NH4NO3 = H2O + O2 + N2

ammonium nitrate ⟶ water + oxygen + nitrogen

Balance the chemical equation algebraically: ⟶ + + Add stoichiometric coefficients, c_i, to the reactants and products: c_1 ⟶ c_2 + c_3 + c_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N and O: H: | 4 c_1 = 2 c_2 N: | 2 c_1 = 2 c_4 O: | 3 c_1 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 4 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 ⟶ 4 + + 2

⟶ + +

ammonium nitrate ⟶ water + oxygen + nitrogen

| ammonium nitrate | water | oxygen | nitrogen molecular free energy | -183.9 kJ/mol | -237.1 kJ/mol | 231.7 kJ/mol | 0 kJ/mol total free energy | -367.8 kJ/mol | -948.4 kJ/mol | 231.7 kJ/mol | 0 kJ/mol | G_initial = -367.8 kJ/mol | G_final = -716.7 kJ/mol | | ΔG_rxn^0 | -716.7 kJ/mol - -367.8 kJ/mol = -348.9 kJ/mol (exergonic) | | |

| ammonium nitrate | water | oxygen | nitrogen Hill formula | H_4N_2O_3 | H_2O | O_2 | N_2 name | ammonium nitrate | water | oxygen | nitrogen IUPAC name | | water | molecular oxygen | molecular nitrogen

| ammonium nitrate | water | oxygen | nitrogen molar mass | 80.04 g/mol | 18.015 g/mol | 31.998 g/mol | 28.014 g/mol phase | solid (at STP) | liquid (at STP) | gas (at STP) | gas (at STP) melting point | 169 °C | 0 °C | -218 °C | -210 °C boiling point | 210 °C | 99.9839 °C | -183 °C | -195.79 °C density | 1.73 g/cm^3 | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 0.001251 g/cm^3 (at 0 °C) solubility in water | | | | insoluble surface tension | | 0.0728 N/m | 0.01347 N/m | 0.0066 N/m dynamic viscosity | | 8.9×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | 1.78×10^-5 Pa s (at 25 °C) odor | odorless | odorless | odorless | odorless