4kmol methane (ch4) is burned completely with the stoichiometric amount of air during a steady-flow combustion process. if both the reactants and the products are maintained at 25°c and 1 atm and the water in the products exists in the liquid form, determine the heat transfer from the combustion chamber during this process. what would your answer be if combustion were achieved with 100 percent excess air?

Heat transfer = 3564 Jolues

The same value

Explanation:

The heat of combustion is the heat released per 1 mole of substunce experimenting the combustion at standard conditions of pressure and temperature ( 1 atm, 298 K):

Qtransfer = - mol x ΔHºc Qtransfer

So look up in appropiate reference table ΔHºc  and solve the problem:

ΔHºc  = - 891 kJ/mol

Qtransfer = - (4 x 10³ mol x  -891 kJ/mol ) = 3564 J

if the combustion were achieved with 100 % excess air, the result will still be the same. As long as the standard conditions are maintained, the heat of combustion remains constant. In fact in many cases the combustion is performed under excess oxygen to ensure complete combustion.

specific gravity is the density of a substance divided by the density of water. since (at standard temperature and pressure) water has a density of 1 gram/cm3, and since all of the units cancel, specific gravity is usually very close to the same value as density

so "c" is the answer

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