50 g of C16H34 are burned with insufficient oxygen for complete combustion to CO2.
C16H34(s) + 16.5 O2(g) -> 16 CO(g) + 17 H2O(l) and some of the reaction forms CO2 and H2O(l) in the reaction C16H34(s) + 24.5 O2(g) -> 19CO2(g) + 17H2O(l)
(P=1 bar, T=298.15K, heat change = -1945.2 kJ)
1. Compute percent C16H34 that reacted to form CO(g) in the process.
2. If experiment carried out at constant V, how much heat would have been released?
To do this question, you need to calculate the enthalpy change for 50 g C16H34 burning by both reactions.
Find each by using the deltaH (dH) tables provided to you in your textbook and use
dHrxn = [Sum(products)] - ...
This solution computes percent C16H34 and the amount of heat that would have been released.