Moles of C2H6 formed = moles of C2H4 used
Mass of C2H6 = 12.1 kg = 12100 g
Molar mass of C2H6 = 30.07 g/mol
So, moles of C2H6 = 12100/30.07 mol
So, heat released = 12100x131/30.07 = 52714 kJ
If that doesn't work, try 52837
Comment if any problem
PLEASE HELP Question 8 1 pts Hydrogenation reactions, in which H2 and an "unsaturated" organic compound...
Organic hydrogenation reactions, in which H2 and an "unsaturated" organic compound combine, are used in the food, fuel, and polymer industries. In the simplest case, ethene (C2H4) and H2 form ethane (C2H6). If 161 kJ is given off per mole of C2H4 reacting, how much heat is released when 15.9 kg of C2H6 forms? kJ 4sf
Using the Heat of Reaction (Hrxn) to Find Amounts Organic hydrogenation reactions, in which H2 and an "unsaturated" organic compound combine, are used in the food, fuel, and polymer industries. In the simplest case, ethene (C2H4) and H2 form ethane (C2H6). If 163 kJ is given off per mole of C2H4 reacting, how much heat is released when 14.9 kg of C2H6 forms? kJ?