Al + NaNO3 = Na + Al(NO3)3

Al aluminum + NaNO_3 sodium nitrate ⟶ Na sodium + Al(NO_3)_3 aluminum nitrate

Balance the chemical equation algebraically: Al + NaNO_3 ⟶ Na + Al(NO_3)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Al + c_2 NaNO_3 ⟶ c_3 Na + c_4 Al(NO_3)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Al, N, Na and O: Al: | c_1 = c_4 N: | c_2 = 3 c_4 Na: | c_2 = c_3 O: | 3 c_2 = 9 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 3 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Al + 3 NaNO_3 ⟶ 3 Na + Al(NO_3)_3

+ ⟶ +

aluminum + sodium nitrate ⟶ sodium + aluminum nitrate

Construct the equilibrium constant, K, expression for: Al + NaNO_3 ⟶ Na + Al(NO_3)_3 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: Al + 3 NaNO_3 ⟶ 3 Na + Al(NO_3)_3 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 Al | 1 | -1 NaNO_3 | 3 | -3 Na | 3 | 3 Al(NO_3)_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Al | 1 | -1 | ([Al])^(-1) NaNO_3 | 3 | -3 | ([NaNO3])^(-3) Na | 3 | 3 | ([Na])^3 Al(NO_3)_3 | 1 | 1 | [Al(NO3)3] 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 = ([Al])^(-1) ([NaNO3])^(-3) ([Na])^3 [Al(NO3)3] = (([Na])^3 [Al(NO3)3])/([Al] ([NaNO3])^3)

Construct the rate of reaction expression for: Al + NaNO_3 ⟶ Na + Al(NO_3)_3 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: Al + 3 NaNO_3 ⟶ 3 Na + Al(NO_3)_3 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 Al | 1 | -1 NaNO_3 | 3 | -3 Na | 3 | 3 Al(NO_3)_3 | 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 Al | 1 | -1 | -(Δ[Al])/(Δt) NaNO_3 | 3 | -3 | -1/3 (Δ[NaNO3])/(Δt) Na | 3 | 3 | 1/3 (Δ[Na])/(Δt) Al(NO_3)_3 | 1 | 1 | (Δ[Al(NO3)3])/(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[Al])/(Δt) = -1/3 (Δ[NaNO3])/(Δt) = 1/3 (Δ[Na])/(Δt) = (Δ[Al(NO3)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| aluminum | sodium nitrate | sodium | aluminum nitrate formula | Al | NaNO_3 | Na | Al(NO_3)_3 Hill formula | Al | NNaO_3 | Na | AlN_3O_9 name | aluminum | sodium nitrate | sodium | aluminum nitrate IUPAC name | aluminum | sodium nitrate | sodium | aluminum(+3) cation trinitrate

| aluminum | sodium nitrate | sodium | aluminum nitrate molar mass | 26.9815385 g/mol | 84.994 g/mol | 22.98976928 g/mol | 212.99 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 660.4 °C | 306 °C | 97.8 °C | 72.8 °C boiling point | 2460 °C | | 883 °C | density | 2.7 g/cm^3 | 2.26 g/cm^3 | 0.968 g/cm^3 | 1.401 g/cm^3 solubility in water | insoluble | soluble | decomposes | surface tension | 0.817 N/m | | | dynamic viscosity | 1.5×10^-4 Pa s (at 760 °C) | 0.003 Pa s (at 250 °C) | 1.413×10^-5 Pa s (at 527 °C) | 0.001338 Pa s (at 22 °C) odor | odorless | | |