H2 + NaCl = HCl + Na

H_2 hydrogen + NaCl sodium chloride ⟶ HCl hydrogen chloride + Na sodium

Balance the chemical equation algebraically: H_2 + NaCl ⟶ HCl + Na Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2 + c_2 NaCl ⟶ c_3 HCl + c_4 Na Set the number of atoms in the reactants equal to the number of atoms in the products for H, Cl and Na: H: | 2 c_1 = c_3 Cl: | c_2 = c_3 Na: | c_2 = 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 = 2 c_3 = 2 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2 + 2 NaCl ⟶ 2 HCl + 2 Na

+ ⟶ +

hydrogen + sodium chloride ⟶ hydrogen chloride + sodium

| hydrogen | sodium chloride | hydrogen chloride | sodium molecular enthalpy | 0 kJ/mol | -411.2 kJ/mol | -92.3 kJ/mol | 0 kJ/mol total enthalpy | 0 kJ/mol | -822.4 kJ/mol | -184.6 kJ/mol | 0 kJ/mol | H_initial = -822.4 kJ/mol | | H_final = -184.6 kJ/mol | ΔH_rxn^0 | -184.6 kJ/mol - -822.4 kJ/mol = 637.8 kJ/mol (endothermic) | | |

| hydrogen | sodium chloride | hydrogen chloride | sodium molecular entropy | 115 J/(mol K) | 72 J/(mol K) | 187 J/(mol K) | 51 J/(mol K) total entropy | 115 J/(mol K) | 144 J/(mol K) | 374 J/(mol K) | 102 J/(mol K) | S_initial = 259 J/(mol K) | | S_final = 476 J/(mol K) | ΔS_rxn^0 | 476 J/(mol K) - 259 J/(mol K) = 217 J/(mol K) (endoentropic) | | |

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

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

| hydrogen | sodium chloride | hydrogen chloride | sodium formula | H_2 | NaCl | HCl | Na Hill formula | H_2 | ClNa | ClH | Na name | hydrogen | sodium chloride | hydrogen chloride | sodium IUPAC name | molecular hydrogen | sodium chloride | hydrogen chloride | sodium

| hydrogen | sodium chloride | hydrogen chloride | sodium molar mass | 2.016 g/mol | 58.44 g/mol | 36.46 g/mol | 22.98976928 g/mol phase | gas (at STP) | solid (at STP) | gas (at STP) | solid (at STP) melting point | -259.2 °C | 801 °C | -114.17 °C | 97.8 °C boiling point | -252.8 °C | 1413 °C | -85 °C | 883 °C density | 8.99×10^-5 g/cm^3 (at 0 °C) | 2.16 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 0.968 g/cm^3 solubility in water | | soluble | miscible | decomposes dynamic viscosity | 8.9×10^-6 Pa s (at 25 °C) | | | 1.413×10^-5 Pa s (at 527 °C) odor | odorless | odorless | |