The volume of a tank of propane, C3H8 filled to a pressure of 150 atm at 25 degr

Question

The volume of a tank of propane, C3H8 filled to a pressure of 150 atm at 25 degrees Celcius is 14.0 L. How much heat is available when all of the propane burns?

C3H8(g) + 13/2 (g) --> 3CO2(g) + 4H2O (l)

H = .2220kJ

The correct answer is 1.91 x 10^5 kJ.

For this question I would please like an explaination of how to do this and on top of that 2 other example questions that you explain. So to clarify this question and two more that you either find or come up with the explaination for all three.

Explanation / Answer

This is a two part question. First, you need to find the moles of propane in the tank.

PV = nRT. Make sure you convert the temperature to Kelvin, and use 0.08206 as the gas constant.
n=85.8759
Once you know how many moles are in the tank, you just multiply that number by the molar enthalpy change (delta H).

=85.8759*2220k=190644.498 k J= 1.9*10^5 k J

given H =- 0.2220kJ but it actually is H =- 2220kJ

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