Input interpretation
oxygen + methylamine ⟶ water + carbon dioxide + nitrogen
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 Set the number of atoms in the reactants equal to the number of atoms in the products for O, C, H and N: O: | 2 c_1 = c_3 + 2 c_4 C: | c_2 = c_4 H: | 5 c_2 = 2 c_3 N: | c_2 = 2 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 9/2 c_2 = 2 c_3 = 5 c_4 = 2 c_5 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 9 c_2 = 4 c_3 = 10 c_4 = 4 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 9 + 4 ⟶ 10 + 4 + 2
Structures
+ ⟶ + +
Names
oxygen + methylamine ⟶ water + carbon dioxide + nitrogen
Reaction thermodynamics
Enthalpy
| oxygen | methylamine | water | carbon dioxide | nitrogen molecular enthalpy | 0 kJ/mol | -22.5 kJ/mol | -285.8 kJ/mol | -393.5 kJ/mol | 0 kJ/mol total enthalpy | 0 kJ/mol | -90 kJ/mol | -2858 kJ/mol | -1574 kJ/mol | 0 kJ/mol | H_initial = -90 kJ/mol | | H_final = -4432 kJ/mol | | ΔH_rxn^0 | -4432 kJ/mol - -90 kJ/mol = -4342 kJ/mol (exothermic) | | | |
Chemical names and formulas
| oxygen | methylamine | water | carbon dioxide | nitrogen Hill formula | O_2 | CH_5N | H_2O | CO_2 | N_2 name | oxygen | methylamine | water | carbon dioxide | nitrogen IUPAC name | molecular oxygen | methanamine | water | carbon dioxide | molecular nitrogen