.24 g/cm^3 | 1 g/cm^3 | solubility in water | reacts | slightly soluble | | surface tension | | | 0.0728 N/m | dynamic viscosity | 4.02×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | | odorless | odorless |