How many liters of ethane, C 2 H 6 at 25 C and 725 mmHg are needed to evolve the

Question

How many liters of ethane, C2H6 at 25 C and 725 mmHg are needed to evolve the same quantity of energy when the ethane is burned in oxygen to CO2(g) and H2O(g)?

(We are to use Table 20.3 and Appendix C for data) (This is from the 10th Edition of General Chemistry from Ebbing and Gammon. Table 20.3 is just a table of the masses of particles and some elements. The Appendix C is the thermodynamic quanitities for substances and ions at 25 C. You may use whatever data you have on These, but please indicate what they are so I may follow the outline for the problem.)

Explanation / Answer

The standard enthalpy of conbustion for ethane is -1560 kJ/mol

moles of ethane needed = 1 mol

Volume of ethane needed = nRT/P

with,

n = 1

R = gas constant

T = 25 + 273 = 298 K

P = 725/760 = 0.954 atm

we get,

Volume of ethane needed = 1 x 0.08205 x 298/0.954

                                          = 25.63 L

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