Question: Calculate the volume of all gases evolved by the complete oxidation of 0.370g of the amino acid alanine, C3H7NO2 if the products are liquid water, nitrogen gas, and carbon dioxide gas; the total pressure is 1.00 atm; and T= 298K .
Since we are given the amount of alanine, 0.370 g, I know that we are going to use mole to mole ratio to solve for the moles of N2 and CO2. But I am unable to come up with the moles of each gas because I am unable to balance the chemical reaction: C3H7NO2 --> H2O(l) + N2(g) + CO2(g). If I find the moles of each gas, then I know to use the ideal gas law and solve for V, which will be the answer. Any help is appreciated.