Input interpretation
water + carbon dioxide + sodium chloride + ammonia ⟶ ammonium chloride + sodium bicarbonate
Balanced equation
Balance the chemical equation algebraically: + + + ⟶ + Add stoichiometric coefficients, c_i, to the reactants and products: c_1 + c_2 + c_3 + c_4 ⟶ c_5 + c_6 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, C, Cl, Na and N: H: | 2 c_1 + 3 c_4 = 4 c_5 + c_6 O: | c_1 + 2 c_2 = 3 c_6 C: | c_2 = c_6 Cl: | c_3 = c_5 Na: | c_3 = c_6 N: | c_4 = c_5 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 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | + + + ⟶ +
Structures
+ + + ⟶ +
Names
water + carbon dioxide + sodium chloride + ammonia ⟶ ammonium chloride + sodium bicarbonate
Reaction thermodynamics
Enthalpy
| water | carbon dioxide | sodium chloride | ammonia | ammonium chloride | sodium bicarbonate molecular enthalpy | -285.8 kJ/mol | -393.5 kJ/mol | -411.2 kJ/mol | -45.9 kJ/mol | -314.4 kJ/mol | -950.8 kJ/mol total enthalpy | -285.8 kJ/mol | -393.5 kJ/mol | -411.2 kJ/mol | -45.9 kJ/mol | -314.4 kJ/mol | -950.8 kJ/mol | H_initial = -1136 kJ/mol | | | | H_final = -1265 kJ/mol | ΔH_rxn^0 | -1265 kJ/mol - -1136 kJ/mol = -128.8 kJ/mol (exothermic) | | | | |
Gibbs free energy
| water | carbon dioxide | sodium chloride | ammonia | ammonium chloride | sodium bicarbonate molecular free energy | -237.1 kJ/mol | -394.4 kJ/mol | -384.1 kJ/mol | -16.4 kJ/mol | -202.9 kJ/mol | -851 kJ/mol total free energy | -237.1 kJ/mol | -394.4 kJ/mol | -384.1 kJ/mol | -16.4 kJ/mol | -202.9 kJ/mol | -851 kJ/mol | G_initial = -1032 kJ/mol | | | | G_final = -1054 kJ/mol | ΔG_rxn^0 | -1054 kJ/mol - -1032 kJ/mol = -21.9 kJ/mol (exergonic) | | | | |
Entropy
| water | carbon dioxide | sodium chloride | ammonia | ammonium chloride | sodium bicarbonate molecular entropy | 69.91 J/(mol K) | 214 J/(mol K) | 72 J/(mol K) | 193 J/(mol K) | 96 J/(mol K) | 102 J/(mol K) total entropy | 69.91 J/(mol K) | 214 J/(mol K) | 72 J/(mol K) | 193 J/(mol K) | 96 J/(mol K) | 102 J/(mol K) | S_initial = 548.9 J/(mol K) | | | | S_final = 198 J/(mol K) | ΔS_rxn^0 | 198 J/(mol K) - 548.9 J/(mol K) = -350.9 J/(mol K) (exoentropic) | | | | |
Equilibrium constant
![K_c = ([NH4Cl] [NaHCO3])/([H2O] [CO2] [NaCl] [NH3])](../image_source/5cbcc9d5e466030f2bea0483c7d62319.png)
K_c = ([NH4Cl] [NaHCO3])/([H2O] [CO2] [NaCl] [NH3])
Rate of reaction
![rate = -(Δ[H2O])/(Δt) = -(Δ[CO2])/(Δt) = -(Δ[NaCl])/(Δt) = -(Δ[NH3])/(Δt) = (Δ[NH4Cl])/(Δt) = (Δ[NaHCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/45daa0d4e1773228da866b9f35bc6e06.png)
rate = -(Δ[H2O])/(Δt) = -(Δ[CO2])/(Δt) = -(Δ[NaCl])/(Δt) = -(Δ[NH3])/(Δt) = (Δ[NH4Cl])/(Δt) = (Δ[NaHCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| water | carbon dioxide | sodium chloride | ammonia | ammonium chloride | sodium bicarbonate Hill formula | H_2O | CO_2 | ClNa | H_3N | ClH_4N | CHNaO_3 name | water | carbon dioxide | sodium chloride | ammonia | ammonium chloride | sodium bicarbonate IUPAC name | water | carbon dioxide | sodium chloride | ammonia | ammonium chloride | sodium hydrogen carbonate