1. Nitroglycerin, an explosive, decomposes according to the following equation

   4 C₃H₅(NO₃)₃(s) ----> 12 CO₂(g) + 10 H₂O(g) + 6 N₂(g) + 1 O₂(g)

   If the total volume of (all) gases produced is 185 L when collected at 1.43 atm and 311.3 K, calculate

   a) the total moles of gas present (give answer to 5 SFs) = mol

   b) the mass of nitroglycerin (molar mass = 227.1 g/mol) that would have reacted (give answer to correct # of SFs) = g

   c) the mole fractions, X, of the following gases AFTER the reaction is complete.

   i) N₂ (X_N2) (give answer as decimal to 3 SFs) =

   ii) O₂ (X_O2) (give answer as decimal to 3 SFs) =

   d) the partial pressures, P, of the following gases AFTER the reaction is over.

   i) CO₂ (P_CO2) = atm

   ii) H₂O (P_H2O) = = atm