NaOH + Na = H2 + Na2O

NaOH sodium hydroxide + Na sodium ⟶ H_2 hydrogen + Na_2O sodium oxide

Balance the chemical equation algebraically: NaOH + Na ⟶ H_2 + Na_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 Na ⟶ c_3 H_2 + c_4 Na_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na and O: H: | c_1 = 2 c_3 Na: | c_1 + c_2 = 2 c_4 O: | c_1 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NaOH + 2 Na ⟶ H_2 + 2 Na_2O

+ ⟶ +

sodium hydroxide + sodium ⟶ hydrogen + sodium oxide

Construct the equilibrium constant, K, expression for: NaOH + Na ⟶ H_2 + Na_2O 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 NaOH + 2 Na ⟶ H_2 + 2 Na_2O 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 NaOH | 2 | -2 Na | 2 | -2 H_2 | 1 | 1 Na_2O | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 2 | -2 | ([NaOH])^(-2) Na | 2 | -2 | ([Na])^(-2) H_2 | 1 | 1 | [H2] Na_2O | 2 | 2 | ([Na2O])^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 = ([NaOH])^(-2) ([Na])^(-2) [H2] ([Na2O])^2 = ([H2] ([Na2O])^2)/(([NaOH])^2 ([Na])^2)

Construct the rate of reaction expression for: NaOH + Na ⟶ H_2 + Na_2O 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 NaOH + 2 Na ⟶ H_2 + 2 Na_2O 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 NaOH | 2 | -2 Na | 2 | -2 H_2 | 1 | 1 Na_2O | 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 NaOH | 2 | -2 | -1/2 (Δ[NaOH])/(Δt) Na | 2 | -2 | -1/2 (Δ[Na])/(Δt) H_2 | 1 | 1 | (Δ[H2])/(Δt) Na_2O | 2 | 2 | 1/2 (Δ[Na2O])/(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[NaOH])/(Δt) = -1/2 (Δ[Na])/(Δt) = (Δ[H2])/(Δt) = 1/2 (Δ[Na2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sodium hydroxide | sodium | hydrogen | sodium oxide formula | NaOH | Na | H_2 | Na_2O Hill formula | HNaO | Na | H_2 | Na_2O name | sodium hydroxide | sodium | hydrogen | sodium oxide IUPAC name | sodium hydroxide | sodium | molecular hydrogen | disodium oxygen(-2) anion

| sodium hydroxide | sodium | hydrogen | sodium oxide molar mass | 39.997 g/mol | 22.98976928 g/mol | 2.016 g/mol | 61.979 g/mol phase | solid (at STP) | solid (at STP) | gas (at STP) | melting point | 323 °C | 97.8 °C | -259.2 °C | boiling point | 1390 °C | 883 °C | -252.8 °C | density | 2.13 g/cm^3 | 0.968 g/cm^3 | 8.99×10^-5 g/cm^3 (at 0 °C) | 2.27 g/cm^3 solubility in water | soluble | decomposes | | surface tension | 0.07435 N/m | | | dynamic viscosity | 0.004 Pa s (at 350 °C) | 1.413×10^-5 Pa s (at 527 °C) | 8.9×10^-6 Pa s (at 25 °C) | odor | | | odorless |